The gas phase reaction between hydrogen and iodine is proposed to occur as follows:

.....step 1..... fast:...... I₂ 2 I

.....step 2..... slow:.... H₂ + 2 I 2 HI

(1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank.

(2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank:

(3) Complete the rate law for the overall reaction that is consistent with this mechanism.
Use the form k[A]^m[B]ⁿ... , where '1' is understood (so don't write it if it's a '1') for m, n etc.

1) H₂+I₂ -> 2HI

2) I

3) k[H₂][I₂]

Hydrogen peroxide decomposes into water and oxygen in a first-order process.
H₂O₂(aq) → H₂O() + 1/2 O₂(g)
At 20.0 °C, the half-life for the reaction is 3.92E+4 seconds. If the initial concentration of hydrogen peroxide is 0.822 M, what is the concentration after 3.27 days?

5.56E-3

The equilibrium constant, K_c, for the following reaction is 77.5 at 600 K.
CO(g) + Cl₂(g) COCl₂(g)
Assuming that you start with equal concentrations of CO and Cl₂ and no COCl₂ is initially present, describe the relative abundance of each species present at equilibrium.

[CO]
[COCl₂]
[Cl₂]
1) Higher 2) Lower 3) Can't tell

2

1

2

Consider the reaction:
C(s) + 1/2 O₂(g) CO(g)

Write the equilibrium constant for this reaction in terms of the equilibrium constants, K_a and K_b, for reactions a and b below:

a.) C(s) + O₂(g) CO₂(g).............K_a

b.) CO(g) + 1/2 O₂(g) CO₂(g).............K_b

K_a / K_b

For the reaction coordinate diagram shown below, what is the order of the reaction?

two fast steps followed by one slow step, with a build up of intermediates between all three steps

onsider the following system at equilibrium where K_c = 1.29E-2 and H^o = 108 kJ/mol at 600 K:
COCl₂(g) CO(g) + Cl₂(g)
The production of CO(g) is favored by
Indicate True (T) or False (F) for each of the following choices.
1. Increasing the temperature.
2 . Decreasing the pressure (by changing the volume).
3. Decreasing the volume.
4. Removing COCl₂.
5. Adding Cl₂.

T

T

F

F

F

For the reaction A → B, the rate law is
.
What are the units of the rate constant where time is measured in seconds?

1/s

The activation energy for the gas phase decomposition of t-butyl acetate is 170 kJ.

CH₃COOC(CH₃)₃ (CH₃)₂C=CH₂ + CH₃COOH
The rate constant at 539 K is 7.12E-4 /s. The rate constant will be 8.33E-3 /s at

576

The equilibrium constant, K_c, for the following reaction is 1.29E-2 at 600 K.
Calculate K_p for this reaction at this temperature.

COCl₂(g) CO(g) + Cl₂(g)

0.635

Which of the following statements is/are CORRECT?
1.A reaction will proceed in the forward direct when Q>K

2.A reaction favors the formation of products if K >> 1.

3.In an Endothermic reaction, increasing the temperature will increase [Reactants

2 only

For the decomposition of ammonia on a tungsten surface at 1100 ^oC

2 NH₃ -> N₂ + 3 H₂

the average rate of disappearance of NH₃ over the time period from t = 0 s to t = 1.63E+3 s is found to be 3.40E-6 M s ^-1.

What is the average rate of appearance of N₂ over the same time period?

1.7E-6

Which of the following is true regarding the rate constant (k)?

1. It is temperature independent
2. It is concentration independent
3. It is a proportionality constant

2 and 3

Write the equilibrium constant expression, K, for the following reaction:
Please enter the compounds in the order given in the reaction.If either the numerator or denominator is 1, please enter 1.

BaSO₄(s) Ba²⁺(aq) + SO₄ ^2-(aq)

[Ba2+] [SO42-]/1

[Ba²⁺][SO₄ ^2-]/1

The equilibrium constant, K_c, for the following reaction is 55.6 at 698 K:

H₂(g) + I₂(g) 2 HI(g)

Calculate the equilibrium concentrations of reactants and product when 0.305 moles of H₂ and 0.305 moles of I₂ are introduced into a 1.00 L vessel at 698 K.

