Question

What is the pressure of 62.76 g of carbon dioxide (CO2) gas if it occupies a volume of

Answer 1

Answer:

P = 995.6 atm

Explanation:

assuming ideal gas:

• PV = RTn

∴ Tst = 25°C ≅ 298 K

∴ V = 35.00 mL = 0.035 L

∴ molar mass CO2 = 44.01 g/mol

∴ mass CO2(g) = 62.76 g

⇒ mol CO2(g) = (62.76 g)*(mol/44.01 g) = 1.426 mol

∴ R = 0.082 atm.L/K.mol

⇒ P = RTn/V

⇒ P = ((0.082 atm.L/K.mol)*(298 K)*(1.426 mol)) / (0.035 L)

⇒ P = 995.6 atm

Answer 2

Answer:

The pressure of the carbon dioxide (CO2) gas is 0.913 atm

Explanation:

Step 1: Data given

Mass of carbon dioxide (CO2) = 62.76 grams

Molar mass of carbon dioxide (CO2) = 44.01 g/mol

Volume = 35000 mL = 35 L

Standard temperature = 273 K

Step 2: Calculate moles CO2

Moles CO2 = mass CO2 / molar mass

Moles CO2 = 62.76 grams / 44.01 g/mol

Moles CO2 = 1.426 moles

Step 3: Calculate the pressure

p*V = n*R*T

⇒with p = the pressure of the gas

⇒with V = the volume of the gas = 35 L

⇒with n = the moles of the gas = 1.426 moles

⇒with R = the gas constant = 0.08206 L*atm/mol *K

⇒with T = the temperature = 273 K

p = (n*R*T) / V

p = (1.426 * 0.08206 * 273) / 35

p = 0.913 atm

The pressure of the carbon dioxide (CO2) gas is 0.913 atm