A system is provided with $200 \,cal$ of heat and the work done by the system on the surrounding is $40 \,J$. Then its internal energy
AIncreases by $600 J$
BDecreases by $800 J$
CIncreases by $800 J$
DDecreases by $50 J$
Easy
Download our app for free and get started
CIncreases by $800 J$
c (c) $\Delta Q = \Delta U + \Delta W$
$\Delta Q = 200cal = 200 \times 4.2 = 840J$ and $\Delta W = 40J$
==>$\Delta U = \Delta Q - \Delta W = 840 - 40 = 800J$
Download our app
and get started for free
Experience the future of education. Simply download our apps or reach out to us for more information. Let's shape the future of learning together!No signup needed.*
An ideal gas undergoes an adiabatic process obeying the relation $PV^{4/3} =$ constant. If its initial temperature is $300\,\, K$ and then its pressure is increased upto four times its initial value, then the final temperature is (in Kelvin):
$n$ moles of a van der Waals' gas obeying the equation of state $\left(p+\frac{n^2 a}{V^2}\right)(V-n b)=n R T$, where $a$ and $b$ are gas dependent constants, is made to undergo a cyclic process that is depicted by a rectangle in the $p-V$ diagram as shown below. What is the heat absorbed by the gas in one cycle?
A sample of an ideal gas is taken through the cyclic process $abca$ as shown in the figure. The change in the internal energy of the gas along the path $ca$ is $-180\, J$. The gas absorbs $250\, J$ of heat along the path $ab$ and $60\, J$ along the path $bc$. The work done by the gas along the path $abc$ is ..... $J$