H₂: 0.0645

I₂: 0.0645

HI: 0.4810

Consider the following reaction where K_p = 9.52E-2 at 350 K:

CH₄(g) + CCl₄(g) 2 CH₂Cl₂(g)

If the three gases are mixed in a rigid container at 350 K so that the partial pressure of each gas is initially one atm, what will happen?

Indicate True (T) or False (F) for each of the following:

1 . A reaction will occur in which CH₂Cl₂(g) is produced.
2. K_p will decrease.
3. A reaction will occur in which CH₄ is produced.
4. Q is greater than K.
5. The reaction is at equilibrium. No further reaction will occur.

F

F

T

T

F

or the gas phase decomposition of t-butyl acetate,

CH₃COOC(CH₃)₃ (CH₃)₂C=CH₂ + CH₃COOH
the rate constant has been determined at several temperatures. When ln k in s^-1 is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.04E+4 K and a y-intercept of 30.7.

The activation energy for the gas phase decomposition of t-butyl acetate is

170

NaHCO₃ (aq) + HNO₃ (aq) NaNO₃(aq) + H₂O(l) + CO₂(g)

Which of the following could be a way to increase the rate of the reaction above?
Indicate "yes" or "no" for each choice.

Increasing the temperature.
Doubling the pressure.
Increasing the concentration of NaHCO₃
Increasing the concentration of HNO₃

Yes

No

Yes

Yes

The reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution

OCl^- + I^- -> OI^- + Cl^-

is first order in OCl^- and first order in I^-.
Complete the rate law for this reaction in the box below.
Use the form k[A]^m[B]ⁿ... , where '1' is understood for m, n ...(don't enter 1) and concentrations taken to the zero power do not appear

k[OCl^-][I^-]

Hydrogen peroxide decomposes into water and oxygen in a first-order process.
H₂O₂(aq) → H₂O() + 1/2 O₂(g)
At 20.0 °C, the half-life for the reaction is 3.92E+4 seconds. If the initial concentration of hydrogen peroxide is 0.696 M, what is the concentration after 7.15 days?

1.25E-5

CO (g) + Br₂ (g) COBr₂(g)

Which of the following could be a way to increase the rate of the reaction indicated above?
Indicate "yes" or "no" for each choice.

Increasing the temperature.
Doubling the pressure.
Increasing the concentration of CO.
Increasing the concentration of Br₂.

Yes to all

In a study of the decomposition of nitrosyl bromide at 10 ^oC

NOBr NO + ½ Br₂

the concentration of NOBr was followed as a function of time.

It was found that a graph of 1/[NOBr] versus time in seconds gave a straight line with a slope of 1.22 M^-1s^-1 and a y-intercept of 2.60 M^-1.

Based on this plot, the reaction is ____ order in NOBr and the rate constant for the reaction is ____

second

1.22

For the second-order reaction below, the rate constant of the reaction is 8.88E-3 M^–1s^–1. How long (in seconds) is required to decrease the concentration of A from 1.34 M to 0.119 M?

2A → B rate = k [A]²

862

The equilibrium constant, K_p, for the following reaction is 0.497 at 500 K.
Calculate K_c for this reaction at this temperature.

PCl₅(g) PCl₃(g) + Cl₂(g)

1.21E-2

The activation energy for the gas phase isomerization of dimethyl maleate is 111 kJ/mol.

cis-CH₃OOCCH=CHCOOCH₃ trans-CH₃OOCCH=CHCOOCH₃
The rate constant is 7.08E-4 s^-1 at 701 K. At what temperature is the rate constant 3.77E-3 s^-1?

768

For the gas phase decomposition of vinyl ethyl ether,

CH₂=CH-OC₂H₅ C₂H₄ + CH₃CHO
the rate constant has been determined at several temperatures. When ln k in s^-1 is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.20E+4 K and a y-intercept of 26.3.

The activation energy for the gas phase decomposition of vinyl ethyl ether is

-183.2

Consider the following reaction:

NH₄Cl (s) -> NH₃ (g) + HCl (g)

If a flask maintained at 554 K contains 0.125 moles of NH₄Cl(s) in equilibrium with 1.59E-2 M NH₃(g) and 2.73E-2 M HCl(g), what is the value of the equilbrium constant at 554 K?

4.34E-4

What does decreasing volume do?

Increases pressure

goes towards fewer moles

if Q > K

increase products

if Q < K

increase reactants