Consider the following reaction and its rate law. Answer the following questions
ID: 1049113 • Letter: C
Question
Consider the following reaction and its rate law. Answer the following questions 2NO_(g) + O_2(g) rightarrow 2NO_2(g) Rate = k[NO]^2 [O_2] True or False The reactions order with respect to NO(g) is 2 due to the stoichiometry of the reaction. True or False The overall reaction order is 3. True or False If the temperature of the reaction is changed we expect a change in the value of k What would happen to the rate of the reaction if the concentration of O_2(g) in the reaction is doubled? Explain. What would happen to the rate of the reaction if the concentration of NO(g) was doubled? Explain.Explanation / Answer
2NO(g) + O2(g)--------> 2NO2(g)
Rate law
Rate = K[NO]2[O2]
order with respect NO is 2
order with respect O2 is 1
overall order is 3
1. True
2. True
3. True
rate constant depends upon temperature. very 10C0 rise rate constant 2 or 3 increases
4. Rate = K[NO]2[O2]
Rate = K[NO]2 [2O2]
Rate1/Rate2 = K[NO]2[O2]/2 K[NO]2[O2]
Rate1/Rate2 = 1/2
Rate2 =2* Rate1
Rate is double
concentration of O2 is double rate is double
5. Rate = K[NO]2[O2]
Rate = K[2NO]2 [O2]
Rate = 4K[NO]2[O2]
Rate1/Rate2 = K[NO]2[O2]/4 K[NO]2[O2]
Rate1/Rate 2 = 1/4
Rate2 = 4*Rate1
Rate is 4 times