A sample of a gas occupies $1.40 \cdot 10^{3}$ $1.40 * 10^3$ mL at 25°C and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg?

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A sample of a gas occupies $1.40 \cdot 10^{3}$ $1.40 * 10^3$ mL at 25°C and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg?

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Answer 1 · 2015-12-31T09:49:32

$V = 2.8 L$ $V = 2.8L$

Explanation:

On its initial state, the gas
- occupies $1.4 L$ $1.4L$
- is on a system of $298.15 k$ $298.15k$ , and
- $1 a t m$ $1 atm$

And on its second state,
- $x L$ $x L$
- $298.15 K$ $298.15K$
- $\frac{380}{760} a t m$ $380/760 atm$

$\frac{P_{0} V_{0}}{T_{0}} = \frac{P V}{T}$ $(P_0V_0)/T_0 = (PV)/T$ ,

Solve for V.

$V = 2.8 L$ $V = 2.8L$

The answer is obtainable through Boyle's Law - when temperature is held constant, there exists an inverse correlation factor between the state functions of pressure and volume.

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A sample of a gas occupies $1.40 \cdot 10^{3}$ $1.40 * 10^3$ mL at 25°C and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg?

1 Answer

Explanation:

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A sample of a gas occupies $1.40 \cdot 10^{3}$ $1.40 * 10^3$ mL at 25°C and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg?