CHEM-10055 ch1-3 Flashcards

What is the molarity or concentration (M or C) ___of a solution prepared by dissolving 10.8 g of MgCl₂ in water to form 750.0 mL of the solution?

(a) 1.44 x10^-2 mol/L (b) 1.13 x10^-1 mol/L (c) 1.51 x10^-1 mol/L

(d) 69.4 mol/L(e) 1.51 x10^-4 mol/L

A solution is prepared by dissolving 10.0 g ethanol in 30.0 g of water. What is the percent (%) by mass concentration of ethanol in this solution?

(a) 25.0%(b) 33.3%(c) 0.25%(d) 0.333%

(e) 3.00 x10²%

A solution is prepared by dissolving 15.5 mL of methanol in 34.5 mL of ethanol. What is the percent (%) by volume concentration of methanol in this solution?

(a) 44.9% (b) 31.0% (c) 2.23 x10²%(d) 0.449%

(e) 0.310%

A solution is prepared by dissolving 20.0 g sodium hydroxide (NaOH) in water to give 500.0 mL of the solution. What is the molarity or concentration of this solution?

(a) 4.00 x 10^-2 mol/L (b) 1.00 x10^-3 mol/L (c) 1.00 x10^-1 mol/L

(d) 1.00 mol/L(e) 25.0 mol/L

What is the (m/v) percent (%) concentration of a solution prepared by dissolving 5.50 g glucose in water to give 75.0 mL of the solution.

(a) 7.33 x 10^-2 % (b) 6.83% (c) 6.83 x10^-2%(d) 13.6%

(e) 7.33%

Write the equations for the solubility of the following compound (an ionic compound) in water and predict if the aqueous solution is strong electrolyte/weak electrolyte/non-electrolyte ___ and good conductor of electricity/weak conductor of electricity/non-conductor of electricity ___ respectively?

KNO ₃ (s)

(a) Strong electrolyte and good conductor of electricity

(b) Strong electrolyte and non-conductor of electricity

(c) Weak electrolyte and weak conductor of electricity

(d) Non-electrolyte and non-conductor of electricity

(e) Weak electrolyte and good conductor of electricity

Write the equations for the solubility of the following compound (a molecular compound) in water and predict if the aqueous solution is strong electrolyte/weak electrolyte/non-electrolyte ___ and good conductor of electricity/weak conductor of electricity/non-conductor of electricity ___ respectively?

C ₁₂ H ₂₂ O ₁₁ (s)

(a) Strong electrolyte and good conductor of electricity

(b) Strong electrolyte and non-conductor of electricity

(c) Weak electrolyte and weak conductor of electricity

(d) Non-electrolyte and non-conductor of electricity

(e) Weak electrolyte and good conductor of electricity

Write the equations for the solubility of the following compound (a weak acid) in water and predict if the aqueous solution is strong electrolyte/weak electrolyte/non-electrolyte ___ and good conductor of electricity/weak conductor of electricity/non-conductor of electricity ___ respectively?

CH ₃ COOH(l)

(a) Strong electrolyte and good conductor of electricity

(b) Strong electrolyte and non-conductor of electricity

(c) Weak electrolyte and weak conductor of electricity

(d) Non-electrolyte and non-conductor of electricity

(e) Weak electrolyte and good conductor of electricity

Write the equations for the solubility of the following compound (a weak base) in water and predict if the aqueous solution is strong electrolyte/weak electrolyte/non-electrolyte ___ and good conductor of electricity/weak conductor of electricity/non-conductor of electricity ___ respectively?

CH ₃ NH ₂

(a) Strong electrolyte and good conductor of electricity

(b) Weak electrolyte and weak conductor of electricity

(c) Strong electrolyte and non-conductor of electricity

(d) Non-electrolyte and non-conductor of electricity

(e) Weak electrolyte and good conductor of electricity

Write the equations for the solubility of the following compound (an ionic compound) in water and predict if the aqueous solution is strong electrolyte/weak electrolyte/non-electrolyte ___ and good conductor of electricity/weak conductor of electricity/non-conductor of electricity ___ respectively?

CaCl ₂ (s)

(a) Weak electrolyte and good conductor of electricity

(b) Strong electrolyte and non-conductor of electricity

(c) Weak electrolyte and weak conductor of electricity

(d) Non-electrolyte and non-conductor of electricity

(e) Strong electrolyte and good conductor of electricity

Write the equations for the solubility of the following compound (a molecular compound) in water and predict if the aqueous solution is strong electrolyte/weak electrolyte/non-electrolyte ___ and good conductor of electricity/weak conductor of electricity/non-conductor of electricity ___ respectively?

