0.345 moles of $C H_{4}$ $CH_4$ is placed in a 15.0 L container at a temperature of 25.2°C. What is the pressure in atm exerted by the gas?

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0.345 moles of $C H_{4}$ $CH_4$ is placed in a 15.0 L container at a temperature of 25.2°C. What is the pressure in atm exerted by the gas?

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Answer 1 · 2016-06-27T10:01:09

Approx. $\frac{1}{2} \cdot atm$ $1/2*"atm"$

Explanation:

$P = \frac{n R T}{V}$ $P=(nRT)/V$ $=$ $=$ $\frac{0.345 \cdot m o l \times 0.00821 \cdot L \cdot a t m \cdot K^{- 1} \cdot m o l^{- 1} \times 298.2 \cdot K}{15.0 \cdot L}$ $(0.345*molxx0.00821*L*atm*K^-1*mol^-1xx298.2*K)/(15.0*L)$

$=$ $=$ $? ? \cdot a t m$ $??*atm$

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0.345 moles of $C H_{4}$ $CH_4$ is placed in a 15.0 L container at a temperature of 25.2°C. What is the pressure in atm exerted by the gas?

1 Answer

Explanation:

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0.345 moles of CH4CH_4 is placed in a 15.0 L container at a temperature of 25.2°C. What is the pressure in atm exerted by the gas?

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0.345 moles of $C H_{4}$ $CH_4$ is placed in a 15.0 L container at a temperature of 25.2°C. What is the pressure in atm exerted by the gas?