An ideal gas initially at $30 K$ undergoes an isobaric expansion at $2.50 k P a$ . If the volume increases from $1.00 m^{3}$ to $3.00 m^{3}$ and $12.5 k J$ is transferred to the gas by heat, What is the change in its internal energy?

7500 J

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7000 J

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700 J

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750 J

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Solution

The correct option is A $7500 J$
in an isobaric process, pressure remains constant
According to first Law of thermodynamics :
$Δ Q = Δ U + Δ W$
$Δ Q = Δ U + P Δ V$ $∵$ P = constant
$Δ U = Δ Q - P Δ V$
$Δ Q = 12.5 k J$ , $Δ V = (3 - 1) m^{3}$ , $P = 2.5 k P a$
so $Δ U = 12500 J - 2 \times 2500 J$
$Δ U = 7500 J$

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An ideal gas initially at 30K undergoes an isobaric expansion at 2.50 kPa. If the volume increases from 1.00 m3 to 3.00 m3 and 12.5 kJ is transferred to the gas by heat, What is the change in its internal energy?

The correct option is A 7500 J in an isobaric process, pressure remains constant According to first Law of thermodynamics :ΔQ=ΔU+ΔWΔQ=ΔU+PΔV ∵ P = constantΔU=ΔQ−PΔVΔQ=12.5 kJ, ΔV=(3−1)m3, P=2.5 kPaso ΔU=12500J−2×2500JΔU=7500J

An ideal gas initially at $30 K$ undergoes an isobaric expansion at $2.50 k P a$ . If the volume increases from $1.00 m^{3}$ to $3.00 m^{3}$ and $12.5 k J$ is transferred to the gas by heat, What is the change in its internal energy?