A reaction obeys the following rate law: Rate = k [A]2 (k = 0.00813 M¹5¹) Initially, a vessel contains A at a concentration of 2.40 M. Determine how long it takes for the concentration of A to decrease by 58.0%. (that is, 58.0% of A are consumed.) Round your answer to two significant figures. O 52 s 25 s 88 s O 37 s 71 s 85 s

When designing a consumer product, it is desirable for it to have a two-year shelf life. Often this means that the active ingredient in the product should not decrease by more than 5% in two years. If the reaction is first order, and the rate constant is: k = 2.56 × 10-2 yr 1, determine the half-life of an active ingredient that has a shelf life of 2.00 years. The half-life of an active ingredient is i yr.

The gas-phase decomposition of NOBr has a k= 0.82 M¹ s1 at 10°C. NOBr(g) → NO(g) + ½ Br₂ (g) rate k[ NOBr]² We start with 0.074 M NOBr in a flask at 10°C. 17T A. How long (in secs) does it take to use up 0.011 M of this NOBr? Only enter the number with no units 2.4

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;

Please don't provide handwritten solution ...

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

A particular first-order reaction has a rate constant of 1.35 x 102 s at 25.0 ° C. What is the magnitude of k at 55.0°C if Ea = 55.5 kJ/mol. 1.05 103 2.67 1065 277 1.35 102 1.65 104

The rate constant for a certain reaction is k = 2.00×10−3 s−1 . If the initial reactant concentration was 0.950 MM, what will the concentration be after 16.0 minutes?