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 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})

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} 4

27^{o} C

is ?

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Calculate the total pressure in mixture of 8 g of dioxygen and 8 g of dihydrogen confined in a vessel of 1 dm3 at 27 oC. [Take R=0.083 bar dm3 K−1 mol−1]

The correct option is B 105.82 barAccording to ideal gas equation,PT.V=nTRT⇒PT=nTRTV Here, we have 8 g of dioxygen and 8 g of dihydrogen Therefore total number of moles, nT=nO2+nH2 =832+82=4.25 ∴P=4.25×0.083×3001=105.82 bar

Calculate the total pressure in mixture of $8 g$ of dioxygen and $8 g$ of dihydrogen confined in a vessel of $1 {dm}^{3}$ at $27^{o} C$ .
[Take $R = 0.083 {bar dm}^{3} K^{- 1} {mol}^{- 1}$ ]