Home
Class 11
PHYSICS
Five moles of hydrogen when heated throu...

Five moles of hydrogen when heated through 20 K expand by an amount of `8.3 xx 10^(-3) m^(3)` under a constant pressure of `10^(5) N//m^(2)`. If `C_(v)` = 20 J/mole K, find `C_(P)`.

Text Solution

Verified by Experts

Mayer.s relation `C_(p) - C_(v) = R`
Multiplying throughout by `mu Delta T`
`mu C_(p) Delta T - mu C_(v) Delta T = mu R Delta T`
`mu Delta T (C_(p) - C_(v)) = P Delta T [therefore mu R Delta T = P Delta V]`
`5 xx 20 (C_(p) - 20) = 105 xx 8.3 xx (10-3)`
`[(therefore mu = 5"," Delta T = 20 K","P = 1 xx 10^(5) N//m^(2)),(C_(v) = "20 J/mole K" and Delta V = 8.3 xx 10^(3) M^(3))]`
`C_(p) - 20 = 8.3`
`therefore` Cp = 28.3 J/mole-K
Promotional Banner

Similar Questions

Explore conceptually related problems

Five moles of hydrogen when heated through 20 K expand by an amount of 8.3xx10^(-3)m^(3) under a constant pressure of 10^(5)N//m^(2). " If "C_(v)=20J//"mole"K,"Find"C_(p) .

Two moles of air, when heated through 10 K expands by an amount of 1.66xx10^(-3)m^(3) under a constant pressure of 10^(5) N//m^(2) . If C_(V)=20.81 J/mole K, then C_(P) is ,

Four moles of a gas when heated through 20^(@)C expand by 6.3 xx 10^(-3) m^(3) under a const-ant pressure of 10^(5) N//m^(2) .. If 30 J "mole"^(-1)k^(-1) is C_(v) then the C_(p) in J "mole"^(-1)k^(-1) is,

How much work to be done in decreasing the volume of and ideal gas by an amount of 2.4xx10^(-4)m^(3) and constant normal pressure of 1xx10^(5) N//m^(2)