2. Use the following data to determine the rate constant and rate law for the fo

Question

2. Use the following data to determine the rate constant and rate law for the following reaction Be sure to include the appropriate units on the rate constant and show all work B] (M 0.100 0.200 0.100 Experiment Number [A] (M) Initial Rate (M/s) 0.100 0.100 0.200 4.0 16 3. Write the rate law based on the following mechanism in terms of reactants. Identify any intermediates molecules NO2 (g) + NO2 (g) NO3(g) NO(g) (slow) NO3 (g) +CO(g) NO2(g) + CO2(g) (fast) 4. Given the following reactions N2(g) + O2(g) +2NO (g) Kp = 1.5. 10-10 2SO2(g) +O2(g) 2SO3(g) Kp 2.5-109 What is the equilibrium constant for the reaction below? Show all work for credit!!! N2(g) + 2SO3(g) 2NO (g)+ 2SO2(g) Kp? 5. How would a change in the following parameters affect the equilibrium of the reactions given below? CO(g) + H2O(g)-CO2(g) + H2(g) H° =-41.0 kJ a. Increase CO pressure Shift toward products/reactants/No change b. Decreasing the volume Shift toward products/reactants/No change C. Increase the pressure of Ar Shift toward products/reactants/No change d. Heating the reaction Shift toward products/reactants/No change

Explanation / Answer

2)

see experiment 1 and 3:

[A] doubles

[B] is constant

rate becomes 4 times

so, order of A is 2

see experiment 1 and 2:

[A] is constant

[B] doubles

rate is constant

so, order of B is 0

overall order = 2 + 0 = 2

Rate law is:

rate = k*[A]^2

Put values from 1st row of table in rate law

rate = k*[A]^2

4 = k*0.1^2*0.1^0

k = 400 M-1.s-1

Answer:

Rate law is: rate = k*[A]^2

k = 400 M-1.s-1

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