Based on the first law oi thermodynamics, which one of the following is correct?

Question

Based on the first law oi thermodynamics, which one of the following is correct? (A) For an isothermal process, Q=+w (B) For an isochoric process, Δ U=-Q (C) For an adiaoatic process, Δ U =-W (D) For a cyclic process, Q =-w

Tardigrade Admin · Accepted Answer

According to first law of thermodynamics, Δ U=Q+W For cyclic process, change in internal energy =0 ∴ Q=-W

Q. Based on the first law oi thermodynamics, which one of the following is correct?

For an isothermal process, $Q = + w$

For an isochoric process, $Δ U = - Q$

For an adiaoatic process, $Δ U = - W$

For a cyclic process, $Q = - w$

According to first law of thermodynamics,

$Δ U = Q + W$

For cyclic process, change in internal energy

$= 0$

$∴ Q = - W$

Q. Based on the first law oi thermodynamics, which one of the following is correct?

For an isothermal process, Q=+w

For an isochoric process, ΔU=−Q

For an adiaoatic process, ΔU=−W

For a cyclic process, Q=−w

According to first law of thermodynamics, ΔU=Q+W For cyclic process, change in internal energy =0 ∴Q=−W

For an isothermal process, $Q = + w$

For an isochoric process, $Δ U = - Q$

For an adiaoatic process, $Δ U = - W$

For a cyclic process, $Q = - w$

According to first law of thermodynamics,

$Δ U = Q + W$

For cyclic process, change in internal energy

$= 0$

$∴ Q = - W$