A sample of 1.0 mol of a monoatomic ideal gas is taken through a cyclic process of expansion and compression as shown in the figure. What will be the value of $Δ H$ for the cycle as a whole?

0

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1 \times R T

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2 \times R T

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None of these.

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Solution

The correct option is A $0$
The net change in enthalpy in a cyclic process is zero, i.e $Δ H_{c y c l e} = 0$ because it is a state function. In a cyclic process as initial and final states are same so $Δ H_{c y c l e} = 0$ .

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Enthalpy

Standard XII Chemistry

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A sample of 1.0 mol of a monoatomic ideal gas is taken through a cyclic process of expansion and compression as shown in the figure. What will be the value of ΔH for the cycle as a whole?

The correct option is A 0The net change in enthalpy in a cyclic process is zero, i.e ΔHcycle=0 because it is a state function. In a cyclic process as initial and final states are same so ΔHcycle=0.

A sample of 1.0 mol of a monoatomic ideal gas is taken through a cyclic process of expansion and compression as shown in the figure. What will be the value of $Δ H$ for the cycle as a whole?

The correct option is A $0$
The net change in enthalpy in a cyclic process is zero, i.e $Δ H_{c y c l e} = 0$ because it is a state function. In a cyclic process as initial and final states are same so $Δ H_{c y c l e} = 0$ .