Question 16: Consider the following reaction: 2 N₂0(g) - > 2 NO(g) +O₂(g). The rate law is: rate = k[N₂0]. If the half-life for the reaction is 0.910 s, the rate constant is: 0.69 S-1 O 1.1 s1 O 1.3 s1 0.76 s-1 0 0.32 s-¹ s1

Consider the following proposed mechanism for the reaction: 2 NO2Cl (g) → 2 NO2 (g) + Cl2 (g) step 1 (slow): NO2Cl (g) → NO2 (g) + Cl (g) step 2 (fast): Cl (g) + NO2Cl (g) → NO2 (g) + Cl2 (g) What is the rate law consistent with this mechanism?     rate = k[NO2][Cl2]   rate = k[NO2Cl]   rate = k[NO2Cl]2   rate = k[NO2Cl]2[Cl]   rate = k[NO2Cl][Cl please answer ASAP

What is the half life of the following reaction, given the following set of conditions (Hint: observe the units for the rate constant to determine the order of the reaction!):  2 HI (g) → H2 (g) + I2 (g)   Initial concentration of HI = 1.00 M k = 1.2 x 10-3 M-1 s-1

You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions: O [A] = 6.0 and [B] = 0.6 O [A] = 3.0 and [B] = 0.6 O [A] = 4.5 and [B] = 0.6 [A] = 1.5 and [B] = 1.2 O [A] = 3.0 and [B] = 1.8 [A] = 1.5 and [B] = 1.8 O [A] = 3.0 and [B] = 1.2 O [A] = 7.5 and [B] = 0.6 Rate = K[A][B][C] Rate = K[A][C] Experiment [A] (M) [B] (M) Rate (M/s) (a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A]* [B]Y? Choose all correct possibilities. k[A]² [C] O Rate = K[A][C]² Rate = k[A]²[C]² Rate = k[A]³ [C] O Rate = K[A][C]³ 1 2 Rate = 1.5 3.0 (b) For a reaction of the form, A + B + C --> Products, the following observations are made: tripling the concentration of A increases the rate by a factor of 9, doubling the concentration of B has no effect on the rate, and doubling the concentration of C…

For the given equation at 800 °C: CO(g) + Ch(g) > COCh(g), the following data were collecica Experiment (COL(M) 0.96 1.92 0.96 (CH] (M) 1.60 1.60 3.20 Rate of appearance COCh (M/s) 0.121 0.242 0.484 Determine the Rate Law for the reaction From your Rate Law determined in question #1 above, determine the value of the rate constant WITH THE APPROPRIATE UNITS. ONLY If you could not answer #1 above, use this "mock" data to solve for k: Rate = K[ARB]?, with [A] = 1.00 M and B]o = 1.50 M, with a rate of 2.50 x 10-2 M/s.

Some measurements of the initial rate of a certain reaction are given in the table below. [N-] N2 H2 initial rate of reaction 2.22M 0.905 M 39.0M/s 2.22M 0.971M 44.9 M/s olo 0.709 M 0.905 M 12.5 M/s Ar Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k ||I k =

Cyclopropane, C3H6, is converted to its isomer propylene, CH2=CHCH3, when heated. The rate law is first order in cyclopropane, and its rate constant is (6.70x10^-4)/s at 500°C. if the initial concentration of cyclopropane is (3.860x10^-2) mol/L, what is the concentration after (8.550x10^2) s? Just enter the number  (e.g. 2.48x10^-4) and the unit.  Note: Your answer is assumed to be reduced to the highest power possible. Your Answer:

: Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl2(g) Determine the rate equation, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) 0.10 0.30 0.20 Rate (mol/L/h) 8.0 x 10-10 3.2 x 10-9 7.2 x 10-9

The decomposition of ethyl chloride, CH3CH2Cl, follows the rate law: Rate = k[CH3CH2Cl]. At 550°C, k = 3.2 x 10-2 sec-1. What is the half-life for this reaction? What was the initial concentration of ethyl chloride if after one minute, 0.01 M remains?

In a study to determine the rate of the following reaction: 2NO(g) +0,(g) 2NO, (g) the concentration of NO was 0.0650 Mat t= 5.0 s and 0.0225 Mat t= 650.0 s. What is the average rate of the reaction during this time period? M/s