Lets number the reaction as 0, 1, 2 from top to bottom
required reaction should be written in terms of other reaction
This is Hess Law
required reaction can be written as:
reaction 0 = -0.5 * (reaction 1) +1 * (reaction 2)
So, ΔHo rxn for required reaction will be:
ΔHo rxn = -0.5 * ΔHo rxn(reaction 1) +1 * ΔHo rxn(reaction 2)
= -0.5 * (-202.4) +1 * (-318.7)
= -217.5 KJ
Answer: -217.5 KJ
For the reaction C2H4(8) + Cl2(g) — C2H4C12(1), determine A,Hº, given that 4 HCl(g) + O2(g)...
For the reaction C2H4(g) + Cl2(g) C2H4C12(1), determine AH°, given that 2 Cl2(g)2 H2O(I) 4 HCl(g)O2(g) -202.4 kJ mol1 1 2 HCI(g) + C2H4(g) +O28) 1 -318.7 kJ mol C2H4C12(1) H2O(1) AH°
71. For the reaction C2H4(g) +C2(g) determine ApH°, given that C2H&C2(1), 2 Cl2(g) + 2H20(1) A,H° =-202.4 kJ mol 1 4 HCl(g) + O2(g) 2 HCl(g) +C2H4(g) +02(8) 2 C2H4CI2(1) + H2O(1) A,H =-318.7 kJ mol-1
Use Hess's law to determine A.Hº for the reaction C3H4(g) + 2 H2(g) -> C3H8(8), given that Hy(8) + O2(8) — H2O(1) A Hº = -285.8 kJ mol-1 C3H4(8) + 402(g) — 3 CO2(g) + 2 H2O(1) A Hº = -1937 kJ mol-1 C3H2(g) + 5O2(g) — 3CO2(g) + 4H2O(1) A Hº = -2219.1 kJ mol-1
The reaction: 2 Cl2(g) + 2 H2O(g) ➝ O2(g) + 4 HCl(g) has ΔG° = +11.2 kJ/mol and ΔH° = +114.4 kJ/mol at 800 K. a) What is the numerical value of the equilibrium constant for this reaction at 800 K? b) What is the numerical value of ΔG for the reaction in a vessel containing 3.6 bar Cl2, 1.4 bar H2O, 0.20 bar O2, and 0.50 bar HCl at 800 K?
Practice with Hess's Law and Standard Heats of Formation 1. (Example) The reaction C2H4 (g) + 6 F2 (g) → 2 CF4(g) + 4 HF (g) can be written as the sum of: C2H4 (9) ► 2 C(s) + 2 H2 (g) AH = -52.3 kJ/mol 2 C(s) + 4 F2 (9) ► 2 CF4(9) AH = -1360 kJ/mol 2 H2(g) + 2 F2 (g) → 4 HF (a) AH = -1074 kJ/mol C2H4(g) + 6 F2(g) → 2 CF4(g)...
Fill in the Blanks Given this balanced chemical reaction, 4 HCl(g) + O2(g) +2H20(0) + 2 C12(e) AH reaction=-202.4 kJ (give answer in decimal notation, i.e. 234,000) a. How many J (joules) of heat are released when 2.50 moles of HCl react with excess oxygen gas? b. How many moles of HCl are there in 89.3 g of HCl? c. How many kJ of heat are released when 89.3 g of HC react with excess O2? (Enter your answers as...
- degreasing agent, Tetrachloroethylene, is produced in the reaction C2H4(g) + 4 HCl(g) + 2 O (8) ► C lic AH (kJ/moly 52 26 - 92.31 a) determine AH°for CC1(1) FC (9) +2 O2(g) → CCI.(l) + 4H2O(1) -285.8 AH x = -878.5 kJ a) AHⓇ for CC (I) = -52.28 kJ b) How much heat (kJ) would be evol amounts of HCl and O:)? uch heat (kJ) would be evolved when 7.5 kg of C2H4(g) reacts completely (with stoichiometric...
Using the reactions below, determine the ∆Hº for 2 N2(g) + 5 O2(g) --> 2 N2O5(g) N2(g) + 3 O2(g) + H2(g) --> 2 HNO3(aq) ∆Hº = -415 kJ/mol N2O5(g) + H2O(l) --> 2 HNO3(aq) ∆Hº = -140 kJ/mol 2 H2(g) + O2(g) --> 2 H2O(l) ∆Hº = -572 kJ/mol
Use Hess's law to determine Ofor the reaction → CO2(g),given that C(graphite) +202(8) — CO(8) A Hº = -110.54 kJ mol C(graphite) + O2(8) —CO2(g) A Hº = -393.51 kJ mol
Enthalpy changes for the following reactions can be determined experimentally: C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(l) C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) ΔHorxn = -1411.1 kJ/mol-rxn ΔHorxn = -1367.5 kJ/mol-rxn Use the given values to determine the enthalpy change for the reaction: C2H4(g) + H2O(l) → C2H5OH(l) ΔHorxn (answer) = kJ/mol-rxn