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General Chemistry 2

The following initial rate data was collected for the reaction, 2 NO + O2_2 \longrightarrow 2NO2_2

[NO2_2]X^X[O2_2]Y^Y

The following initial rate data was collected for the reaction, CH3_3Br + OH^- \longrightarrow CH3_3OH + Br^-

B. What is the rate constant?

The following initial rate data was collected for the reaction, A + B + C \longrightarrow products

What are the reaction orders with respect to the reactants?

A \longrightarrow products

t12_\frac{1}{2} = 180s

A. What % of A is left unreacted at 900 s?

B. What is the rate at [A] = 0.50 M?

The half life of uranium-238 is 4.51 x 109^9 years. What is the rate constant? How much uranium-238 is left after 4 half lives if we start with 64 mg?

A first order reaction has a half life of 20.0 min.

A. Calculate the rate constant for this reaction

B. How much time is required for this reaction to be 75% complete?

Below is a proposed mechanism for a reaction, with k2 > k1. What is the rate law?

NO2+CO k1 NO+NO3NO_2 + CO~ \xrightarrow{k_1}~ NO + NO_3

NO3+CO k2 NO2+CO2NO_3 + CO~ \xrightarrow{k_2}~ NO_2 + CO_2

Below is a proposed mechanism for a reaction, with k1 > k2. What is the rate law?

NO2+CO k1 NO+NO3NO_2 + CO~ \xrightarrow{k_1}~ NO + NO_3

NO3+CO k2 NO2+CO2NO_3 + CO~ \xrightarrow{k_2}~ NO_2 + CO_2

Below is a proposed mechanism for a reaction, with k1 > k2. What is the rate law?

NO+Br2 k1k1 NOBr2NO+ Br_2~ \mathop{\leftrightharpoons}^{k_1}_{k_{-1}}~ NOBr_2

NOBr2+NO k2 NOBr+NOBrNOBr_2 + NO~ \xrightarrow{k_2}~ NOBr + NOBr

For the mechanism proposed below, use the quasi (pseudo) steady state approximation to determine the overall rate law assuming the pseudo steady state.

2 NO + 2H2  2 H2O + N2  overall2~NO~+~2 H_2~\longrightarrow~2~H_2O~+~N_2~~{overall}

2 NO+ H2 k1k1 N2O + H2O2~NO+~H_2~\mathop{\leftrightharpoons}^{k_1}_{k_{-1}}~N_2O~+~H_2O

N2O + H2 k2 N2 + H2ON_2O~+~H_2~\xrightarrow{k_2}~N_2~+~H_2O

Use the pseudo steady state hypothesis to derive the rate law for the rate of production of P

E + S k1k1 ESE~+~S~\mathop{\leftrightharpoons}^{k_1}_{k_{-1}}~ES

ES k2 E +PES~\xrightarrow{k_2}~E~+P

Derive the rate law for the following reaction mechanism

OCl H2O  HOCl+OHOCl^-~H_2O~\leftrightharpoons~HOCl + OH^-

I+HOCl  HOI+Cl  slowstepI^- + HOCl~\longrightarrow~HOI + Cl^-~~{slow step}

HO+OH H2O+OIHO + OH^-\longrightarrow~H_2O + OI^-

Find equilbirium concentrations of each species when starting with 3.0 M I2_2

I2_2 (g) \leftrightharpoons 2 I (g) , KC_C = 3.8 x 105^{-5}

A 3.050 L reaction vessel contains 0.3500 mol CO, 0 mol Cl2_2, 0.05500 mol COCl2_2. Find the molarity of Cl2_2 at equilibrium.

CO + Cl2_2 \leftrightharpoons COCl2_2 , KC_C = 1200

At 1000 K, 0.250 mol SO2_2 and 0.200 mol O2_2 react in a 10.0 L reaction vessel to form 0.162 mol of SO3_3 at equilibrium. What is Keq_{eq} at 1000 K for the reaction?

2 SO2_2 (g) + O2_2 (g) \leftrightharpoons 2 SO3_3 (g)

3 A(s) + 5 B(g) \leftrightharpoons 5 C(g) + 6 D(s) \triangleH = 0 kJ

A. Predict the change in A when D is added

B. Predict the direction of reaction when the pressure is increased

C. Predict the direction of reaction when the heat is increased

Determine how the following changes will effect the concentrations of the reactants and products.

2 NO2_2 (g) \leftrightharpoons N2_2O4_4 (g) \triangleH = -58 kJ

A. Addition of N2_2O4_4

B. Removal of NO2_2

C. Increase in volume

D. Decrease in temperature

heat + 2 NO2_2(g) \leftrightharpoons N2_2O4_4(g)

Which of the following changes will not be effective in increasing the amount of N2_2O4_4? (more than one answer may be chosen)

a decrease in volume, an increase in heat, an addition of N2_2, or removal of N2_2O4_4

A vessel contains 0.5 M acetic acid, which dissociates as shown below. What is the concentration of the acetate ion at equilibrium, given the Ka_a below?

CH3_3COOH (aq) \leftrightharpoons CH3_3OO^{-} (aq) + H+^+ (aq) , Ka_a = 1.8 x 105^{-5}

Define acids and bases according to the Bronsted-Lowry and Lewis theories.