C ₂ H ₅ OH(l)

(a) Non-electrolyte and non-conductor of electricity

(b) Strong electrolyte and non-conductor of electricity

(c) Weak electrolyte and weak conductor of electricity

(d) Strong-electrolyte and good-conductor of electricity

(e) Weak electrolyte and good conductor of electricity

Which of the following compound is insoluble in water?

(a)NaCl (b) (NH₄)₂CO₃ (c) CaCO₃ (d) K₂CO₃ (e) NaNO₃

Which of the following compound is soluble in water?

(a)Ca₃(PO₄)₃ (b) Fe(OH)₃ (c) CaCO₃ (d) Na₂CO₃

(e) AgCl

All following compounds are insoluble in water except ___?

(a) Mg₃(PO₄)₃ (b) Mg(ClO₄)₂ (c) FeCO₃ (d) Fe₂O₃ (e) AgCl

All following compounds are soluble in water except ___?(a)K₃PO₄ (b) FeCl₃ (c) Na₂SO₄ (d) NaClO₄ (e) MgCO₃

What is true ___about a cucumber placed in a salt-water solution (12%) (m/V) to make pickle?

(a) The water leaves the cucumber and cucumber’s cells crenate

(b) The water enters the cucumber and cucumber ’s cells swell

(c) The water leaves the cucumber and cucumber’s cells swell

(d) The water enters the cucumber and cucumber ’s cells crenate

(e) The water neither enters nor leaves the cucumber

Solution A with 5.8% (m/V) concentration of NaCl is separated from solution B of NaCl with 2.8% (m/V) concentration by a semipermeable membrane.

(a) Solution A is isotonic solution

(b) Solution A is hypotonic solution

(c) Solution A is hypertonic solution

(d) None of the above (A, B, & C) is true

What are (m/V)% concentrations NaCl ___ and D-glucose (C ₆ H ₁₂ O ₆) ___ respectively of the physiological solutions often used in hospitals,?

(a) 5.0% NaCl and 0.90% C₆H₁₂O₆

(b) 090% NaCl and 5.0% C₆H₁₂O₆

(c) 5.0% NaCl and 9.0% C₆H₁₂O₆

(d) 9.0% NaCl and 5.0% C₆H₁₂O₆

(e) 3.0% NaCl and 5.0% C₆H₁₂O₆

An aqueous solution of NaCl with 2.5% (m/V) concentrations is ___ to the physiological solutions often used in hospitals,

(a) Isotonic (b) hypotonic (c) Hypertonic (d) None is true

An aqueous solution of glucose (C ₆ H ₁₂ O ₆ ) With 3.5% (m/V) concentrations is ___ to the physiological solutions often used in hospitals,

(a) Isotonic (b) hypotonic (c) Hypertonic (d) None is true

An aqueous solution of glucose (C ₆ H ₁₂ O ₆ ) With 5.0% (m/V) concentrations is ___ to the physiological solutions often used in hospitals,

(a) Isotonic (b) hypotonic (c) Hypertonic (d) None is true

What is true statement ___ about a process called osmosis?

(a) Solute molecules move from a concentrate solution to a dilute solution

(b) Solute molecules move from a dilute solution to a concentrate solution

(c) Solvent molecules move across semipermeable membrane from a concentrate

solution to a dilute solution

(d) Solvent molecules move across semipermeable membrane from a dilute

solution to a concentrate solution

(e) Neither solute nor solvent molecules move across semipermeable membrane

What is true statement ___ about a process called diffusion?

(a) Solute molecules move from a concentrate solution to a dilute solution

(b) Solute molecules move from a dilute solution to a concentrate solution

(c) Solvent molecules move across semipermeable membrane from a concentrate

solution to a dilute solution

(d) Solvent molecules move across semipermeable membrane from a dilute

solution to a concentrate solution

(e) Neither solute nor solvent molecules move across semipermeable membrane

Why is water (H2O) called a universal solvent ___?

1. Most of the chemical substances present in the living systems are soluble in water
2. Most of the biochemical reactions occur in water as a solvent
3. Water is highly polar solvent and many substances dissolve in water

(a) 1 only (b) 1 and 2 only (c) 1 and 3 (d) 2 and 3 only (e) 1, 2, and 3

What is true about a condition called dehydration ___?

