Question

Use the ideal gas calculate the properties of a gas samle as indicated below. Use the value for the gas constant R=0.08205 l x at/mol x K.

Calculate the volume occupied by a 3.50 grams sample of CO₂ gas at a temperature of 37.5 Celsius and a pressure of 1726 torr.

A 57.00 gram sample of argon gas is held in a 7.00 L container. At what temperature (Celsius) will the same pressure in the container equal 14.80 atmospheres?

Answer 1

Answer – We are given, mass of CO₂ = 3.50 g , T = 37.5^oC + 273 = 310.5 K

P = 1726 torr / 760 torr = 2.27 atm

First we need to calculate the moles of CO₂

Moles of CO₂ = 3.50 g / 44.0 g.mol^-1

                       = 0.0795 moles

We know Ideal gas law

PV =nRT

So, V = nRT/P

          = 0.0795 moles * 0.0821 L.atm.mol^-1.K^-1 * 310.5 K / 2.27 atm

           = 0.893 L

          = 893 mL

Given, mass of Ar = 57.00 g , volume = 7.00 L, , P = 14.80 atm

Moles of Ar = 57.00 g / 39.948 g.mol^-1

                    = 1.43 moles

We know Ideal gas law

PV =nRT

So, T = PV/nR

          = 14.80 atm * 7.00 L / 1.43 moles * 0.0821 L.atm.mol^-1.K^-1

          = 884.4 K

So temp, in degree Celsius = 884.4 – 273.15

                                            = 611.2 ^oC