Question

If 4.70 LL of CO₂CO₂ gas at 18 °C°C at 793 mmHg is used, what is the final volume, in liters, of the gas at 37°C°C and a pressure of 755 mmHg , if the amount of CO₂ remains the same?

A 125 mL bubble of hot gases at 213°C°C and 1.90 atm is emitted from an active volcano. What is the final temperature, in degrees Celsius, of the gas in the bubble outside the volcano if the final volume of the bubble is 132 mL and the pressure is 0.850 atm , if the amount of gas does not change?

Answer 1

In both queries, we need to apply the ideal gas law while keeping the principal amount of gas constant. The formula used is P1V1/T1 = P2V2/T2, and temperatures must be converted to Kelvin for calculation purposes. The final volume of CO₂ and the final temperature of the gas bubble can thus be evaluated.

Step-by-step explanation:

To answer these questions, we will use the gas laws, which describe how gases behave with changes in volume, pressure, and temperature. In both problems, we are considering a situation where gas amount remains constant, so the ideal gas law can be applied.

For the first question, we will use the formula P1V1/T1 = P2V2/T2 where P is pressure, V is volume, and T is temperature (in Kelvin). After substituting the values and converting temperatures from Celsius to Kelvin by adding 273 to each, the final volume of the CO₂ gas can be calculated.

The second question also applies the same formula but solving for the final temperature. Converting Celsius to Kelvin and substitifying the original values, the final temperature in Kelvin can be obtained. Subtracting 273 from this result will give us the final temperature in Celsius.

Learn more about Gas Laws