A gas mixture contains 0.70 moles of nitrogen gas, 0.20 moles of hydrogen gas, and 0.10 moles of methane (CH4). What is the partial pressure of nitrogen?

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A gas mixture contains 0.70 moles of nitrogen gas, 0.20 moles of hydrogen gas, and 0.10 moles of methane (CH4). What is the partial pressure of nitrogen?

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Answer 1 · 2014-09-24T18:26:07

If the total pressure of the mixture is 1.00 atm, the partial pressure of nitrogen is 0.70 atm.

The partial pressure $P_{i}$ $P_"i"$ of a gas $i$ $i$ is equal to its mole fraction $x_{i}$ $x_i$ times the total pressure $P_{i}$ $P_i$ of the mixture.

$P_{i} = x_{i} P_{tot}$ $P_"i" =x_"i"P_"tot"$ and $x_{i} = \frac{n_{i}}{n_{tot}}$ $x_i = n_"i"/n_"tot"$ .

$n_"tot" = n_"N₂" + n_"H₂" + n_"CH₄"$ = (0.70 + 0.20 + 0.10) mol = 1.00 mol

$x_"N₂" = "0.70 mol"/"1.00 mol"$ = 0.70

$P_"N₂" = x_"N₂"P_"tot"$ = 0.70 × 1.00 atm = 0.70 atm

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A gas mixture contains 0.70 moles of nitrogen gas, 0.20 moles of hydrogen gas, and 0.10 moles of methane (CH4). What is the partial pressure of nitrogen?

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