7. Given a 32.0 g sample of methane gas (CH), determine the pressure that would be exerted on a container with a volume of 850 cm at a temperature of 30 °C. Note: Carbon = 12.0 and Hydrogen = 1.0

P = 58.52 atm

Explanation:

Given data:

Mass of sample = 32.0 g

Pressure of sample = ?

Volume of gas = 850 cm³

Temperature of gas = 30°C

Solution:

Number of moles of gas:

Number of moles = mass/molar mass

Number of moles = 32.0 g/ 16 g/mol

Number of moles = 2 mol

Pressure of gas:

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

Now we will convert the temperature.

30+273 = 303 K

850 cm³ × 1L /1000 cm³ = 0.85 L

by putting values,

P× 0.85 L = 2 mol × 0.0821 atm.L/ mol.K  × 303 K

P = 49.75 atm.L/ 0.85 L

P = 58.52 atm

1.solid

2.carbon dioxide

3.helium