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Which law can be used to calculate the number of moles of a contained gas?
7. Gases
Chemistry Gas Laws
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Consider 4.20 L of a gas at 365 mmHg and 20°C. If the container is compressed to 3.00 L and the temperature is increased to 36°C, what is the new pressure, P2, inside the container? Assume no change in the amount of gas inside.
A
520 mmHg
B
550 mmHg
C
480 mmHg
D
500 mmHg
Verified step by step guidance1
Identify the initial and final conditions of the gas: initial volume (V1) = 4.20 L, initial pressure (P1) = 365 mmHg, initial temperature (T1) = 20°C, final volume (V2) = 3.00 L, and final temperature (T2) = 36°C.
Convert the temperatures from Celsius to Kelvin by adding 273.15 to each: T1 = 20 + 273.15 K and T2 = 36 + 273.15 K.
Use the combined gas law, which is expressed as \( \frac{P1 \cdot V1}{T1} = \frac{P2 \cdot V2}{T2} \), to relate the initial and final states of the gas.
Rearrange the combined gas law to solve for the final pressure (P2): \( P2 = \frac{P1 \cdot V1 \cdot T2}{T1 \cdot V2} \).
Substitute the known values into the equation: P1 = 365 mmHg, V1 = 4.20 L, T1 = 293.15 K, V2 = 3.00 L, and T2 = 309.15 K, and calculate P2.
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