Thermodynamics Hydrogen question

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SUMMARY

The discussion focuses on calculating the change in internal energy (delta U) and heat transfer (Q) for hydrogen (H2) in a closed tank under standard conditions. The user correctly applies the ideal gas law (pV = nRT) to determine the number of moles (n) and utilizes the formula delta U = (3/2)nR(delta T) to find the change in internal energy, resulting in a value of 254.9 J. It is confirmed that no work is done by the gas since the volume remains constant during the cooling process.

PREREQUISITES
  • Understanding of the ideal gas law (pV = nRT)
  • Familiarity with the first law of thermodynamics
  • Knowledge of specific heat capacities for gases
  • Basic concepts of internal energy and heat transfer
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  • Study the first law of thermodynamics in detail
  • Learn about specific heat capacities of different gases
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smiljanic997
1.The problem statement:
Hydrogen (H2) is at standard conditions in a closed tank, V = 5l, and then it's cooled down for 55K. Find delta U and Q.

2. Questions:
If it says standard conditions, can I just use pV = nRT to find n and then deltaU = j/2*nR(delta)T? Also, is there any work that a gas does, if the V is constant?
I'm a bit confused about certain terms here, so I'd like someone to explain it to me, as I'm preparing for an exam at university.Now, I've done some work and my result for U was 254.9J, but I don't know if I'm correct here.
 
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smiljanic997 said:
1.The problem statement:
Hydrogen (H2) is at standard conditions in a closed tank, V = 5l, and then it's cooled down for 55K. Find delta U and Q.

2. Questions:
If it says standard conditions, can I just use pV = nRT to find n and then deltaU = j/2*nR(delta)T? Also, is there any work that a gas does, if the V is constant?
I'm a bit confused about certain terms here, so I'd like someone to explain it to me, as I'm preparing for an exam at university.Now, I've done some work and my result for U was 254.9J, but I don't know if I'm correct here.
I confirm your answer.
 

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