A gas sample with a volume of 5.3 l has a pressure of 735 mm hg at 28 c. What is the sample if the volume remains at 5.3 l but the temperature rises to 86 c

876.63 mmHg

Explanation:

Step 1:

Data obtained from the question:

Initial volume (V1) = 5.3 L

Initial pressure (P1) = 735 mmHg

Initial temperature (T1) = 28°C

Final volume (V2) = constant i.e the same as the initial volume (5.3L)

Final temperature (T2) = 86°C

Final pressure (P2) =..?

Step 2:

Conversion of celsius temperature to Kelvin temperature. This is illustrated below:

Temperature (Kelvin) = temperature (celsius) + 273

Initial temperature (T1) = 28°C

Initial temperature (T1) = 28°C +273 = 301K

Final temperature (T2) = 86°C

Final temperature (T2) = 86°C + 273 = 359K

Step 3:

Determination of the new pressure of the gas. This is illustrated below:

Since the volume of the gas is constant, the new pressure of the gas can be obtained by the equation below:

P1/T1 = P2/T2

Initial pressure (P1) = 735 mmHg

Initial temperature (T1) = 301K

Final temperature (T2) = 359K

Final pressure (P2) =..?

P1/T1 = P2/T2

735/301 = P2/359

Cross multiply to express in linear form

301 x P2 = 735 x 359

Divide both side by 301

P2 = (735 x 359)/301

P2 = 876.63 mmHg

Therefore, the new pressure of the gas is 876.63 mmHg

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