Elemental boron can be formed by the reaction of boron trichloride with hydrogen.
2BCl3(g) + 3H2(g) ? 2B(s) + 6HCl(g)
What is ?G°rxn for this reaction? Substance:
BCl3(g) HCl(g) ?G°f (kJ/mol): –388.7 –95.3
A) –293.4 kJ/mol
B) 293.4 kJ/mol
C) –205.6 kJ/mol
D) 205.6 kJ/mol
E) –2141.6 kJ/mol
Elemental boron can be formed by the reaction of boron trichloride with hydrogen. 2BCl3(g) + 3H2(g)...
Elemental boron can be formed by reaction of boron trichloride with hydrogen. BC13(g) + 1.5H2(g) → B(s) + 3HCl(g) Calculate AGº for the reaction at 500K. Substance BC13(g) H2(g) B(s) HCl(g) AH°F (kJ/mol): -403.8 -92.307 AG°f (kJ/mol): -388.7 o 0 -95.299 S°(J/K·mol): 290.1 130.7 5.86 186.9 AG° = -RTINK AG = RTinQ + AG° AG° = AH° - TAS° -78.6 kJ 293.4 kJ 78.6 kJ 86.7 kJ -86.7 kJ
Question 8 Filaments of elemental boron might be made by reducing boron trichloride with molecular hydrogen: 2BC13(g) + 3H2(g) - 2B(s) + 6HCl(g) Is the reaction thermodynamically feasible under standard conditions at 298 K? Yes, it is thermodynamically feasible under these conditions. O No, it is not thermodynamically feasible under these conditions. LINK TO TEXT Is the reaction thermodynamically feasible under standard conditions at 995 K? Yes, it is thermodynamically feasible under these conditions. No, it is not thermodynamically feasible...
Using the following thermochemical data: 2Y(s) + 6HF(g) → 2YF3(s) + 3H2(g) 2Y(s) + 6HCl(g) 2YC13(s) + 3H2(g) calculate AHⓇ for the following reaction: YF3(s) + 3HCl(g) → YC13(s) + 3HF(g) AH° = -1811.0 kJ/mol AH = -1446.2 kJ/mol Select one: O a. 364.8 kJ/mol O b.-3257.2 kJ/mol C. 182.4 kJ/mol O d.-1628.6 kJ/mol O e. 729.6 kJ/mol
2. Hydrogen fluoride can be produced from elemental fluorine and hydrogen according to the reaction H2(g) + F2(g) → 2HF(g). The reaction has an equilibrium constant, Kc, of 7.75 x 102 at a certain temperature. a. Calculate the equilibrium concentration of HF(g) if 5.750 mol of H, and Fz are introduced into a 1.500 L flask. b. Calculate the reaction quotient if 3.25 mol of EACH species is introduced into a 3.000 L flask. What does this value tell us...
solution pls 13. Find the Hºrn for the reaction 2NH3(g) + 3Cl2(g) → N2(g) + 6HCl(g). AH°F (NH3) = -46 kJ/mol, AH°F (HCI) = -92.3 kJ/mol Answer: -461.8 kJ 14. Use the standard enthalpies of formation to calculate AH°rxn: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) AH°F (Fe2O3) = -826 kJ/mol, AH°F (CO) = -110.5 kJ/mol, AH°F (CO2) = -393.5 kJ/mol Answer: -23 kJ 15. Given the following reaction: B2H6(g) + 6H2O(l) → 2H3BO3(g) + 6H2(g) AH°= -493.4 kJ AH°t...
4. Hydrogen reacts with nitrogen to form ammonia (NH3) according to the reaction 3H2(g) + N2(g) + 2NH3(g) The value of AH is -92.38 kJ/mol, and that of AS is -198.2 J/mol · K. Determine AGⓇ at 25°C. Show work
1)Use: 2Al + 6HCl → 3H2 + 2AlCl3 a) If 5.34 g H2 are formed, how many grams of Al reacted? b) If 2.500 kg Al reacts, how many moles of H2 are produced? c) If 6.13 moles of Al react, how many moles of HCl need to react? d) If 125.00 moles HCl reacts, how many mg of AlCl3 are produced? e) If 4.81 x 1024 formula units of AlCl3 are produced, how many moles of HCl reacted?
Metal oxides can be reduced with hydrogen gas to give the metal. H2(g) ZnO(s) H2O(g) +Zn(s) Compound Ha(g) Zno AH(kJ/mol) AG (kJ/mol) S (J/Kemol) 130.7 -348.3 43.6 -318.3 H2O(g) Zn(s) -241.8 188.8 -228.6 41.6 What is the entropy change for the reaction? Errent 13 56.1 J/K 2. -56.1 J/K Cacb180.8)- (u 190.) 3. 404.7 J/K 43.6 J/K 4. Metal oxides can be reduced with hydrogen gas to give the metal. H2O(g) +Zn(s) H2(g)+ZnO(s) AG (kJ/mol) AH (kJ/mol) S(J/Kemol) 130.7 Compound...
The following thermochemical equation is for the reaction of hydrogen chloride(g) with ammonia(g) to form ammonium chloride(s). HCI(g) + NH3(g) NH CH) AH = -176 kJ/mol-rxn How many grams of HCI(g) would have to react to produce 51.9 kJ of energy? grams The following thermochemical equation is for the reaction of hydrogen bromide(r) with chlorine() to form hydrogen chloride) and bromine(g) 2HBr(g) + Cl2(g) +2HCl(g) + Brz(8) AH = -81.1 kJ/mol-rxn When 16.4 grams of hydrogen bromide(g) react with excess...
Part A: Draw the Lewis structures of all the molecules involved in the reaction: N2(g)+3H2(g)→2NH3(g) Part B: If the bond energy for the N≡N bond is 946 kJ/mol, how much energy is needed to break all the bonds in 3.0 mol of nitrogen molecules? Part C: If the bond energy for the H−H bond is 432 kJ/mol, how much energy is needed to break all the bonds in 9 hydrogen gas? Part D: If the bond energy for the N=H...