At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.141 s H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.290M. Calculate the concentration of H₂CO3 in the vessel 4.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM X

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Using an integrated rate law for a first-order reaction
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.141 s¯¹:
H₂CO3(aq) → H₂O (aq) + CO₂ (aq)
Suppose a vessel contains H₂CO3 at a concentration of 0.290M. Calculate the concentration of H₂CO3 in the vessel 4.40 seconds later. You may assume no
other reaction is important.
Round your answer to 2 significant digits.
M
x10
X
Ś
Transcribed Image Text:Using an integrated rate law for a first-order reaction At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.141 s¯¹: H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.290M. Calculate the concentration of H₂CO3 in the vessel 4.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś
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