A substance is taken through the process $a b c$ as shown in figure. If the internal energy of the substance increases by $5000 J$ and a heat of $2625 c a l$ is given to the system, calculate the value of $J$ .

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Solution

Given that,
$Δ Q = (2625 \times J) J$ ---- conversion of cal to J.

$Δ U = 5000 J$

From the graph,

$Δ W = - 200 \times 10^{3} \times 0.03 = - 6000 J$

Now,
$Δ Q = - Δ W + Δ U$

$\Rightarrow 2625 J = 6000 + 5000$

$J = \frac{11000}{2625} = 4.19 J / c a l$

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A substance is taken through the process abc as shown in figure. If the internal energy of the substance increases by 5000J and a heat of 2625 cal is given to the system, calculate the value of J.

Given that,ΔQ=(2625×J)J ---- conversion of cal to J.ΔU=5000JFrom the graph, ΔW=−200×103×0.03=−6000JNow, ΔQ=−ΔW+ΔU⇒2625J=6000+5000J=110002625=4.19J/cal

A substance is taken through the process $a b c$ as shown in figure. If the internal energy of the substance increases by $5000 J$ and a heat of $2625 c a l$ is given to the system, calculate the value of $J$ .

Given that,
$Δ Q = (2625 \times J) J$ ---- conversion of cal to J.

$Δ U = 5000 J$

From the graph,

$Δ W = - 200 \times 10^{3} \times 0.03 = - 6000 J$

Now,
$Δ Q = - Δ W + Δ U$

$\Rightarrow 2625 J = 6000 + 5000$

$J = \frac{11000}{2625} = 4.19 J / c a l$