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BVP Medical BVP Medical Solved Paper-2014

  • question_answer
    40 cal of heat is required to raise the temperature of 2 mol of an ideal gas at constant pressure from \[64V,\,\,2\Omega \] to \[15min\]. The amount  of heat required to raise the     temperature of the same. Sample of the gas     through the same range of temperature  (\[20\text{ }min\]to\[7.5min\] ) at constant volume will be (gas constant = 2 cal/mol)

    A)  \[25min\]                          

    B)  \[\frac{\omega M}{M+m}\]

    C)  \[\frac{\omega (M-2M)}{M+2m}\]                        

    D)  \[\frac{\omega (M+2M)}{M}\]

    Correct Answer: B

    Solution :

                    Heat at constant pressure \[{{Q}_{p}}=m{{c}_{p}}\Delta \theta \] Heat at constant volume                 \[{{Q}_{V}}=m{{c}_{V}}\Delta \theta \]                 \[{{Q}_{p}}-{{Q}_{V}}=M({{C}_{P}}-{{C}_{V}})\Delta \theta \]                 \[70-{{Q}_{V}}=mR\Delta \theta \]                 \[70-{{Q}_{V}}=2\times 2(35-30)\]                 \[70-{{Q}_{V}}=20\]                 \[{{Q}_{V}}=70-20=50cal\]


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