(a) Intake of water significantly exceeds the output of water in living organisms

(b) Output of water significantly exceeds the intake of water in living organisms

(c) Intake of water is equal to the output of the water in living organisms

(d) All of the above (A, B, &C) are true

(e) None of the above (A, B, C, & D) are true

What are the causes of the condition called dehydration ___?

(i) Severe diarrhea (ii) Vomiting(iii) High fever

(iv) High environmental temperature

(a) i only(b) i and ii only (c) i, ii, and iii only (d) i, ii, iii, and iv

(e) i, ii, and iv only

What are the essential or important roles of water in the living systems ___?

(i) Water is universal solvent

(ii) Water transports oxygen from lungs to the different parts of body

(iii) Water transports CO₂ from different parts of body to the lungs

(iv) Water transports nutrients into all the cells and organs of our body.

(a) i and ii only (b) i, ii, and iv only (c) i, ii, and iii only

(d) ii, iii, and iv only (e) i, ii, iii, and iv

Unique properties of water are due to which of the followings ____?

(i) High heat of vaporization

(ii) High boiling point compared to all other solvents with similar molar masses

(iii) Low boiling point compared to all other solvents with similar molar masses

(iv) High specific heat

(a) i and ii only (b) i, ii, and iv only (c) i, ii, and iii only

(d) ii, iii, and iv only (e) i, iii, and iv only

In the liquid state and in the solid state, oxygen (O) atom of the water (H ₂ O) molecule forms ___ bonds.

(a) Two covalent bonds between O and H atoms

(b) Two covalent bonds and two ionic bonds

(c) Two covalent bonds and two H-bonds

(d) One covalent bond and one H-bond

(e) Two ionic bonds and two H-bonds

What is true about a solution ____?

(a) Heterogenous mixture of two or more pure substances

(b) Homogenous mixture of two or more pure substances

(c) Component of the solution which dissolves the other component(s) and is present in larger amount and determines the physical state of the solution

(d) Component of the solution which is being dissolved by the other component

(e) None of the above (A, B, C, & D) is true

What is true about a solvent ____?

(a) Heterogenous mixture of two or more pure substances

(b) Homogenous mixture of two or more pure substances

(c) Component of the solution which dissolves the other component(s) and is present in larger amount and determines the physical state of the solution

(d) Component of the solution which is being dissolved by the other component

(e) None of the above (A, B, C, & D) is true

What is true about a solute ____?

(a) Heterogenous mixture of two or more pure substances

(b) Homogenous mixture of two or more pure substances

(c) Component of the solution which dissolves the other component(s) and is present in larger amount and determines the physical state of the solution

(d) Component of the solution which is being dissolved by the other component

(e) None of the above (A, B, C, & D) is true

Unique properties of water are due to which of the following ____?

(a) H-bonding interactions between water molecules

(b) Covalent bonding between oxygen and hydrogen atoms

(c) Ionic bonding interactions between hydrogen and oxygen atoms

(d) Ion-dipole interactions

(e) Metallic binding interactions

Which of the following is the solvent in a gaseous mixture called air____?

(a) Oxygen (O₂) (b) Nitrogen (N₂) (c) Carbon dioxide (CO₂)

(d) Argon (Ar) (e) Water vapors (H₂O(g))

Solubility of ionic compounds in water is mainly due to ____?

(a) H-bonding interactions

(b) Covalent bonding interaction

(c) Ionic bonding interactions

(d) Ion-dipole interactions

(e) Dipole-dipole interactions

For an ionic compound to dissolve in water what is the requirement ____?

(a) Lattice energy should be greater than the hydration (solvation) energy

(b) Hydration (solvation) energy should be greater than the lattice energy

(c) Hydration (solvation) energy should be less than or equal to lattice energy

(d) None of the above (A, B, & C) is true

A condition called Gout is due to the accumulation or deposition of which chemical compound(s) in the cartilage and tendons at the joints ____?

(a) Calcium phosphate only

(b) Calcium oxalate only

(c) Uric acid and calcium phosphate/calcium oxalate

(d) Sodium phosphate and calcium oxalate

(e) Uric acid only

A condition called kidney stone is due to the accumulation or deposition of which chemical compound(s) in the urinary tract, kidneys, ureter, or bladder ____?

