Question

A mixture of gases contains 0.31 molCH4,0.25 mol0.31 \mathrm{~mol} \mathrm{CH}_4, 0.25 \mathrm{~mol} C2H6\mathrm{C}_2 \mathrm{H}_6, and 0.29 molC3H80.29 \mathrm{~mol} \mathrm{C}_3 \mathrm{H}_8. The total pressure is 1.501.50 bar. Calculate the partial pressures of the gases.

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a mixture of gases contains 0.31 moles of methane (CH4\mathrm{CH_4}), 0.25 moles of ethane (C2H6\mathrm{C_2H_6}) and 0.29 moles of propane (C3H8\mathrm{C_3H_8}). The total pressure is 1.50 bar. We need to calculate the partial pressures of the gases.

Moles of methane (nCH4n_{\mathrm{CH_4}}) = 0.31  mol\mathrm{0.31\; mol}

Moles of ethane (nC2H6n_{\mathrm{C_2H_6}}) = 0.25  mol\mathrm{0.25\; mol}

Moles of propane (nC3H8n_{\mathrm{C_3H_8}}) = 0.29  mol\mathrm{0.29\; mol}

Total pressure (PtotalP_{\mathrm{total}}) = 1.50  bar\mathrm{1.50\; bar}

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