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..22050..324100.379150.408200.423250.431300.435 At the start of the reaction (time =0 ), only formic acid is present. What is the formic acid pressure (in totr) when the total pressure is 375 ? Hint use Dalton's law of partial pressure and the reaction stoichiometry. What is the rate constant (in 51 )? (To determine the rate, you must use a reactant concentration or pressure. Use the procedure of in the previous question to determine the HCOOH pressure as a function of the total pressure.) Answer: What is the half-life (in s)