When an ideal gas undergoes an adiabatic change causing a temperature change of $Δ$ T, then which of the following statements are correct
(i) there is no heat gained or lost by the gas
(ii) the work done by the gas is equal to change in internal energy.
(iii) the change in internal energy per mole of the gas is $C_{v} \times Δ T$ , where $C_{v}$ is the molar heat capacity at constant volume

(i), (ii), (iii)

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(i), (ii)

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(i), (iii)

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(i)

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Solution

The correct option is B (i), (ii)
In adiabatic process Q = 0
$∴$ No heat is gained or lost,
$△ v = Q - W$
$Q = 0$
$∴ △ V = W$
Change in internal energy cannot be calculated.
Directly, we used to use the first law of thermadyherin, which here given.
$△ v = W$
ANSWER : (B).

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(b) Keeping the volume constant and

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The correct option is B (i), (ii)In adiabatic process Q = 0∴ No heat is gained or lost,△v=Q−WQ=0∴△V=WChange in internal energy cannot be calculated.Directly, we used to use the first law of thermadyherin, which here given.△v=WANSWER : (B).

The correct option is B (i), (ii)
In adiabatic process Q = 0
$∴$ No heat is gained or lost,
$△ v = Q - W$
$Q = 0$
$∴ △ V = W$
Change in internal energy cannot be calculated.
Directly, we used to use the first law of thermadyherin, which here given.
$△ v = W$
ANSWER : (B).