Calculate Delta U and Delta H in calories 1 mole of a monoatomic ideal gas is heated constant pressure of 1 atm from 25-oC to 50-oC-

Question

Toppr Admin · Accepted Answer

For monoatomic ideal gas- Cv-32RCp-x394-H-x394-T-x2234-x394-H-Cp-x394-T-xA0-mol-x2212-1 - or nCp-x394-T for n moles -52-xD7-1-987-xD7-25-124-2-xA0-calWork done- w-x2212-P-x394-V-x2212-P-V2-x2212-V1-x2212-PV2-x2212-PV1-x2212-nRT2-x2212-nRT1-x2212-mR-T2-x2212-T1-x2212-1-xD7-1-987-323-x2212-298-xA0-cal-x2212-49-7-xA0-cal-x394-E-q-w-124-2-x2212-49-7-xA0-cal-74-5-xA0-cal-

Calculate ΔU and ΔH in calories if 1 mole of a monoatomic ideal gas is heated at constant pressure of 1 atm from 25oC to 50oC.

For monoatomic ideal gas, Cv=32RCp=ΔHΔT∴ΔH=CpΔT mol−1 ( or nCpΔT for n moles )=52×1.987×25=124.2 calWork done, w=−PΔV=−P(V2−V1)=−(PV2−PV1)=−(nRT2−nRT1)=−mR(T2−T1)=−1×1.987(323−298) cal=−49.7 calΔE=q+w=124.2−49.7 cal=74.5 cal.

Calculate $Δ U$ and $Δ H$ in calories if 1 mole of a monoatomic ideal gas is heated at constant pressure of 1 atm from $25^{o} C$ to $50^{o} C$ .