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Answer :
For gas with a molar heat capacity at a constant pressure of 7R/2, where R is the gas constant, the change in state from 25°C and 2.50 atm to 125°C and 6.5 atm is 0.0821 L·atm/(mol·K).
Given:
Number of moles (n) = 2.00 mol
Initial temperature (T1) = 25°C
Initial pressure (P1) = 2.50 atm
Final temperature (T2) = 125°C
Final pressure (P2) = 6.5 atm
Molar heat capacity at constant pressure (C) = 7R/2
To calculate the heat (Q) absorbed or released by the gas, we use the formula Q = nCΔT, where ΔT = T2 - T1.
ΔT = (125°C - 25°C) = 100°C
Substituting the values into the formula, we have:
Q = (2.00 mol) * (7R/2) * (100°C) = 700R mol°C
Therefore, the heat absorbed or released by the gas is 700R mol°C.
Note: The value of R depends on the units used for pressure and volume. If the units are in atm and L, then R = 0.0821 L·atm/(mol·K).
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