Given:
Gof(NO2(g)) = 51.8 KJ/mol
Gof(H2O(l)) = -237.2 KJ/mol
Gof(HNO3(l)) = -79.9 KJ/mol
Gof(NO(g)) = 86.7 KJ/mol
Balanced chemical equation is:
3 NO2(g) + H2O(l) ---> 2 HNO3(l) + NO(g)
ΔGo rxn = 2*Gof(HNO3(l)) + 1*Gof(NO(g)) - 3*Gof( NO2(g)) -
1*Gof(H2O(l))
ΔGo rxn = 2*(-79.9) + 1*(86.7) - 3*(51.8) - 1*(-237.2)
ΔGo rxn = 8.7 KJ
Answer: 8.7 KJ
Calculate AG°(1V K3/uok) for the reaction NO2(g) + H20(1) -> HNO3(1) + NO(g). (unbalanced) Substance AGfº(kJ/mol)...
Calculate ΔG°(in kJ/mol) for the reaction NO2(g) +
H2O(l) --> HNO3(l) + NO(g).
(unbalanced)
Question 7 Calculate AG°(in kJ/mol) for the reaction NO2(g) + H2O(0) --> HNO3(1) + NO(g). (unbalanced) Substance AGF(kj/mol) NO2(g) 51.8 NO(g) 86.7 HNO3(0) -79.9 H2O(l) -237.2 Write answer to two significant figures and correct sign.
Calculate ΔG°(in kJ/mol) for the reaction NO2(g) + H2O(l) --> HNO3(l) + NO(g). ( unbalanced) Substance ΔGfo(kJ/mol) NO2(g) 51.8 NO(g) 86.7 HNO3(l) -79.9 H2O(l) -237.2 Write answer to two significant figures and correct sign.
Given the values of AGfº given below in kJ/mol, calculate the value of AG in kJ for the reaction at 298 K.: 3 NO2(g) + H20(1) > 2 HNO3(0) + NO(g) AGº (NO2) = 49. AG (H2000) = -237. AGRO (HNO3) --77. AGP (NO) = 85.
Substance AGP (kJ/mol) AS (J/mol K) NO (g) 86.7 211 NO2 (g) 51.8 240 NOCI (g) 66.3 264 N20 (g) 103.6 220 What is the value of AH° (in kJ) at 25.0 °C for the reaction: N20 (g) + NO2 (g) → 3 NO (g) 5.5 kJ 53.2 kJ 109 kJ 156.2 kJ
QUESTION 19 Calculate AG, in kJ, for the following reaction: 2 HNO, (lia) + NO (g) - 3 NO, (g) + H2O (lia) Substance AG (kJ) HNO3 () - 79.71 NO (9) 86.57 51.30 NO2 (9) H20 (0) -237.18 QUESTION 20 Calculate the equilibrium constant for the reaction from the previous question at O "C. ENTER A NUMBER WITH FOUR SIG FIGS. K=e-4CRT R = 8.314 J/K mol
You are studying the combustion of ethane by the following unbalanced chemical reaction: a C2H6(g) + b O2(g) --> C CO2(g) + d H2O(g) How many kilojoules of Gibb's Free Energy are liberated by burning 19.419g of ethane in excess oxygen? Substance AG°f(kJ/mol C2H6(g) -32.04 O2(g) 0 CO2(g) -394.36 H2O(g) -228.59
Calculate ΔG°, in kJ, for the following reaction: 2 HNO3 (liq) + NO (g) → 3 NO2 (g) + H2O (liq) Substance ΔGf° (kJ) HNO3 (ℓ) −79.71 NO (g) 86.57 NO2 (g) 51.30 H2O (ℓ) −237.18
Nitrogen Ahºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 191.6 N2(9) 0 0 N(g) 472.7 455.6 153.3 NH3(g) -46.1 -16.5 192.5 NH3(aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 90.3 86.6 210.8 NO(9) NOCI(g) 51.7 66.1 261.8 NO2(g) 33.2 51.3 240.1 N20(9) 82.1 104.2 219.9 N204(9) 9.2 97.9 304.3 N204(0) -20.0 97.0 209.0 N205(s) -42.0 134.0 178.0 N2H4(0) 50.6 149.3 121.2 N2H3CH3 () 54.0 180.0 166.0 HNO3(aq) -207.4 -111.3 146.4 HNO3(1) -174.1 -80.7 155.6 HNO3(9) -135.1 -74.7 266.4 NH4ClO4(s) -295.0...
1. Calculate ΔHnn for the following reaction. 3NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) Given. AHof (NO2(g)) = +33.2 klymol AHof (H20(1)) =-187.8 ki/mol AHof (HNO3(aq)) =-207.0 kJ/mol AHof (NO(g)) = +91.3 kJ/mol
Using the equation and thermodynamic data: CO(g) + O2(g) --> CO2(g) (unbalanced) AH(rxn) = -566.0 kJ ( for the balanced equation) Substance sºu/mol*K) O2(g) 205.0 CO(g) 197.7 CO2(g) 213.8 NOTE: Write all answers to four significant figures. a. What is the Assys(J/mol*K) = b. What is the Assurr(J/mol*K) = c. What is the Asuniv( J/mol*K) = d. At what temperature(°C) will the reaction go from spontaneous to non-spontaneous?