A sample of methane gas at a pressure of
0.867 atm and a temperature of
21.8°C, occupies a volume of
18.6 L. If the gas is compressed at constant temperature to
9.71 L, the pressure of the gas sample will be
atm.

1.661 atm

Explanation:

Data obtained from the question include:

P1 (initial pressure) = 0.867 atm

V1 (initial volume) = 18.6 L

V2 (final volume) = 9.71 L

P2 (final pressure) =?

Since the temperature is constant, the gas is obeying Boyle's law. Now using the Boyle's law equation P1V1 = P2V2, we can calculate the final pressure as shown below:

P1V1 = P2V2

0.867 x 18.6 = P2 x 9.71

Divide both side by 9.71

P2 = (0.867 x 18.6) /9.71

P2 = 1.661 atm

Therefore, the final pressure of the gas is 1.661 atm

1 a

2 d

3 a

4 c

explanation:

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