Consider the reaction of nitrogen monoxide and chlorine to form nitrosyl chlorid

Question

Consider the reaction of nitrogen monoxide and chlorine to form nitrosyl chloride: 2 NO(g) + Cl_2(g) rightarrow 2 NOCl(g) Calculate DeltaG when pNO = 0.30 atm, pCl_2 = 0.10 atm, and pNOCl = 0.45 atm. The DeltaGdegree_f of NO(g), Cl_2(g) and NOCl (g) are 86.6, 0 and 66.2 kj/mol, respectively. A) -40.8 kJ B) -33 kJ C) -7.8 kJ D) 23 kJ E) 40.8 kJ 10) Calculate the entropy change when a He atom in the gas phase expands from V_1 to 2V_1 at constant temperature. A) 5.8 kJ/K B) 9.6 times 10^-24 kJ/K C) -5.8 kJ/K D) 0 kJ/K E) not enough information

Explanation / Answer

since enthalpy change= sum of enthalpy of products- sum of enthalpy of reactants

= 2*66.2- (1*0+2*86.6)

where 2, 1 and 2 are coefficients of NOCl, Cl2 and No

=-40.8 Kj

delG= delGf+ RT lnQ= -40.8 *1000 +8.314*298.15 ln(0.45*0.45/0.1*0.3*0.3)=-33100 Kj= -33.1 Kj

b) entropy change= -R ln (P/P0)

P= final pressure and P0 = initial pressure

at constant temperature

PV= P0VO

P/Po= Vo/V= 1/2

entropy change= -8.314*ln(1/2)=5.76J/K ( no correct answer)

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