When $1 \ mole$ of gas is heated at constant volume and heat supplied is $500 \ J$,then which of the following is correct?

  • A
    $\Delta U = -0.5 \ J, q = -500 \ J$
  • B
    $q = -500 \ J, \Delta U = 0$
  • C
    $q = 500 \ J, w = 0$
  • D
    $w = 500 \ J, \Delta U = 0$

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Similar Questions

Based on the first law of thermodynamics,which one of the following is correct?

The volume of an ideal gas contracts from $10.0 \ L$ to $2.0 \ L$ under an applied pressure of $2.0 \ atm$. During contraction,the system also evolved $900 \ J$ of heat. The change in internal energy (in $J$) involved in the system is $(1 \ L \ atm = 101.3 \ J)$:

The first law of thermodynamics is only:

When a certain volume of gas expands against a constant external pressure of $2.40 \times 10^5 \ Pa$ at $300 \ K$ to a final volume of $2.2 \times 10^{-3} \ m^3$. If the work obtained is $-0.048 \ kJ$,what is the initial volume of the gas?

For which of the following processes is $q = \Delta U$?

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