(a) Calcium phosphate only

(b) Calcium oxalate only

(c) Uric acid and calcium phosphate/calcium oxalate

(d) Sodium phosphate and calcium oxalate

(e) Uric acid only

The solubility of carbon dioxide (CO ₂ ) gas in water at a certain temperature is 2.56 x 10 ^-5 mol/L with a CO₂ pressure of 1.85 atm above the solution. What will be the solubility of CO₂ if the pressure of CO₂ above the solution is increased to 6.95 atm at the same temperature ____?

(a) 9.62 x 10^-5 mol/L (b) 6.81 x 10^-6mol/L (c) 5.02 x 10⁵ mol/L

(d) 9.62 x 10⁵ mol/L (e) 9.62 x 10^-4 mol/L

The solubility of carbon dioxide (CO ₂ ) gas in water at a certain temperature is 9.75 x 10 ^-6 mol/L with a CO₂ pressure of 4.80 atm above the solution. What will be the required pressure of CO₂ above the solution at the same temperature to increase the solubility to 4.65 x 10 ^-5 mol/L ____?

(a) 1.01 atm(b) 22.9 atm(c) 9.45 x 10^-11 atm (d) 2.29 atm (e) 2.29 x 10^-1 atm

The concentration of Mg ²⁺ ions in a solution are 1.5 mmol/L, what is this concentration expressed in mEq/L ____?

(a) 1.5 mEq/L(b) 0.75 mEq/L(c) 4.5 mEq/L

(d) 3.0 mEq/L (e) 6.0 mEq/L

The concentration of Fe ³⁺ ions in a solution are 1.5 mmol/L, what is this concentration expressed in mEq/L ____?

(a) 1.5 mEq/L(b) 0.75 mEq/L(c) 4.5 mEq/L

(d) 3.0 mEq/L (e) 6.0 mEq/L

The concentration of Fe ³⁺ ions in a solution are 1.50 mEq/L, what is this concentration expressed in mmol/L ____?

(a) 1.50 mmol/L(b) 0.500 mmol/L(c) 3.00 mmol/L

(d) 4.5 mmol/L (e) 0.750 mmol/L

The concentration of Ca ²⁺ ions in a solution are 1.50 mol/L, what is this concentration expressed in mmol/L ____?

(a) 3.00 mmol/L(b) 0.500 mmol/L(c) 1.50 x 10^2- mmol/L

(d) 1.50 x 10^3- mmol/L (e) 1.50 x 10³ mmol/L

Which of the following solution will exert the highest osmotic pressure (π) ___?

(a) 3.00 mol/L NaCl(b) 6.00 mol/L C₆H₁₂O₆ (c) 3.00 mol/L MgCl₂

(d) 3.00 mol/L FeCl₃ (e) 3.00 mol/L KCl

What is true about a process called dialysis ___?

(a) The process used by kidneys to remove urea and other small molecules from the blood

(b) The artificial process of removing urea and other small molecules from the blood when kidneys of a patient are failing.

(c) Both of the above (a and b) are true

(d) None of the above (a and b) are true

What is true about a process called hemodialysis ___?

(a) The process used by kidneys to remove urea and other small molecules from the blood

(b) The artificial process of removing urea and other small molecules from the blood when kidneys of a patient are failing.

(c) Both of the above (a and b) are true

(d) None of the above (a and b) are true

What is/are true about a solution ___?

(i) Aqueous solutions are transparent

(ii) Components do not separate on standing

(iii) Components chemically react with each other

(iv) Homogenous mixture of two or more pure substances

(a) i and ii only(b) ii and iii only (c) i, ii, and iii only

(d) I, ii, and iv only (e) i, ii, iii, and iv

What is the true statement about the solubility of a compound ___?

(a) A given amount of a solute dissolved in a given volume of a solution

(b) The minimum amount of a solute that can dissolve in a given volume of solvent

(c) The maximum amount of a solute that can dissolve in a given volume of a

solvent/solution at a given temperature

(d) The maximum amount of a solute that can dissolve in a given volume of

solvent/solution

(e) Any amount of a solute that can dissolve in any amount of a solvent at any

temperature

Write a balanced chemical equation for the synthesis of glucose (C ₆ H ₁₂ O ₆ ) and oxygen (O₂) from CO₂ and H₂O in plants and answer the following question:

The coefficients for O ₂ ___, CO ₂ ___, and H ₂ O ___ respectively are:

(a) 1, 6, 6 (b) 6, 1, 6 (c) 6, 6, 1 (d) 6, 1, 1 (e) 6, 6, 6

Write a balanced chemical equation for the synthesis of glucose (C₆H₁₂O₆) and oxygen (O₂) from CO₂ and H₂O in plants and answer the following question:

