Calculate the total pressure in a mixture of 8 g of dioxygen and 4 g of dihydrogen confined in a vessel of 1 dm 3 at 27°C. R = 0.083 bar dm 3 K – 1 mol – 1 .

Question

Philoid · Accepted Answer

Given:

Mass of dioxygen= 8 g

Mass of dihydrogen= 4 g

Now, molar mass of dioxygen = 32g

Thus, number of moles of dioxygen = 8/32 = 0.25 mole

Also, molar mass of dihydrogen = 2g

Thus, number of moles of dihydrogen = 4/2 = 2 mole

Therefore, total number of moles in the mixture:

= 0.25 + 2 = 2.25 mole

Given: -

V = volume = 1 dm³,

n = number of moles = 2.25 mol

R = universal gas constant = 0.083 bar dm³ K^-1 mol^-1

T = temperature = 27°C = 300 K

Let the total pressure be P.

From ideal gas equation we know that -

PV = nRT

= 56.025 bar.

Hence, total pressure of the mixture is 56.025 bar.

Calculate the total pressure in a mixture of 8 g of dioxygen and 4 g of dihydrogen confined in a vessel of 1 dm3 at 27°C. R = 0.083 bar dm3 K–1 mol–1.

Calculate the total pressure in a mixture of 8 g of dioxygen and 4 g of dihydrogen confined in a vessel of 1 dm³ at 27°C. R = 0.083 bar dm³ K^–¹ mol^–¹.