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ExtremeBDS [4]
3 years ago
11

A gas has an initial volume of 168 cm3 at a temperature of 255 K and a pressure of 1.6 atm. The pressure of the gas decreases to

1.3 atm, and the temperature of the gas increases to 285 K. What is the final volume of the gas?

Chemistry
2 answers:
katen-ka-za [31]3 years ago
6 0
I wrote the answer on this paper and here is the calculations step by step

very sry the "V" must be replaced with 285 and the 285 must be replaced with "V" and the answer is 231.09 cm3. sorry for the inconvenience.

Brianna bts
2 years ago
it very okay thxs
Anit [1.1K]3 years ago
5 0

<u>Answer:</u> The volume when the pressure and temperature has changed is 231.1cm^3

<u>Explanation:</u>

To calculate the volume when temperature and pressure has changed, we use the equation given by combined gas law. The equation follows:

\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}

where,

P_1,V_1\text{ and }T_1 are the initial pressure, volume and temperature of the gas

P_2,V_2\text{ and }T_2 are the final pressure, volume and temperature of the gas

We are given:

P_1=1.6atm\\V_1=168cm^3\\T_1=255K\\P_2=1.3atm\\V_2=?cm^3\\T_2=285K

Putting values in above equation, we get:

\frac{1.6atm\times 168cm^3}{255K}=\frac{1.3atm\times V_2}{285K}\\\\V_2=231.1cm^3

Hence, the volume when the pressure and temperature has changed is 231.1cm^3

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Substitute the values into above formula as follows.

\frac{P_{1}V_{1}}{T_{1}} = \frac{P_{2}V_{2}}{T_{2}}\\\frac{985 torr \times 105 L}{300 K} = \frac{760 torr \times V_{2}}{273 K}\\V_{2} = \frac{94116.75}{760} L\\= 123.84 L

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