B. C6H12O3 decomposes by a first order reaction at 225 C to C2H4O. The equation is C6H12O3 (g) → 3 C:H4O (g) The rate constant for this reaction at 225 C is 3.05 X 10 4 /s. If we start with a 0.250 M concentration of CoH12O3, what will its concentration be after 2.00 minutes?

The rate constant for a first order reaction is 0.54 s-1. If a 1.57 M sample reacts for 12 seconds, what concentration (in molarity) will remain?

The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction. 2N2O5 → 4NO2 + O2 The rate constant at a given temperature is found to be 5.25 x 10-4 s-1. If the initial concentration of N2O5 is 0.11 M, what is its concentration after exactly 11 minutes have passed?   Round your answer to 2 decimal places.

The reaction so2cl2(g)→so2(g)+cl2(g) is first order. At 660 k it has a rate contsant of 4.5 X 10^-2 s^-1 Determine the concentration of SO2Cl2 at 15.2 seconds, if the initial concentration is 0.583 M.

At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.00717 s : CICH,CH,CI (g) → CH,CHCI (g) + HCI (g) Suppose a vessel contains CICH,CH,Cl at a concentration of 1.00M. Calculate the concentration of CICH,CH,Cl in the vessel 89.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. |M Ox10 ?

4 At a certain temperature the rate of this reaction is first order in CICH₂CH₂Cl with a rate constant of 6.83 × 10 CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HC1 (g) S Suppose a vessel contains CICH₂CH₂Cl at a concentration of 0.890M. Calculate the concentration of CICH₂CH₂Cl in the vessel 880. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

A valid mechanism for the following overall reaction is given below. Overall reaction: 2 NO (g) + Cl2 (g) → 2 NOCI (g) Step 1: NO (g) + Cl2 (g) → NOCI2 (g) Step 2: NOC12 (g) + NO (g) → 2 NOCI (g) (slow) (fast) What is the rate law for this reaction? Rate = k[NO]?[Cl2] Rate = k[NO][CI] Rate = k[NO][Cl2][NOCI] Rate = k[Cl2][NOC12]

Nitrogen dioxide undergoes thermal decomposition according to the second-order reaction 2 NO2(g) → 2 NO(g) + O2(g). When 0.665 M NO2 is allowed to react for 50.0 seconds, its concentration falls to 0.0954 M. What is the rate constant for the reaction? (in M1s-1)

At a certain temperature the rate of this reaction is second order in CICH₂CH₂Cl with a rate constant of 0.00455 M S -1 CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HC1 (g) Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.11 M. Calculate the concentration of CICH₂CH₂Cl in the vessel 900. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

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