At a certain temperature the rate of this reaction is second order in SO3 with a rate constant of 4.13M *S : 2SO3 (g) → 2SO₂(g) + O₂(g) Suppose a vessel contains SO3 at a concentration of 0.110 M. Calculate the concentration of SO3 in the vessel 7.80 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M ☐ x10 X

Consider the following rate law for the reaction A + B → products. rate = k{A}2{B}2 The reaction is order with respect to A, order with respect to B, and order overall.

Initial rate: 1.6 •10^-7mol/L•s K=6.4 •10^-9L/mol•s Rate law: k[HI]^2 Can you please show me the steps.

Consider this reaction: 2SO3 (g) →2SO₂(g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.894 M¹-s¹) [S0₂] Suppose a vessel contains SO3 at a concentration of 0.390 M. Calculate the concentration of SO3 in the vessel 8.60 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M Explanation Check 0 10 Q Search a Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use O Privacy Center

The reaction of NOBr(g) to form NO(g) and Br2(g) is second order: 2NOBr(g) → 2NO(g) + Br₂(g) The rate constant is 0.556 L mol-¹ s¹ at some temperature. If the initial concentration of NOBr in the container is 0.21 M, how long will it take for the concentration to decrease to 0.028 M? t = S

At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0424 s¯¹: S 2NH3(g) → N₂(g) + 3H₂(g) Suppose a vessel contains NH3 at a concentration of 0.460M. Calculate the concentration of NH3 in the vessel 17.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X 5

Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0022 M⚫s 1: 2 HI (g) →H₂ (g) +12(g) Suppose a 4.0 L flask is charged under these conditions with 250. mmol of hydrogen iodide. How much is left 7.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. X x10

NOBr(g) decomposes to form NO and Br2 by the reaction 2 NOBr(g) + 2 NO(g) + Br2(8) It is found that the reaction is second order in NOBr. The rate constant has been found to be 0.170 M-1 s1. In a situation where the initial concentration of NOBr in a vessel is 0.690 M, how long will it take for the concentration of Br2 to reach 0.180 M? (Assume, of course, that there was no Br in the vessel to begin with.) Report your result in seconds with one decimal place but do not put units in the

After 48 seconds, 10.% of reactant has reacted. If the reaction is a 1st order reaction, the special rate constant k = _.

The following reaction was studied at 25°C. The following results were obtained. a) What is the rate law for this reaction at this temperature? b) What is the value of the rate constant? Be sure to include the correct units in your answer.