Question #d4a17

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Question #d4a17

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Answer 1 · 2017-12-13T13:05:50

Using the Combined gas law and adjusting it to solve for Pressure, I calculate the container will have a pressure of 144.2 Atmospheres. Remember to convert the Celsius temperature to Kelvins!

Explanation:

Since you can't use either Boyle's Law or Charles' Law, the combined gas law would be best for a problem like this:

$\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$ $(P_1V_1)/T_1 = (P_2V_2)/T_2$

The question calls for :
(a) An answer in Atmospheres
(b) Unchanging volume

Because of (a), we will need to readjust the formula to solve for pressure:

$\frac{T_{2} P_{1} V_{1}}{T_{1} V_{2}} = P_{2}$ $(T_2P_1V_1)/(T_1V_2) = P_2$

Since volume is kept constant, $V_{1}$ $V_1$ and $V_{2}$ $V_2$ are equal and thus cancel. Also, you must remember to convert the temperature from Celsius to Kelvins (simply add 273.15 to each of the Celsius temperatures).

$P_{2} = \frac{(338.15 K) (125 A T M)}{293.15 K}$ $P_2 = ((338.15 K)(125 ATM))/(293.15 K)$

$P_{2} = 144.2 A T M$ $P_2 = 144.2 ATM$

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Question #d4a17

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