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?
- Anonymous9 years agoFavorite Answer
- 9 years ago
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!