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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

Expert Solution

Given:

No of mole of Hydrogen gas, $n = 1.5 m o l$

Initial temperature, $T_{i} = 290 K$

Final temperature, $T_{f} = 418 K$

So, the change in temperature is, $∆ T = T_{f} - T_{i} = 128 K$

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