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The temperature of a gas at pressure p and volume V is 27 degree Celsius keeping it volume constant if its temperature is raised to 927 degree Celsius then its pressure will be?
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The temperature of a gas at pressure p and volume V is 27 degree Celsi...
Understanding the Problem
When a gas is heated at constant volume, its pressure changes according to Gay-Lussac's law, which states that the pressure of a gas is directly proportional to its absolute temperature (in Kelvin).
Initial Conditions
- Initial Temperature (T1) = 27°C = 300 K (converted to Kelvin)
- Initial Pressure (P1) = p
- Final Temperature (T2) = 927°C = 1200 K (converted to Kelvin)
Applying Gay-Lussac's Law
The relationship can be expressed as:
- P1/T1 = P2/T2
Where:
- P2 is the final pressure we need to find.
Calculating Final Pressure
1. Rearranging the formula gives us:
P2 = P1 * (T2/T1)
2. Substituting the values:
P2 = p * (1200 K / 300 K)
3. Simplifying the expression:
P2 = p * 4
Conclusion
The final pressure after raising the temperature to 927°C while keeping the volume constant will be:
- Final Pressure (P2) = 4p
Thus, the pressure of the gas will quadruple when the temperature is increased from 27°C to 927°C at constant volume.
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The temperature of a gas at pressure p and volume V is 27 degree Celsius keeping it volume constant if its temperature is raised to 927 degree Celsius then its pressure will be?
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