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A 1.50-mol sample of hydrogen gas is heated at constant pressure from 290 K to 418 K. (a) Calculate the energy transferred to the gas by heat. 5529.6 X KJ (b) Calculate the increase in its internal energy. kJ (c) Calculate the work done on the gas. KJ

A 1.50-mol sample of hydrogen gas is heated at constant pressure from 290 K to 418 K. (a) Calculate the energy transferred to the gas by heat. 5529.6 X KJ (b) Calculate the increase in its internal energy. kJ (c) Calculate the work done on the gas. KJ

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A through breakdown of the three part question would be very helpful as I am stuck.
A 1.50-mol sample of hydrogen gas is heated at constant pressure from 290 K to 418 K. (a) Calculate the energy transferred to the gas by heat. 5529.6 X kJ (b) Calculate the increase in its internal energy. KJ (c) Calculate the work done on the gas. kJ
Transcribed Image Text:A 1.50-mol sample of hydrogen gas is heated at constant pressure from 290 K to 418 K. (a) Calculate the energy transferred to the gas by heat. 5529.6 X kJ (b) Calculate the increase in its internal energy. KJ (c) Calculate the work done on the gas. kJ
Expert Solution
Given:

No of mole of Hydrogen gas, n=1.5 mol

Initial temperature, Ti=290 K

Final temperature, Tf=418 K

So, the change in temperature is, ∆T=Tf-Ti=128 K

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