13)
Given:
Hof(NH3(g)) = -46.0 KJ/mol
Hof(Cl2(g)) = 0.0 KJ/mol
Hof(N2(g)) = 0.0 KJ/mol
Hof(HCl(g)) = -92.3 KJ/mol
Balanced chemical equation is:
2 NH3(g) + 3 Cl2(g) ---> N2(g) + 6 HCl(g)
ΔHo rxn = 1*Hof(N2(g)) + 6*Hof(HCl(g)) - 2*Hof( NH3(g)) - 3*Hof(Cl2(g))
ΔHo rxn = 1*(0.0) + 6*(-92.3) - 2*(-46.0) - 3*(0.0)
ΔHo rxn = -461.8 KJ
Answer: -461.8 KJ
Only 1 question at a time please
solution pls 13. Find the Hºrn for the reaction 2NH3(g) + 3Cl2(g) → N2(g) + 6HCl(g)....
15. Given the following reaction: BzH6(g) + 6H2O(l) → 2H3BO3(g) + 6H2(g) AH°= -493.4 kJ AH°F (H3BO3) = -1088.7 kJ/mol AH°4 (H2O) = -285.5 kJ/mol Answer: 30.8 kJ
2.Calculate the enthalpy of reaction for the following reaction: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ΔHfo(Fe2O3(s)) = -824.2 kJ/mol ΔHfo(CO(g)) = -110.5 ΔHfo(Fe(s)) = ? ΔHfo(CO2(g)) = -393.5 kJ/mol
which of the following statements is/are true concerning a state function Using the standard enthalpies of formation listed below, determine the standard enthalpy change for the following reaction: Fe2O3(s) + 3CO(g) ---> 2Fe(s) + 3C02() AH°-m AH" for Fe2O3(s) --824.2 kJ/mol AH® for CO(g) = -110.5 kJ/mol AH", for CO2(g) - -393.5 kJ/mol
Calculate the enthalpy of reaction for the following reaction: Question 19 Not yet answered Marked out of 1.00 Fe2O3(s) + 3CO(g) – 2Fe(s) + 3C02(9) P Flag question AH °(Fe2O3(s)) = -824.2 kJ/mol AH°(CO(g)) = -110.5 AH°(Fe(s)) = ? AH°(CO2(g)) = -393.5 kJ/mol Answer:
I need someone to show me how to solve thus problem, I think I have the right idea, but I may be plugging in something wrong. What is ΔS° at 298 K for the following reaction? Fe2O3(s)+ 3CO(g)→ 3CO2(g) + 2Fe(s) Substance ΔG°f(kJ/mol) ΔH°f(kJ/mol) Fe2O3(s). -741.0 -822.2 CO(g) -137.2 -110.5 CO2(g) -394.4 -393.5 Thanks
Using the following equation: 2NH3 + 3Cl2 --> N2 + 6HCl if you had 5.64 g of Cl2 gas, how many moles of hydrochloric acid would be produced? if you had 0.653 mol of HCl gas produced, how many g of ammonia gas was used?
1).From the standard enthalpies of formation, calculate ΔH°rxn for the reaction C6H12(l) + 9O2(g) → 6CO2(g) + 6H2O(l) For C6H12(l), ΔH°f = –151.9 kJ/mol (5 points) Substance ∆H°f , kJ/mol C6H12(l) –151.9 O2(g) 0 H2O(l) –285.8 CO2(g) –393.5 2).Determine the amount of heat (in kJ) given off when 1.26 × 104 g of ammonia are produced according to the equation N2(g) + 3H2(g) → 2NH3(g) ΔH°= –92.6 kJ/mol Assume that the reaction takes place under standard conditions at 25oC.
help with these please N2(g) + O2(g) 2NO(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: CH (9) +202(g) →CO2(g) + 2H2O(g) de manera en cas de este mai mare de mise en contact tenda Using standard thermodynamic data at 298K, calculate the free energy change when 1.62 moles of CH4(g) react at standard conditions. AGºrx Nz9) +202(g) +2NO2(g) Using standard thermodynamic data at 298K, calculate the free...
I hope the answer is clear and correct thanks Question 1 (1 point) What is the change in enthalpy (in kJ mol'?) for the following reaction F2(g) + Cabr,(s) CaF() + Brz(1) O 1) -112 kJmo12 O2) 504 kJmo11 03) -504 kJmol 1 04) 537 kJmo11 O 5) -537 kJmol'i Question 2 (1 point) What is true about the following reaction at 25°C? F,(g) + 2HCl(g) 2 2017(g) + H (9) Ahrº=76 kJ mol'i Asr°=-10.13 J mol'i Ki Agrº=79 kJ...
4. Only ideal processes can be thermodynamically "reversible." Why can rear proce y can real processes not be? 5. Consider the following reactions. (Note: if this were an exam we would give you an excerpt on tabular data from Appendix 4 (Table A4.3). 2Fe(s) + 3Cla(s) 2FeCl(s) N2H4(8) + H2(g) + 2NH3(g) (a) Would you expect the entropy change for the above reaction to be >0, <0, or no (small)? Justify your answer. (d) Would you expect the entropy change...