Name of the reaction ___, name of the catalyst ___, and source of energy ___ respectively are:

(a) Chlorophyll, synthesis, & solar (b) photosynthesis, chlorophyll, & solar

(c) Photosynthesis, chloroform, & solar

(d) metabolism, chlorophyll, & solar

(e) Photolysis, chloroplast, & Sun

Write a balanced chemical equation for the reaction which occurs in animals consuming glucose (C₆H₁₂O₆) and oxygen (O₂) producing CO₂ and H₂O and answer the following question:

Name of the reaction ___, nature of the reaction endothermic or exothermic ___, and amount d of energy involved ___ respectively are:

(a) Metabolism of glucose, exothermic, and 2800 kJ

(b) Photosynthesis, endothermic, and 2800 kcal

(c) Photosynthesis, exothermic, and 2800 kJ

(d) Metabolism of glucose, endothermic, 2800 kJ

Which of the following compounds have the highest boiling point ____ and lowest boiling point ____ respectively?

(i) C₄H₁₀ (ii) C₅H₁₀ (iii) C₃H₈ (iv) CH₄ (v) C₂H₆

(a) iv and ii (b) i and iv(c) ii and iv (d) ii and v(e) v and ii

In the following pair, identify the one with higher boiling point ___ and this is due to ___?

PH ₃ , NH ₃

` (a) PH₃ and higher molar mass

(b) NH₃ and lower molar mass

(c) PH₃ and H-bonding interactions (

d) NH₃ and H-bonding interactions

(e) PH₃ and dipole-dipole interaction

In the following pair, identify the one with higher boiling point ___ and this is due to ___?

H ₂ O, H ₂ S

` (a) H₂S and higher molar mass

(b) H₂O and lower molar mass

(c) H₂O and H-bonding interactions

(d) H₂S and H-bonding interactions

(e) H₂S and dipole-dipole interaction

Arrange the following compounds in order of decreasing boiling points ___?

(i) N ₂ (ii) O ₂ (iii) H ₂ (iv) NO

(a) ii > iv > i > iii

(b) iii > i > ii > iv

(c) i > ii > iv > iii

(d) iv > i > ii > iii

(e) iv > ii > i > iii

Arrange the following compounds in order of increasing boiling point (lowest first) ____.

(i) C ₄ H ₁₀ (ii) C ₈ H ₁₈ (iii) C ₂ H ₆ (iv) C ₇ H ₁₆ (v) C ₆ H ₁₄

(a) i < iii < v < iv < ii

(b) iii < i < v < iv < ii

(c) ii < iv < v < i < iii

(d) iii < v < i < iv < ii

(e) None of the above is true

The pressure of a tire is measured to be 45.0 psi. What is this pressure expressed in kPa ___?

(a) 3.06 kPa

(b) 3.10 x 10³ kPa

(c) 2.33 x 10³ kPa

(d) 3.10 x 10² kPa

(e) None of the above is true

In a stormy day, the atmospheric pressure was found to be 798 mm Hg. What is this pressure express in kPa ____ and atm. ____ respectively?

(a) 1.06 x 10² and 1.05 atm (b) 1.05 kPa and 1.06 x 10² atm

(c) 15.4 kPa and 1.05 atm (d) 1.064 x 10² kPa and 1.06 atm

(e) None of the above is true

62. A sample of H₂ gas occupies a volume of 2.75 L at a pressure of 875 mm Hg at a certain temperature. What volume ___ will it occupy, in liters, if the pressure is decreased to 437 mm Hg with no change in temperature?

(a) 1.37 L (b) 5.51 L (c) 1.39 x 10⁵ L (d) 55.1 L (e) 13.7 L

A 2.50 L balloon is filled with helium gas at 750.0 mm Hg pressure and at a certain temperature. What is the pressure ___ in another 7.50 L balloon filled with the same amount of helium at the same temperature?

(a) 2.50 x 10^-2 mm Hg

(b) 2.25 x 10³ mm Hg

(c) 2.50 x 10³ mm Hg

(d) 2.50 x 10² mm Hg

(e) 2.50 x 10^-3 mm Hg

A sample of gas has a volume of 4.0 L at a pressure of 7.5 atm. If the pressure is decreased to 2.5 atm, the volume of the sample will be ____:

(a)1.0 L

(b) 2.0 L

(c) 4.0 L

(d) 8.0 L

(e) 12 L

A sample of gas has a volume of 500.0 mL at a pressure of 2.80 atm. If the gas is transferred to another container with 250.0 mL volume, the pressure of the gas will be ___.

