NO2(g) + CO(g) → NO(g) + CO2(g) The rate of the above reaction depends only on the concentration of nitrogen dioxide at temperatures below 225°C. At a temperature below 225°C the following data were obtained: Time [NO2] (s) (mol/L) 0.520 1.90x103 0.477 4.75x103 0.424 7.12x103 0.388 1.42x104 0.310 2.85x104 0.220 Which of the following expressions for the rate law (either differential or integrated) are completely consistent with the above experimental data. v 1/[NO2] - 1/[NO2]o = kt v K[CO][NO2] = -d[NO2]/dt v [NO2] = [NO2]o - kt v k[NO2]² = d[NO]/dt v k[NO2]² = -d[CO]/dt Submit Answer Tries 0/99 Calculate the rate constant (k). Enter the numerical value and corresponding units.

Consider following reaction:              2 A2B5(g)  →  4AB2(g) + B2(g) The rate constant is 0.129 s-1 at 298 K for this reaction. What is the percent of A2B5 left after the first 19.091 s? Report your answer with three decimals. Enter numbers only;

The data below were collected for the following reaction at 35° C: 2(CH3)3 CSOH(g) → (CH3)3CS(O)SC(CH3)3 (g) Time (min) [(CH3)3 CSOH] (mol · L−¹) 0.0 1.554 10.8 0.661 19.1 0.343 37.0 0.083 59.5 0.014 75.1 0.004 Part C From the slope of the appropriate plot, determine the value of the rate constant at this temperature. VG ΑΣΦ Submit Request Answer ? 5-1

Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased