Question

Tricia puts 44 g of dry ice (solid CO2) into a 2.0-L container and seals the top. The dry ice turns to gas at room temperature (20°C) Find the pressure increase in the 2.0-L container. (One mole of CO2 has a mass of 44 g, R = 0.0821 L×atm/molxK. Ignore the initial volume of the dry ice.)
A) 6 atm
B) 18 atm
C) 2 atm
D) 12 atm

Answer 1

Answer:

Corect answer is D

Explanation:

Assuming that the  C O 2  gas is behaving ideally, therefore, we can use the ideal gas law to find the pressure increase in the container by:

P V=nRT ⇒  P=n R T /V

n=no of moles of the gas = mass/molar mass

Molar mass o f  C O 2=44g/mol, mass = 44g

mole n = 1mole

T=20C=293K

R=0.0821L.atm/mol.K

P=nRT/V

P = 1 x 0.0821 x 293/2

P = 12atm