Question

Rate constants for the reaction NO2(g)+CO(g)→NO(g)+CO2(g) are 1.3M−1s−1 at 700 K and 23.0M−1s−1 at 800 K....

Rate constants for the reaction NO2(g)+CO(g)→NO(g)+CO2(g) are 1.3M−1s−1 at 700 K and 23.0M−1s−1 at 800 K. What is the rate constant at 760 K ? Express your answer using two significant figures.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Rate constants for the reaction NO2(g)+CO(g)?NO(g)+CO2(g) are 1.3M?1s?1 at 700 K and 23.0M?1s?1 at 800 K....
Rate constants for the reaction NO2(g)+CO(g)?NO(g)+CO2(g) are 1.3M?1s?1 at 700 K and 23.0M?1s?1 at 800 K. Part A What is the value of the activation energy in kJ/mol? Ea = 134   kJ/mol   SubmitMy AnswersGive Up Correct Part B What is the rate constant at 770K ? Express your answer using two significant figures. k =   /(M?s)
The reaction between nitrogen dioxide and carbon monoxide is NO2(g)+CO(g)→NO(g)+CO2(g) The rate constant at 701 K...
The reaction between nitrogen dioxide and carbon monoxide is NO2(g)+CO(g)→NO(g)+CO2(g) The rate constant at 701 K is measured as 2.57 M−1⋅s−1 and that at 895 K is measured as 567 M−1⋅s−1. The activation energy is 1.5×102 kJ/mol. Predict the rate constant at 525 K . Express the rate constant in liters per mole-second to three significant figures.
Consider the reaction CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.150 MCO and...
Consider the reaction CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.150 MCO and 0.150 MH2O. Part A What will be the equilibrium concentration of CO? Express the concentration in molarity to two significant figures.
Consider the following reaction: 2NO(g)+2H2(g)→N2(g)+2H2O(g). If the rate constant for this reaction at 1000 K is...
Consider the following reaction: 2NO(g)+2H2(g)→N2(g)+2H2O(g). If the rate constant for this reaction at 1000 K is 6.0×104M−2s−1, what is the reaction rate when [NO]= 2.90×10−2M and [H2]= 1.80×10−2M? Express your answer using two significant figures. rate =   M/s   SubmitMy AnswersGive Up Part C What is the reaction rate at 1000 K when the concentration of NO is increased to 0.14 M, while the concentration of H2 is 1.80×10−2M? Express your answer using two significant figures.
Consider the reaction, NO2(g) + CO(g) → NO(g) + CO2(g), for which the rate law has...
Consider the reaction, NO2(g) + CO(g) → NO(g) + CO2(g), for which the rate law has been determined to be: Rate = [NO2]2[CO]. Which of the following statements is/are false? I. The reaction can occur in a single step. II. The rate of change of NO2 is twice the rate of change of CO. III. Doubling the concentrations of NO2 and CO simultaneously will increase the rate by a factor of four.
The following is a proposed mechanism for the reaction NO2 (g) + CO (g) --> NO...
The following is a proposed mechanism for the reaction NO2 (g) + CO (g) --> NO (g) + CO2 (g). The rate law for the reaction is rate = k [NO2]2 a) is this a plausible mechanism? Explain. B) identify the reactants, intermediates, and products. NO2 (g) + NO2 (g)--> NO3 (g) + NO (g) (slow) and NO3 (g) + CO (g) --> NO2 (g) + CO2 (g) (fast)
The following is a proposed mechanism for the reaction NO2 (g) + CO (g) --> NO...
The following is a proposed mechanism for the reaction NO2 (g) + CO (g) --> NO (g) + CO2 (g). The rate law for the reaction is rate = k [NO2]2 a) is this a plausible mechanism? Explain. B) identify the reactants, intermediates, and products. NO2 (g) + NO2 (g)--> NO3 (g) + NO (g) (slow) and NO3 (g) + CO (g) --> NO2 (g) + CO2 (g) (fast)
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌...
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌ COCl2 (g) A reaction mixture initially contains a CO concentration of 0.1530 M and a Cl2 concentration of 0.176 M at 1000 K. Part A What is the equilibrium concentration of CO at 1000 K? Express your answer in molarity to three significant figures. Part B What is the equilibrium concentration of Cl2 at 1000 K? Express your answer in molarity to three significant...
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌...
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌ COCl2 (g) A reaction mixture initially contains a CO concentration of 0.1470 M and a Cl2 concentration of 0.172 M at 1000 K. Part A What is the equilibrium concentration of CO at 1000 K? Express your answer in molarity to three significant figures. Part B What is the equilibrium concentration of Cl2 at 1000 K? Express your answer in molarity to three significant...
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌...
For the following reaction, Kc = 255 at 1000 K. CO (g) + Cl2 (g) ⇌ COCl2 (g) A reaction mixture initially contains a COconcentration of 0.1450 M and a Cl2concentration of 0.170 M at 1000 K. Part A What is the equilibrium concentration of CO at 1000 K? Express your answer in molarity to three significant figures. Part B What is the equilibrium concentration of Cl2 at 1000 K? Express your answer in molarity to three significant figures. Part...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT