When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay: HCOOH(g) CO2(g) + H2 (g) The rate of reaction is monitored by measuring the total pressure in the reaction container.

Time (s) . . . P (torr) 0 . . . . . . . . . 220 50 . . . . . . . . 324 100 . . . . . . . 379 150 . . . . . . . 408 200 . . . . . . . 423 250 . . . . . . . 431 300 . . . . . . . 435 At the start of the reaction (time = 0), only formic acid is present. What is the formic acid pressure (in torr) when the total pressure is 294? Hint: use Dalton's law of partial pressure and the reaction stoichiometry.