During the adiabatic expansion of 2 textm texto textl of an ideal gas, the increase in internal energy was found to be equal to (.-200 textJ.) . The work done by the gas during the process will be equal to

Question

During the adiabatic expansion of 2 textm texto textl of an ideal gas, the increase in internal energy was found to be equal to (.-200 textJ.) . The work done by the gas during the process will be equal to (A) 0 (B) 400 textJ (C) -200 textJ (D) 200 textJ

Tardigrade Admin · Accepted Answer

According to first law of thermodynamics, Δ Q=Δ U+Δ W ...(i) Given, Δ U=-200 textJ Δ Q=0 (due to adiabatic process) Substituting in Equation (i), we get 0=-200+Δ W Longrightarrow Δ W=200 textJ

Q. During the adiabatic expansion of $2 m o l$ of an ideal gas, the increase in internal energy was found to be equal to $(- 200 J)$ . The work done by the gas during the process will be equal to

$0$

$400 J$

$- 200 J$

$200 J$

According to first law of thermodynamics,
$Δ Q = Δ U + Δ W$ ...(i)
Given, $Δ U = - 200 J$
$Δ Q = 0$ (due to adiabatic process)
Substituting in Equation (i), we get
$0 = - 200 + Δ W$
$⟹ Δ W = 200 J$

Q. During the adiabatic expansion of 2mol of an ideal gas, the increase in internal energy was found to be equal to (−200J) . The work done by the gas during the process will be equal to

0

400J

−200J

200J

According to first law of thermodynamics, ΔQ=ΔU+ΔW ...(i) Given, ΔU=−200J ΔQ=0 (due to adiabatic process) Substituting in Equation (i), we get 0=−200+ΔW ⟹ΔW=200J

Q. During the adiabatic expansion of $2 m o l$ of an ideal gas, the increase in internal energy was found to be equal to $(- 200 J)$ . The work done by the gas during the process will be equal to

$0$

$400 J$

$- 200 J$

$200 J$

According to first law of thermodynamics,
$Δ Q = Δ U + Δ W$ ...(i)
Given, $Δ U = - 200 J$
$Δ Q = 0$ (due to adiabatic process)
Substituting in Equation (i), we get
$0 = - 200 + Δ W$
$⟹ Δ W = 200 J$