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1. A gas that has a volume of 28L, a temperature of 45°C and an unknown pressure has its volume increase to 34L and its temperature decreased to 35°C
If I measure the pressure after the change to be 2.0atm what was the original pressure of the gas?
2. If a gas has a pressure of 450mmHg and a volume of 250L at a temperature of 22.0°C, what would the new temperature be at 750mmHg?
(Give answer in °C)
Pls help this brother out thank you
1. A gas that has a volume of 28L, a temperature of 45°C and an unknown pressure has its volume increase to 34L and its temperature decreased to 35°C
If I measure the pressure after the change to be 2.0atm what was the original pressure of the gas?
2. If a gas has a pressure of 450mmHg and a volume of 250L at a temperature of 22.0°C, what would the new temperature be at 750mmHg?
(Give answer in °C)
Pls help this brother out thank you
Answers & Comments
1. The pressure of a gas can be related to its volume, temperature, and number of particles through the Ideal Gas Law, which states that PV = nRT, where P is pressure, V is volume, n is the number of particles, R is the ideal gas constant, and T is temperature in Kelvin.
Since the number of particles in the gas is constant, we can simplify the equation to:
P1V1 / T1 = P2V2 / T2
where P1, V1, and T1 are the original pressure, volume, and temperature, and P2, V2, and T2 are the final pressure, volume, and temperature.
Substituting the given values, we get:
P1 * 28 / (45 + 273) = 2 * 34 / (35 + 273)
Solving for P1, we get:
P1 = 2 * 34 * (45 + 273) / (35 + 273) / 28
P1 = 2.47 atm
Therefore, the original pressure of the gas was 2.47 atmospheres.
2. The pressure, volume, and temperature of a gas are related by the Ideal Gas Law, which states that PV = nRT, where P is pressure, V is volume, n is the number of particles, R is the ideal gas constant, and T is temperature in Kelvin.
Since the number of particles in the gas is constant, we can simplify the equation to:
P1V1 / T1 = P2V2 / T2
where P1, V1, and T1 are the original pressure, volume, and temperature, and P2, V2, and T2 are the final pressure, volume, and temperature.
Substituting the given values, we get:
450 * 250 / (22 + 273) = 750 * 250 / T2
Solving for T2, we get:
T2 = 750 * 250 * (22 + 273) / (450 * 250) - 273
T2 = 67.22 °C
Therefore, the new temperature would be 67.22 °C at a pressure of 750 mmHg.