When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay:

The rate of reaction is monitored by measuring the total pressure in the reaction container.

Calculate the rate constant and half-life in seconds for the reaction. At the start of the reaction (time = 0), only formic acid is present. (Find the partial pressure of formic acid using Dalton’s law of partial pressure and the reaction stoichiometry to find P_HCOOH at each time.)

Transcribed Image Text:

HCOOH(g)→CO,(g)+H,(g)