The heat provided to the diatomic gas and monoatomic gas is 1870.65 J and 1122.39 J respectively.
The specific heat of a substance can be defined as the quantity of heat required to raise the temperature of the substance with mass in one unit by one-degree Celcius.
Whenever the heat can be lost or absorbed the substance's temperature will be changed:
Q = m.C.ΔT
Given, the number of moles of the gas, n = 1.8 mol
The change in the temperature, ΔT = 50 K
The molar specific heat at constant volume for the diatomic gas:
[tex]C_v =\frac{5}{2}R[/tex]
Heat provided to the diatomic gas:
[tex]Q = n\times C_v \times \triangle T[/tex]
Q = 1.8 × (5/2) R × 50
Q = 1.8 × (5/2) ×8.314 × 50
Q = 1870.65 J
The molar specific heat at constant volume for the monoatomic gas:
[tex]C_v =\frac{3}{2}R[/tex]
Heat provided to the monoatomic gas:
[tex]Q = n\times C_v \times \triangle T[/tex]
Q = 1.8 × (3/2) R × 50
Q = 1.8 × (3/2) ×8.314 × 50
Q = 1122.39 J
Learn more about specific heat capacity, here:
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