In a closed insulated container,a liquid is stirred with a paddle to increase its temperature. In this process,which of the following is true?
- A$ \Delta E = W = Q = 0 $
- B$ \Delta E \neq 0, \ Q = W = 0 $
- C$ \Delta E = W \neq 0, \ Q = 0 $
- D$ \Delta E = Q \neq 0, \ W = 0 $
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Assertion : For a reaction $2NH_{3(g)} \to N_{2(g)} + 3H_{2(g)}$ ; $\Delta H > \Delta E$.
Reason : Enthalpy change is always greater than internal energy change.
Reason : Enthalpy change is always greater than internal energy change.
$A$ system absorbs $600 \ J$ of heat and does work equivalent to $300 \ J$ on its surroundings. The change in internal energy is ...... $J$.
Medium
View Solution$A$ gas absorbs $100 \ J$ of heat and is simultaneously compressed by a constant external pressure of $1.5 \ atm$ from a volume of $8.0 \ L$ to $2.0 \ L$. The change in internal energy for the gas in Joules is $(1 \ L \cdot atm = 101.32 \ J)$.
One mole of an ideal gas performs $900 \ J$ of work on the surroundings. If the internal energy increases by $625 \ J$,find the value of $\Delta H$. (in $J$)
If one mole of ammonia and one mole of hydrogen chloride are mixed in a closed container to form ammonium chloride gas,then
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