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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?

Answer 1

Henry Antrim

#"58.96 g"#

Apply the 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"#

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Answer 2

Cameron Andrews

Use the ideal gas law: PV = nRT. Rearrange to solve for moles (n): n = PV / RT. Convert temperature to Kelvin. Substitute values and solve for moles. Convert moles to grams using the molar mass of CO2 (44.01 g/mol).

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.