Calculate E° for the reaction:
3 P + 5 HNO3 + 2 H2O →5 NO + 3 H3PO4
E°H3PO4/P, H3O+ = -0.411, E°NO3-/NO, H3O+ = +0.957
Use standard reduction potentials to calculate ΔG° for the reaction: 3 P + 5 HNO3 + 2 H2O →5 NO + 3 H3PO4 E°H3PO4/P, H3O+ = -0.411, E°NO3-/NO, H3O+ = +0.957. (answer in kj) The number of significant digits is set to 3; the tolerance is +/-1.0%
Use standard reduction potentials to calculate ΔG° for the reaction: 8 NO + 3 H2O →2 NO3- + 3 N2O + 2 H3O+ E°NO3-/NO, H3O+ = +0.957, E°NO/N2O, H3O+ = +1.591
GlauUUUUR URION Downloadable eTextbook signment FULL SCREEN PRI ES Chapter 17, Question 27 Parameterization Calculate Eº for the reaction: 3 P + 5 HNO3 + 2 H20-5 NO + 3 H3PO4 FºH3PO4/P, H30+ = -0.411, E°NO3 /NO, H30+ = +0.957 Round your answer to 3 significant figures. The number of significant digits set to 3; the tolerance is +/-1 in the 3rd significant digit LINK TO TEXT By accessing this Question Assistance, you will learn while you earn points based...
Calculate E° for the reaction: 4 As + 3 O2 + 2 H2O →4 HAsO2 E°O2/H2O, H3O+ = +1.229, E°HAsO2/As, H3O+ = +0.248 Round your answer to 3 significant figures. V The number of significant digits is set to 3; the tolerance is +/-4%
4) Based on the balanced reaction: 2 HNO3 + Ba(OH)2 → Ba(NO3)2 + 2 H2O, how many grams of water could be made by the complete reaction of excess HNO3 and (8.1400x10^2) mL of (6.30x10^ -1) M Ba(OH)2?
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
Consider the following chemical reaction. NH3(g) + 2 O2(g) → HNO3(aq) + H2O(l) Calculate the change in enthalpy (ΔH) for this reaction, using Hess' law and the enthalpy changes for the reactions given below. (1a) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(l); ΔH = −1166.0 kJ/mol (2a) 2 NO(g) + O2(g) → 2 NO2(g); ΔH = −116.2 kJ/mol (3a) 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g); ΔH = −137.3 kJ/mol
What type of reaction is the following? Ca(OH)2(s) + 2 HNO3(aq) + Ca(NO3)2(aq) + 2 H2O(1) O Acid-base neutralization reaction O Hydrogen displacement reaction O Disproportionation reaction O Combustion reaction O Combination reaction Type here to search o E:
15. The pH of a solution of ferric nitrate, Fe(NO3)3, is not 7.00. This fact is best explained by the equation: A) NO3-(aq) + H2O(1) + HNO3(aq) + OH(aq) B) Fe3+(aq) + 6 H2O(1) Fe(OH)3(aq) + 3 H30+(aq) C) [Fe(OH2)6]3+(aq) + H20(1) 3 H3O+(aq) + [Fe(OH2)5(OH)]2+(aq) D) H3O+(aq) + OH-(aq) + 2 H2O(1) E) HNO3(aq) + H2O() H30+(aq) + NO3-(aq)
Given the following reaction: 4 Zn + 10 HNO3 ? 4 Zn(NO3)2 + NH4NO3 + 3 H2O If we start with 3.32 g of Zn and excess of HNO3, how many g of each product will be formed?