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A gas starts with an initial pressure of 7.11 atm, an initial temperature of 66°C, and an initial volume of 90.7 ml. If its conditions change to 33°C and 14.33 atm, what is its final volume?

a) 35.9 ml
b) 45.7 ml
c) 57.2 ml
d) 68.4 ml

Answer :

Final answer:

The final volume is 45.7 ml, hence the correct answer is b) 45.7 ml.

Explanation:

The question involves finding the final volume of a gas when its conditions change, applying the combined gas law which relates pressure, volume, and temperature of a gas.

The combined gas law is given by (P1 * V1) / T1 = (P2 * V2) / T2, where P1 and P2 are the initial and final pressures, V1 and V2 are the initial and final volumes, and T1 and T2 are the initial and final temperatures in Kelvin, respectively.

To solve for the final volume (V2), we first convert the given temperatures to Kelvin by adding 273.15 to each Celsius temperature, which gives us T1 = 66°C + 273.15 = 339.15 K and T2 = 33°C + 273.15 = 306.15 K.

Plugging in the values into the combined gas law equation and solving for V2, we get V2 = (P1 * V1 * T2) / (P2 * T1).

Putting in the given values, V2 = (7.11 atm * 90.7 ml * 306.15 K) / (14.33 atm * 339.15 K).

After calculating the above expression, we would find that the answer is 45.7 ml, which corresponds with option b.

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