A cylinder containing hydrogen gas

AI Thread Summary
To calculate the energy required to raise the temperature of 270 L of hydrogen gas from 0.0°C to 31°C at 10 atm, the ideal gas law (PV = nRT) is used to determine the mass of hydrogen, which is found to be 0.12061 kg. The specific heat capacity is applied in the equation Q = MCΔT, but the initial calculations did not yield correct results. It was noted that the molecular weight of hydrogen is 2 g/mol, indicating a potential error in mass calculation. The discussion highlights the importance of using consistent units and understanding the properties of diatomic gases. Accurate calculations are crucial for determining the energy required in thermodynamic processes.
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Homework Statement



A cylinder contains 270 L of hydrogen gas (H2 at 0.0 C) and a pressure of 10 atm. How much energy is required to raise the temperature of this gas to 31°C? (answer needs to be kJ)

Homework Equations


PV =nRT
and
Q= MCT



The Attempt at a Solution


PV = nRT==> M= .12061 kg
Q = MC T
(.12061)(.014304) (31) ====> also tried using kelvins instead of celsius for temp...neither has worked
 
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hydrogen gas is diatomic.
 
sorry, i don't know what that means. Terrible at physics...
 
The MW of H2= 2 gms so your mass is off by a factor of 2 as well.
 
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