When formic acid is heated, it decomposes to hydrogen and carbondioxide in a fir

Question

When formic acid is heated, it decomposes to hydrogen and carbondioxide 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. A) What is the formic acid pressure (in torr) when the total pressure is 273? Hint: use Dalton's law of partial pressure and the reaction stoichiometry. B) What is the rate constant (ins-1)? C) What is the half-life (in s)

Explanation / Answer

PARTIAL PRESSURE METHOD IS TOO LONG APPLY THIS ONE K*t=Ln(Pinf-Pini /Pinf-Pt) WHERE Pinf=TOTAL PRESSURE AT INFINITY Pini=TOTAL PRESSURE AT TIME T=0 Pt =TOTAL PRESSURE AT TIME T=t

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