The molar specific heat of oxygen at constant pressure is Cp= text7.03 cal mol- 1 K- 1 and R=8.31 J text mol text-1 textK text-1 . The amount of heat taken by 5 moles of oxygen, when heated at constant volume from 10 ° C to 20 ° C, will be approximately

Question

The molar specific heat of oxygen at constant pressure is Cp= text7.03 cal mol- 1 K- 1 and R=8.31 J text mol text-1 textK text-1 . The amount of heat taken by 5 moles of oxygen, when heated at constant volume from 10 ° C to 20 ° C, will be approximately (A) 25 cal (B) 50 cal (C) 253 cal (D) 500 cal

Tardigrade Admin · Accepted Answer

Given, Cp=7.03 cal mol- 1 K- 1 ,R=8.315 J mol- 1 K- 1 n=5 moles , T2=20 oC, T1=10 oC, Δ Q= ? ∴ Heat, Δ Q=nCVΔ T =n(Cp - R)Δ T [∵ Cp - Cv = R] =5[7.03 - (8.31/4.2)]× (20 - 10) ∼ eq253 cal

Q. The molar specific heat of oxygen at constant pressure is $C_{p} = 7.03 c a l m o l^{- 1} K^{- 1}$ and $R = 8.31 J mol^{-1} K^{-1}$ . The amount of heat taken by $5$ moles of oxygen, when heated at constant volume from $10^{\circ} C$ to $20^{\circ} C,$ will be approximately

$25 c a l$

$50 c a l$

$253 c a l$

$500 c a l$

Q. The molar specific heat of oxygen at constant pressure is Cp​=7.03calmol−1K−1 and R=8.31J mol-1K-1 . The amount of heat taken by 5 moles of oxygen, when heated at constant volume from 10∘C to 20∘C, will be approximately

25cal

50cal

253cal

500cal

Given, Cp​=7.03calmol−1K−1,R=8.315Jmol−1K−1 n=5moles , T2​=20oC,T1​=10oC, ΔQ=? ∴ Heat, ΔQ=nCV​ΔT =n(Cp​−R)ΔT [∵Cp​−Cv​=R] =5[7.03−4.28.31​]×(20−10) ∼eq253cal

Q. The molar specific heat of oxygen at constant pressure is $C_{p} = 7.03 c a l m o l^{- 1} K^{- 1}$ and $R = 8.31 J mol^{-1} K^{-1}$ . The amount of heat taken by $5$ moles of oxygen, when heated at constant volume from $10^{\circ} C$ to $20^{\circ} C,$ will be approximately

$25 c a l$

$50 c a l$

$253 c a l$

$500 c a l$