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Standard XII

Chemistry

Introduction

An ideal gas ...

Question

An ideal gas is taken through a cyclic thermo dynamical process through four steps. The amounts of heat involved in steps are
$Q_{1} = 5960 J, Q_{2} = - 5585 J, Q_{3} = - 2980 J, Q_{4} = 3645 J$ ; respectively, the corresponding works involved are $W_{1} = 2200, W_{2} = - 825 J, W_{3} = - 1100 J$ and $W_{4}$ respectively. Find the value of $W_{4}$ and efficiency of the cycle

1315 J, 10%

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765 J, 11%

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both of them

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none of these

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Solution

The correct option is B 765 J, 11%
Given;-
$\begin{matrix} Q_{1} = 5960 J, W_{1} = 2200 J Q_{2} = 5585 J, W_{2} = 825 J Q_{3} = 2980 J, W_{3} = 1100 J Q_{4} = 3645 J, W_{4} = f i n d η = f i n d \end{matrix}$
In cycic process $Δ U = 0$
$A / q$ $1 s t$ law of thermodynamics
$Δ Q = Δ U + W$
$\Rightarrow + 1040 = 275 + W_{4}$
$\Rightarrow W_{4} = 1040 - 275$
$= 765$
$η % = \frac{o u t p u t}{i n p u t} \times 100$

$= \frac{1040}{5960 + 3645}$

$= \frac{208}{1321} \times 100$
Hence, we get
$η = 10.82 %$

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Similar questions

Q. An ideal gas is taken through a cyclic thermodynamic process involving four steps. The amounts of heat involved in these steps are

Q_{1} = 5960 J, Q_{2} = - 5585 J, Q_{3} = - 2980 J

and

Q_{4} = 3645 J

, respectively. The corresponding amounts of work done are

W_{1} = 2200 J, W_{2} = - 825 J

and

W_{3} = - 1100 J

and

W_{4} = r e s p e c t i v e l y

.
Find the value of

W_{4}

Q. An ideal gas is taken through a cyclic thermodynamic process through four steps. The amounts of heat involved in these steps are

Q_{1} = 5960 J

Q_{2} = - 5585 J

Q_{3} = - 2980 J

and

Q_{4} = 3645 J

respectively. The corresponding works involved are

W_{1} = 2200 J

W_{2} = - 825 J

W_{3} = - 1100 J

and

W_{4}

respectively.
What is the efficiency of the cycle?

An ideal gas is taken through a cyclic thermodynamic process through four steps. The measures of heat involved in these steps are: $Q_{1} = 5960 J, Q_{2} = - 5585 J, Q_{3} = - 2980 J$ and $Q_{4} = 3645 J,$ respectively. The corresponding quantities of work involved are $W_{1} = 2200 J, = W_{2} = - 825 J$ and $W_{3} = 1100 J$ respectively.

The value of $W_{4}$ ( in $J$ ) is:

(write the absolute value of an answer)

Q. An ideal gas is taken through a cyclic thermodynamic process involving four steps. The amounts of heat involved in these steps are

Q_{1} = 5960 J, Q_{2} = - 5585 J, Q_{3} = - 2980 J

and

Q_{4} = 3645 J

, respectively. The corresponding amounts of work done are

W_{1} = 2200 J, W_{2} = - 825 J

and

W_{3} = - 1100 J

and

W_{4} = r e s p e c t i v e l y

.
What is the efficiency of the cycle?

An ideal gas is taken through a cyclic thermodynamical process through four steps $Q_{1}$ = 5960J, $Q_{2}$ = –5585J, $Q_{3}$ = –2980J and $Q_{4}$ = 3645J, respectively. The corresponding works involved are $W_{1} = 2200 J, W_{2} = - 825 J, W_{3} = - 1100 J$ and $W_{4}$ respectively. The value of W4 is:

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The correct option is B 765 J, 11%Given;-Q1=5960J,W1=2200JQ2=5585J,W2=825JQ3=2980J,W3=1100JQ4=3645J,W4=findη=findIn cycic process ΔU=0A/q 1st law of thermodynamicsΔQ=ΔU+W⇒+1040=275+W4⇒W4=1040−275=765η%=outputinput×100=10405960+3645=2081321×100Hence, we getη=10.82%