How would you find the number of grams of CO2 that exert a pressure of 785 torrs at a volume of 32.5 L and a temperature of 32 degrees C?

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Answer 1 · 2018-06-06T09:55:33

$"58.96 g"$

Use ideal gas equation

$"PV = nRT"$

$"n" = "PV"/"RT"$

$color(white)("n") = "785 torr × 32.5 L"/"62.36 L torr / mol K × (32 + 273) K"$

$color(white)("n") = 1.34\ "mol"$

Mass of $"CO"_2$ is

$"m" = 1.34 cancel"mol" × 44 "g"/cancel"mol" = "58.96 g"$