From the data in the table, obtained at 360 K,   (a) determine the overall order of the reaction.       Initial Rate of Disappearance of X (M/s) [X] (M) [Y](M) 0.053 0.10 0.50 0.127 0.20 0.30 1.02 0.40

17. SHOW ALL YOUR WORK OGiven the following data, determine the order of the reaction with respect to NO(g). 2 NO(g) + Cl2(g)→ 2 NOCI(g) Experiment 1 [C2] (M) 0.0100 [NO] (M) Rate (M/s) 3.4 x 104 1.36 x 103 3.4 x 104 0.0300 0.0150 0.0150 0.0100 3 0.0400

3. Consider NO₂ (g) + CO (g) → NO (g) + CO₂ (g). The initial rates are shown in the table below. Please compute (a) the rate law for the reaction and (b) compute the value of k. [CO] 0.050 0.050 0.100 0.100 [NO₂] 0.050 0.100 0.200 0.100 Initial Rate (M/s) 0.0040 0.016 0.256 0.0640

A certain reaction is first order in N, and second order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N] [H,] initial rate of reaction x10 2.37 M 0.112 M 0.123 M/s alo ) 2.37 M 0.0539 M M/s 18 Ar 0.339 M 0.784 M | M/s

6. The following data were obtained for the reaction: A → products. Determine the rate law for this reaction, including the value of k. [A] (M) time (s) 0.800 0 0.775 40 0.750 83 0.725 129 0.700 179

Consider the hypothetical reaction: 2 X + Y → 2 Z and its general rate law: Rate = The following data were obtained when the reaction was studied at 660 K: k[X][Y]n [X], M 0.010 0.020 0.010 [Y], M 0.010 0.010 0.020 (a) What is the order of reaction with respect to X? (b) What is the order of reaction with respect to Y? (c) What is the overall order of reaction? (d) What is the rate law? (e) What is the value of the rate constant? (2 points) (2 points) (1 point) (1 point) (2 points) Rate, M/s 2.5 x 10-5 1.0 x 10-4 5.0 x 10-5 (f) What is the rate of the reaction if [X] =0.015 M and [Y] =0.005 M? (2 points)

Determine the (a) rate law (b) solve for the order, and (c) value of rate constant for the reaction. C + D + E ⟶⟶ Products Reaction # [C]0 [D]0 [E]0 Initial rate (mol/L s) 1 0.400 0.300 0.560 7.14 x 10 -4 2 0.100 0.500 0.200 4.55 x 10 -5 3 0.100 0.200 0.200 4.55 x 10 -5 4 0.400 0.300 0.750 1.28 x 10 -3 5 0.100 0.300 0.560 3.57 x 10 -4

Consider the reaction: A + B --> products.  From the following data obtained at a certain temperature, determine the order of the reaction (rate law) and calculate the rate constant:   [A] (M)                       [B] (M)                       Rate (M/s)   1.50                             1.50                             3.15 X 10-1 1.50                             2.50                             2.98 X 10 –1 3.00                             1.50                             5.50 X 10-1

A certain reaction is second order in N, and first order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. initial rate of reaction x10 0.537 M 0.350 M 21.0 M/s 0.169 M 0.350 M || M/s 0.261 M 0.721 M M/s

The decomposition of N,0, can be described by the equation 2N,0,(soln) – 4 NO,(soln) + 0,(g) Consider the data in the table for the reaction at 45 "C in carbon tetrachloride solution. t (8) IN3Ogl (M) 1.934 175 1.732 446 1.461 825 1.151 Given the data, calculate the average rate of reaction for each successive time interval. What is the average rate of reaction for the time interval from 0 s to 175 s? average rate of reaction: M/s What is the average rate of reaction for the time interval from 175 s to 446 s? average rate of reaction: M/s What is the average rate of reaction for the time interval from 446 s to 825 s? average rate of reaction: M/s