Chemistry question!! Please help!

Question

Determine how many liters 8.93 g of carbon dioxide gas would occupy at the following conditions.

A) STP

____ L

B) 110 C and 1.00 atm

______ L

C) 237 K and 147 kPa

______ L

Answer 1

Use the ideal gas equation to solve for each problem.

PV = nRT

P = pressure in units of atm

V = volume in units of Liters

n = # of moles of gas

R = gas constant = 0.0821 L atm mol^-1 K^-1

T = Kelvin temperature

A) STP = standard temperature (0 °C = 273.15 K) and pressure = 1 atm

n = moles = g of CO₂ / molar mass of CO₂ = 8.93 g CO₂ x (1 mol CO₂ / 44 g CO₂) = 0.203 mol CO₂

Rearrange the ideal gas law equation to solve for V...

V = nRT / P = (0.203 mol x 0.0821 L atm mol^-1 K^-1 x 273.15 K) / 1 atm = 4.55 L

B) T = 110 °C + 273.15 = 383.15 K, P = 1.00 atm

V = nRT / P = (0.203 mol x 0.0821 L atm mol^-1 K^-1 x 383.15 K) / 1.00 atm = 6.39 L

C) T = 237 K, P = 147 kPa

1 atm = 101.3 kPa

147 kPa x (1 atm / 101.3 kPa) = 1.45 atm

V = nRT / P = (0.203 mol x 0.0821 L atm mol^-1 K^-1 x 237 K) / 1.45 atm = 2.72 L