Chapter -15&16

The gas phase reaction A+B -> C has a reaction rate which is experimentally observed to follow the relationship rate=k[A]2[B]. If the concentration of A is tripled and the concentration of B is doubled, the reaction rate would be increased by a factor of ____

18

Nitrogen oxide and bromine combine to form nitrosyl bromide, NOBr 2NO(g) +Br2(g) -2NOBr(g) In a 5.0 liter reaction at equilibrium at a constant temperature, it was determined there was 0.45 mil NO, 0.17 mol Br and 1.32 mol NOBr. What is the value of kc at this temperature?

253

At 500 c the following reaction has kp=133. If a reaction is initiated with the partial pressure of each gas at 1.0 atm, what is the total pressure of the reaction mixture at equilibrium? H2(g) + Br2(g)!— 2HBr(g)

3.0 atm

The half life of the zero order reaction A->B is 0.56 minutes. If the initial concentration of a is 3.4 M, what is the rate constant?

3.04 mol/L•min

4Br2(g) + CH4(g) -> 4HBr(g) + CBr(g)

Kc=[CBr4] [HBr) ^4/ [Br2]^4 [CH4]

The half-life for the reactant A in the first order reaction below is 36.2 seconds. What is the rate constant for this reaction at the same temperature? A → B a. 52.2 s−1 b. 0.0276 s−1 c. 0.0191 s−1 d. 18.1 s−1 e. 0.00832 s−1

0.0191 s^-1

A reaction begins with 0.600 moor of A and 0.200 mole of B in a 2.00-L container at a certain temperature. What will be the equilibrium concentration of C? A(g) + B(g) —C(g) kc=23.5

0.0836 M

The specific rate constant, k, for a reaction is 2.64*10^-2 s^-1 at 25c, and the activation energy 74.0 kJ/mol. Calculate K at 50c

0.266 s-1

In the following reaction D[B]/Dt=0.89 mol/L•s. What is the value of the rate of the reaction at this time? A+3B-> AB3

0.30 mol/L•s

What is the value of Kc for the reaction 2A(g) +3B(g) -2C(g) + D(g) if at equilibrium [A]=0.60 M, [B]=0.30M, [C]=0.10 M and [D]=0.50 M

0.51

Consider the following reaction in which all reactants and products are gases. 1.00 mol of A an 2.00 mol of B are placed in a 5.0 liter container. After equilibrium has been established, 0.50 mol of D is present in the container. Calculate the equilibrium constant kc for the reaction A+2B-2C+D

1.0

Evaluate the specific rate constant for the reaction at 800 c. The rate law expression is rate= k[NO]2 [H2]. Choose the closer answer

1.3*10^2 M^-2 •s-1

The numerical value of the equilibrium constant kc for the following gas phase reaction is 0.50 at a certain temperature. When a certain reaction mixture reaches equilibrium, the concentration of O2 is found to be 2.0 M, while the concentration of SO3 is found to be 10M. What is the equilibrium concentration of SO2 in this mixture.

10M

One of the reactions that is used to produce gaseous hydrogen commercially follows. A proper expression for the rate of this reaction could be ____. H2O(g) + CO(g) → H2(g) + CO2(g) a. b. c. k d. e.

-DH2O/Dt

The equilibrium constant for the reaction CO(g) + H2O(g) - CO2(g) +H2(g) is 26 at 50c what is Kc for 3CO2(g) +3H2(g)-3CO(g)+3H2O(g) at the same temperature?

5.7 *10^-5

The Kc tor the following reaction is 56.2 at 305c A2(g) +B2(g) -2C(g)

5.7 M

Suppose the activation energy of a certain reaction is 250 kJ/mol. If the rate constant at T1 = 300 K is k1, and the rate constant at T2 = 320 K is k2, then k2/k1 = ____. (The universal gas constant = 8.314 J/mol•K.) a. 3 × 10−29 b. 0.067 c. 15.0 d. 525 e. 3 × 1028

525

Which of the following is the best definition of chemical equilibrium?

A condition where the forward and reverse reaction rates of a reversible reaction are equal and constant

The following reaction is initiated and the concentrations are measured after ten minutes: A(g) +3 B(g)-AB3(g); Kc=1.33 *10^-2 [A]=1.78 M [B]=2.21 M [AB3]=1.19 M

No, because Q>K

The reaction is _____ order in A and _____ order in B.

Second,first

Consider the following reaction involving a solids. 3Fe(s) +4H2O(g) - Fe3O4(s) +4H2(g)

[H2]^4/[H2O]^4