If 1.30 g of dry ice (solid carbon dioxide) is placed in an empty balloon, what will be the volume of the balloon at 15.0°C and 740 torr once all of the dry ice has sublimed (i. e., converted to gaseous CO2)?

0.717 L

Explanation:

First, we will calculate the moles corresponding to 1.30 g of carbon dioxide (MW 44.01).

1.30 g × (1 mol/44.01 g) = 0.0295 mol

The pressure, in atm, is:

740 torr × (1 atm/760 torr) = 0.974 atm

The temperature, in Kelvin, is:

15.0°C + 273.15 = 288.2 K

We can find the volume of the gas using the ideal gas equation.

P × V = n × R × T

V = n × R × T / P

V = 0.0295 mol × 0.0821 atm.L/mol.K × 288.2 K / 0.974 atm

V = 0.717 L