Given constant volume, what pressure would $50 \cdot a t m$ $50*atm$ of gas at $0$ $0$ $^{\circ} C$ $""^@C$ , develop at a temperature of $300$ $300$ $^{\circ} C$ $""^@C$ ?

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Given constant volume, what pressure would $50 \cdot a t m$ $50*atm$ of gas at $0$ $0$ $^{\circ} C$ $""^@C$ , develop at a temperature of $300$ $300$ $^{\circ} C$ $""^@C$ ?

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Answer 1 · 2015-11-14T20:29:30

Gay Lusaac's law holds that at constant volume, $(\frac{P_{1}}{T_{1}} = \frac{P_{2}}{T_{2}})$ $((P_1)/T_1 = (P_2)/T_2)$ (i.e. pressure is proportional to temperature at constant volume).

Explanation:

So, $P_{2}$ $P_2$ $=$ $=$ $\frac{P_{1} T_{2}}{T_{1}}$ $(P_1T_2)/T_1$ $=$ $=$ $\frac{50.0 \cdot a t m \times 273 K}{573 K}$ $(50.0*atmxx273K)/(573K)$ $=$ $=$

$? ? a t m o s p h e r e s$ $?? atmospheres$

This is reasonable on the basis that we would expect a given quantity of gas to exert less pressure at lower temperature. Note that I converted the temperature to the Kelvin scale in order to avoid multiplying by $0$ $0$ .

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Given constant volume, what pressure would $50 \cdot a t m$ $50*atm$ of gas at $0$ $0$ $^{\circ} C$ $""^@C$ , develop at a temperature of $300$ $300$ $^{\circ} C$ $""^@C$ ?

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Given constant volume, what pressure would $50 \cdot a t m$ $50*atm$ of gas at $0$ $0$ $^{\circ} C$ $""^@C$ , develop at a temperature of $300$ $300$ $^{\circ} C$ $""^@C$ ?