The decomposition of SO2Cl2 SO2Cl2(g) --> SO2(g) + Cl2(g) is order 1 with respect to SO2Cl2 and its half-life (t1/2) is 263 minutes at 300oC. Initially, in a 1.0 L container, the partial pressure of SO2Cl2 is 4.00 kPa. a) What will be the partial pressure of SO2Cl2, SO2 and Cl2 after 10.0 hours?

24.) At 700 °C, hydrogen gas reduces nitric oxide according to the equation 2H2(g) + 2NO(g)  2H2O(g) + N2(g) whichobeys the rate law, Rate = k [H2][NO]2. What is the value of the rate constant, in 1M2⋅h , if the initial rate of thereaction is 0.183 M/h when the initial [H2] = 0.220 M and the initial [NO] = 0.250 M.a. 3.33 b. 0.075 c. 0.003 d. 13.33 e. 15.15

The reaction A(aq) ---> B(aq) + C(aq) is a first order reaction. The half-life of A(aq) is 93.4 s at 25.0oC and its half-life is 71.7 s at 45.0oC. What is its half-life (in s) at 65.0oC?

The decomposition reaction of ammonia gas (NH3) into hydrogen gas (H2) and nitrogen (N2) with a Pt catalyst is a zero order reaction at a temperature of 1130 K (i) rate of reaction = rate constant,(ii) reaction rate depends on ammonia concentration,(iii) the rate of decomposition of ammonia becomes constant when the ammonia has completely reacted,(iv) an increase in gas pressure will change the rate of the reaction. A. (ii) and (iv)B. (i) and (ii)C. (i), (ii) and (iii)D. (ii), (iii) and (iv)E. (i), (iii) and (iv)

In a study of the gas phase decomposition of nitrogen dioxide at 383 °C NO2(9)NO(g) +½ O2(g) the following data were obtained: NO2], M seconds 0.436 0.218 0.109 5.45x10-2 4.78 14.3 33.4 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.436 M is ]s and when the starting concentration is 0.218 M is (2) The average A(1/[NO2]) / At from t= 0 s to t= 4.78 s is The average A(1/[NO,]) / At from t= 4.78 s to t = 14.3 s is (3) Based on these data, the rate constant for this v order reaction is

In a study of the decomposition of hydrogen iodide on a gold surface at 150 °CHI(g)½ H2(g) + ½ I2(g)the following data were obtained: [HI], M 0.573 0.287 0.144 7.20×10-2 seconds 0 520 781 912 Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 0.573 M is s and when the starting concentration is 0.287 M is s.(2)The average rate of disappearance of HI from t = 0 s to t = 520 s is  M s-1.(3)The average rate of disappearance of HI from t = 520 s to t = 781 s is  M s-1.(4)Based on these data, the rate constant for this _______zerofirstsecond order reaction is M s-1.

In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)- →½ H2(g) + ½ I2(g) the following data were obtained: [HI], M seconds 1.48 0.740 0.370 0.185 750 2.25x103 5.25x103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.48 M is 750 s and when the starting concentration is 0.740 M is 1500 S. (2) The average A(1/[HI]) / At from t = 0 s to t = 750 s is M-1 s-1. The average A(1/[HI]) / At from t 750 s to t = 2.25×103 s is M-1 s-1. (3) Based on these data, the rate constant for this 0 order reaction is M-1 s-1.

Consider the hypothetical reaction A(g)  +  B(g)                  C(g) The four containers below represent this reaction being run with different initial amounts of A and B. Assume that the volume of each container is 1.0L. The reaction is second order with respect to A and first order in respect to B. Which of the containers, W,X,Y or Z, would have the greatest reaction rate? Justify your answer.

12.) The reaction: 2NO(g) + Cl₂ (3) 20NCI (3) is second order in NO), first order in Cl₂(3), and third order overall. Compare the initial vale of reachon. mixture. OF 0.02 mol mol with (a) the rate of the reaction when half of the NOA) has been consumed, of a OF NO) and 0.02 of cl₂g in a one-liter container (g) (b) the rate of the reaction when half of the Clz) has been consumed, (c) the rate of the reaction when two-thirds of the NO(g) has been consumed, (d) the initial rate of a mixture OF 0.04 mol OF NO) and 0.02 mol OF Cl₂ ) in one-liter container

c) Calculate its half-life 2. The following data were obtained for the gas-phase decomposition of dinitrogen pentaoxide 2N,O, (g) 4NO, (g) +0; () IN,OJ, (mol / L.) Initial Rate (mol /Ls) 0.0750 8.90 x 104 0.190 2.26 x 10 0.275 3.26 x 10 0.410 4.85 x 10 Defining the rate as -A [N;OJ/A write the rate law and caiculate the value of the rate constant