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The reaction 2 NO1g2 + O21g2 2 NO21g2 is second order in
Chapter , Problem 14.91(choose chapter or problem)
The reaction 2 NO1g2 + O21g2 2 NO21g2 is second order in NO and first order in O2. When 3NO4 = 0.040 M, and 3O24 = 0.035 M, the observed rate of disappearance of NO is 9.3 * 10-5 M>s. (a) What is the rate of disappearance of O2 at this moment? (b) What is the value of the rate constant? (c) What are the units of the rate constant? (d) What would happen to the rate if the concentration of NO were increased by a factor of 1.8?
Questions & Answers
QUESTION:
The reaction 2 NO1g2 + O21g2 2 NO21g2 is second order in NO and first order in O2. When 3NO4 = 0.040 M, and 3O24 = 0.035 M, the observed rate of disappearance of NO is 9.3 * 10-5 M>s. (a) What is the rate of disappearance of O2 at this moment? (b) What is the value of the rate constant? (c) What are the units of the rate constant? (d) What would happen to the rate if the concentration of NO were increased by a factor of 1.8?
ANSWER:Problem 14.91The reaction 2 NO(g) + O2(g) 2 NO2(g) is second order in NO and first order in O2. When[NO] = 0.040 M, and [O2] = 0.035 M, the observed rate of disappearance of NO is 9.3 x 10-5M/s. (a) What is the rate of disappearance of O2 at this moment (b) What is the value of therate constant (c) What are the units of the rate constant (d) What would happen to the rate ifthe concentration of NO were increased by a factor of 1.8 Step-by-step solution Step 1 of 4 (A) 2NO(g) + O (g) 2NO (g) 2 2 [NO] [O ] Rate = 1 = 2 2 t t [NO] = 2Rate t 2Rate = 9.3 x 10 M/s 9.3×10 5M/s Rate = 2 = 4.65 x 10 M/s [O ] 2 = 4.7 x 10 M/s t