(a) 1.40 atm

(b) 2.80 atm

(c) 5.60 atm

(d) 11.20 atm

(e) 0.700 atm

Which of the following bond s is the strongest bond ___?

(a) Covalent bond

(b) Metallic bond

(c) H-bond

(d) Coordinate covalent bond

(e) Ionic bond

Which of the following bond s is the strongest force/bond ___?

(a) London dispersion force (LDF)

(b) Dipole-dipole force

(c) H-bonding force

(d) None of the above is true

In the following pair, identify the one with higher boiling point ___ and this is due to ___?

H-Cl, H-Br

(a) H-Cl and dipole-dipole interaction

(b) H-Br and dipole-dipole interaction

(c) H-Cl and H-bonding interactions

(d) H-Br and H-bonding interactions

(e) H-Br and higher molar mass

In the following pair, identify the one with higher boiling point ___ and this is due to ___?

AsCl ₃ , SbBr ₃

(a) SbBr₃ and higher molar mass

(b) AsCl₃ and lower molar mass

(c) SbBr₃ and H-bonding interactions

(d) AsCl₃ and H-bonding interactions

If the pressure above the surface of the liquid is increased, the boiling point of the liquid will ___?

(a) Increase (b) Decrease (c) Stay the same

(d) None of the above (a, b, and c) is true

If the pressure above the surface of the liquid is decreased, the boiling point of the liquid will ___?

(a) Increase (b) Decrease (c) Stay the same

(d) None of the above (a, b, and c) is true

For a reaction to proceed spontaneously in the forward reaction, the Gibbs free energy (ΔGº) for the reaction should be ___?

(a) Negative (b) Positive (c) Neither positive nor negative

(d) None of the above (a, b, and c) is true

The heat of the reaction (q _rxn ) depends on____?

(a) Specific heat of the substance (c) (b) mass of the substance (m)

(c) change in temperature (ΔT)

(d) All of the above (A, B, and C) are true

(e) None of the above is true

The activation energy for the forward reaction (E _af ) = 225.0 kJ/mol and the activation energy of the reverse (backward) reaction (E _ar ) = 465.0 kJ/mol. What is the energy of the reaction (ΔH) ____?

(a) -240.0 kJj/mol

(b) 240.0 kJ/mol

(c) 345.0 kJ/mol

(d) 225.0 kJ/mol

(e) 465.0 kJ/mol

Which of the following factors affects the rate of a chemical reaction ____?

(a) Presence of a catalyst(b) Temperature

(c) Surface area of the reactants

(d) Orientations of the colliding molecules

(e) All of the above (A, B, C, & D)

What is the kinetic energy (KE) of a car with a mass (m) of 1.250 kg moving with a velocity (v) of 29.3 m/s ____?

(a) 1.07 x 10⁶ kg.m²/s²

(b) 5.37 x 10⁵ kg.m²/s²

(c) 3.66 x 10⁴ kg.m²/s²

(d) 1.83 x 10⁴ kg.m²/s²

(e) 7.33 x 10⁴ kg.m²/s²

What is the potential energy (PE) of a box with a mass (m) of 60.5 kg sitting on a shelf 6.75 meter (m) above the ground ____?

(a) 4.00 x 10⁴ kg.m²/s²

(b) 41.7 kg.m²/s²

(c) 2.76 x 10³ kg.m²/s²

(d) 1.38 x 10³ kg.m²/s²

(e) 4.00 x 10³ kg.m²/s²

What is the amount of heat energy (q) required to raise the temperature of 285.6 g of water from 25.5ºC to 98.8ºC ____?

(Given: specific heat (c) of water = 4.184 J/g.ºC)

(a) 2.10 x10² J

(b) 3.0 x 10⁴ J

(c) 1.18 x 10⁵ J

(d) 8.76 x 10⁴ J

(e) None of the above (A, B, C, & D) is true

How much heat energy (q) is given off when 75.8 g of methane (CH ₄ ) is burned with excess oxygen____?

(Given: Heat of combustion of CH ₄ is - 802.3 kJ/mol of methane)

(a) 6.08 x10⁴ kJ

(b) 3.79 x 10³ kJ

(c) -3.80 x 10³ kJ

(d) -6.08 x 10⁴ kJ

(e) None of the above (A, B, C, & D) is true

does chemistry suck?