A 5.0 L air sample at a temperature of -50°C has a pressure of 800.00 mmHg. What the new pressure if the temperature is raised to 100°C and the volume expands to 7.0
L?

956 mmHg

Explanation:

The combined gas law states that P1V1/T1 = P2V2/T2 when moles of gas are constant. We're looking for P2, so solve all of that for P2. Make sure you convert your temperatures to Kelvin by adding 273 to the Celsius temperatures.

P2 = P1V1T2/T1V2

P1 = 800.00 mmHg

V1 = 5.0 L

T2 = 100 + 273 = 373 K

T1 = -50 + 273 = 223 K

V2 = 7.0 L

P2 = (800.00 mmHg)(5.0 L)(373 K) / (223 K)(7.0 K) = 956 mmHg

? you expect us to answer this? ? this is your schoolwork, i don't think we can with this, i think it would considering being

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