Identify the correct equation relating enthalpy $(H)$ and internal energy $(E)$.
- A$E_2 - E_1 - H_2 + H_1 = n_2RT - n_1RT$
- B$E_2 - E_1 - H_2 - H_1 = n_2RT - n_1RT$
- C$H_2 - H_1 - E_2 + E_1 = n_2RT - n_1RT$
- D$H_2 - H_1 - E_2 + E_1 = n_2RT + n_1RT$
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Out of molar entropy $(I)$,specific volume $(II)$,heat capacity $(III)$ and volume $(IV)$,which are extensive properties?
What will be the work done on an ideal gas enclosed in a cylinder,when it is compressed by a constant external pressure,$p_{ext}$ in a single step as shown in the figure? Explain graphically.
Medium
View SolutionFor one mole of an ideal gas,which of these statements must be true?
$(a)$ $U$ and $H$ each depend only on temperature.
$(b)$ Compressibility factor $Z$ is not equal to $1$.
$(c)$ $C_{P,m} - C_{V,m} = R$
$(d)$ $dU = C_V dT$ for any process.
$(a)$ $U$ and $H$ each depend only on temperature.
$(b)$ Compressibility factor $Z$ is not equal to $1$.
$(c)$ $C_{P,m} - C_{V,m} = R$
$(d)$ $dU = C_V dT$ for any process.
Which of the following thermodynamic relations is correct?
DifficultWBJEE 2010
View SolutionCalculate the work done in joule if $2 \ mol$ of an ideal gas expands isothermally from $15.5 \ dm^3$ to $20 \ dm^3$ at a constant external pressure of $1 \ atm$. (in $J$)
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