At a certain temperature, the rate of this reaction is first order in H2CO3 with a rate constant of 3.00 s^-1: H2CO3(aq) + H2O(aq) -> CO2(aq). Suppose a vessel contains H2CO3 at a concentration of 1.12 M. Calculate the concentration of H2CO3 in the vessel 0.240 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

Name: at a certain temperature the rate of this reaction is first order in h2co3 with a rate constant of 300s1 h2co3aqh2oaqco2aq suppose a vessel contains h2co3 at a concentration of 112m calculat 48035
Uploaded: 2022-06-15T08:06:02-08:00
Duration: 2 min 19 s
Channel: Shaiju T
Description: at a certain temperature the rate of this reaction is first order in h2co3 with a rate constant of 300s1 h2co3aqh2oaqco2aq suppose a vessel contains h2co3 at a concentration of 112m calculat 48035

          At a certain temperature, the rate of this reaction is first order in H2CO3 with a rate constant of 3.00 s^-1: H2CO3(aq) + H2O(aq) -> CO2(aq).
Suppose a vessel contains H2CO3 at a concentration of 1.12 M. Calculate the concentration of H2CO3 in the vessel 0.240 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

Added by Sandra A.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Shaiju T

06/15/2022

Step 1

240 seconds using the first-order rate law equation: \[ [A]_t = [A]_0 \times e^{-kt} \] where: [A]_t = concentration of H2CO3 after time t [A]_0 = initial concentration of H2CO3 (1.12 M) k = rate constant (3.00 s^-1) t = time (0.240 seconds) Show more…

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At a certain temperature, the rate of this reaction is first order in H2CO3 with a rate constant of 3.00 s^-1: H2CO3(aq) + H2O(aq) -> CO2(aq). Suppose a vessel contains H2CO3 at a concentration of 1.12 M. Calculate the concentration of H2CO3 in the vessel 0.240 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.