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Standard XII

Chemistry

Ideal Gas Equation

Calculate the...

Question

Calculate the total pressure of a mixture of 8 g of oxygen and 4g of hydrogen confined in vessel of $1 d m^{3}$ at $27^{0} C$ .
$(R = 0.083 b a r d m^{3} k^{- 1} {m o l}^{- 1})$

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Solution

Moles of $O_{2}$ = $\frac{8}{32}$ = $\frac{1}{4}$
Moles of $H_{2}$ = $\frac{4}{2}$ = 2
Therefore total moles of both gas(n) = $\frac{1}{4} +$ = $\frac{9}{4}$
Given :
V = 1 $d m^{3}$
T = 300 K
$(R = 0.083 b a r d m^{3} k^{- 1} {m o l}^{- 1})$
PV = nRT
P = $(9 \times 0.083 \times 300)$ / $(4 \times 1) = 56.025 b a r$

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Calculate the total pressure of a mixture of 8 g of oxygen and 4g of hydrogen confined in vessel of 1dm3 at 270C.(R=0.083bardm3k−1mol−1)

Moles of O2 = 832 = 14Moles of H2 = 42 = 2Therefore total moles of both gas(n) = 14+ = 94Given :V = 1 dm3T = 300 K(R=0.083bardm3k−1mol−1)PV = nRTP = (9×0.083×300) / (4×1)=56.025 bar

Calculate the total pressure of a mixture of 8 g of oxygen and 4g of hydrogen confined in vessel of $1 d m^{3}$ at $27^{0} C$ .
$(R = 0.083 b a r d m^{3} k^{- 1} {m o l}^{- 1})$