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# At standard temperature and pressure, carbon dioxide has a density of 1.98 kg/m3...?

What volume does 1.70 kg of carbon dioxide occupy at standard temperature and pressure?

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- Anonymous9 years agoFavorite Answer
dk

- 9 years ago
PV=nRT

n is the number of moles. There are 30 grams per mole of CO2. 1.7 kg of CO2 is 1700 g. 1700/30 = 56.67 moles of CO2.

R is a constant .082

T = 25C= 298K

P = 1

Solve for V

V=nRT/P = (56.67 x .082 x 298)/1 = 1385 liters

- Andrew SmithLv 79 years ago
1.70 kg / 1.98 kg/m^3

= 1.70/1.98 kg * m^3 / kg ( to divide by a fraction invert it and multiply )

= 0.859 m^3

The units guide you to the correct formula!

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