The rate law for the reaction 2S0 2(g) + O 2(g) 2S0 3(g) is, under certain conditions, rate = k[SO 2][O 2]. Which of the following is NOT true? A catalyst does not appear in the rate law. The reaction is second order with respect to [SO2]. %3D The reaction is first order with respect to [O2]. The reaction is second order overall.

The rate law for the reaction 2S0 2(g) + O 2(g) 2S0 3(g) is, under certain conditions, rate = k[SO 2][O 2]. Which of the following is NOT true? A catalyst does not appear in the rate law. The reaction is second order with respect to [SO2]. %3D The reaction is first order with respect to [O2]. The reaction is second order overall.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Pp
Consider the reaction aA + bB dD + eE C = catalyst The rate law is Rate = k[A]ª[B][C]S Which of the following statements is incorrect? The exponents q and r are always equal to the coefficients a and b, respectively. The overall reaction order is q + r+ s. O The exponent s must be determined experimentally. The symbol k represents the rate constant. O The exponents q, r, and s are often integers.
Consider the reaction, A + B + C => D, which is found to be first order in A, first order in B and first order in C. Which step of the proposed mechanism must be slow in order to agree with this rate law? 1. A(g) + B(g) => X(g) 2. X(g) + C(g) => Y(g) 3. Y(g) => D(g) A. 1 B. only 3 C. Either 2 or 3 D. only 2
The balanced chemical equation and rate law for the reaction between NO(g) and H2(g) at a particular temperature are 2NO(g) + 2H₂(g) → N₂(g) + 2H₂O(g) Rate = k[NO] [H₂] What is the reaction order with respect to nitric oxide AND the overall order of the reaction? 2,3 2,4 4,3 1,4 0,2
Consider the reaction and its rate law. 3A+3B⟶productsrate=?[A][B]2 What is the order with respect to A?
Consider the reaction and its rate law. 4A + 3B What is the order with respect to A? order: products What is the order with respect to B? order: What is the overall reaction order? overall order: rate = k[A]²[B]²
5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T
Initial rate: 1.6 •10^-7mol/L•s K=6.4 •10^-9L/mol•s Rate law: k[HI]^2 Can you please show me the steps.
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H,O,(aq) → H,0M + ½ O2(g) is first order in H,02 with a rate constant of 1.10×10-3 min!. If the initial concentration of H,O2 is 5.68×10-2 M, the concentration of H,O, will be |M after 2006 min have passed.
The following reaction is observed to be second order with respect to NO and first order with respect to Br2. Br2 (g) + 2NO (g) --> 2NOBr (g)
During kinetic studies, the following reaction was determined to be second order in respect to NO and zeroth order in respect to O2. What is the rate law for the reaction? 2 NO (g) + O2(g) -----> 2NO2 (g)
During kinetic studies, the following reaction was determined to be second order in respect to NO and zeroth order in respect to O2. What is the rate law for the reaction? 2 NO (g) + O2 (g) 2 NO2 (g) rate = k [O2]? %3D O rate = k [NO]?[O2]? rate = k [NO][O2] rate = k [NO]2[O2] %3D O rate = k [NO]? %3D