calculate the total pressure of a mixture of 8grams of O2 and 4grams of H2 and enclosed in a vessel of 1 dm^3 at 27°C ?
Given that R = 0.083 bar dm^3 K^-1 mol^-1

Open in App

Solution

Given,

Mass of oxygen = 8 g, molar mass of oxygen = 32 g/mol

Mass of hydrogen = 4 g, molar mass of hydrogen = 2 g/mol

Therefore amount of oxygen = 8/ 32 = 0.25 mol

And amount of hydrogen = 4/2 = 2 mol

From the gas equation PV = n RT, we get,

P X 1 = (0.25 + 2) X 0.083 X 300 = 56.02 bar

Hence, the total pressure of the mixture is 56.02 bar.

Suggest Corrections

Similar questions

Q. 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

^{\circ} C

. (R = 0.083 bar dm

^{3}

^{- 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.

Q. Calculate the total pressure in mixture of

8 g

of dioxygen and

8 g

of dihydrogen confined in a vessel of

1 {dm}^{3}

27^{o} C

.
[Take

R = 0.083 {bar dm}^{3} K^{- 1} {mol}^{- 1}

]

Q. The total pressure in a mixture of 8 g of dioxygen and 4 g of dihydrogen confined in a vessel of 1

{d m}^{3}

27^{o} C

is :

(R = 0.083 bar dm

^{3}

^{- 1}

mol

^{- 1}

)

Calculate the total pressure of a mixture of 8 g of oxygen and 4g of hydrogen confined in vessel of

1 d m^{3}

27^{0} C

(R = 0.083 b a r d m^{3} k^{- 1} {m o l}^{- 1})

Join BYJU'S Learning Program

calculate the total pressure of a mixture of 8grams of O2 and 4grams of H2 and enclosed in a vessel of 1 dm^3 at 27°C ? Given that R = 0.083 bar dm^3 K^-1 mol^-1

calculate the total pressure of a mixture of 8grams of O2 and 4grams of H2 and enclosed in a vessel of 1 dm^3 at 27°C ?
Given that R = 0.083 bar dm^3 K^-1 mol^-1