Lets number the reaction as 0, 1, 2, 3 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 = +1 * (reaction 1) +2 * (reaction 2) +1 * (reaction 3)
So, ΔHo rxn for required reaction will be:
ΔHo rxn = +1 * ΔHo rxn(reaction 1) +2 * ΔHo rxn(reaction 2) +1 * ΔHo rxn(reaction 3)
= +1 * (379.1) +2 * (-110.0) +1 * (-285.9)
= -126.8 KJ
Answer: -126.8 KJ
12) Given the reactions below calculate the AHⓇrxn for the following reaction: 2LiH(s) + O2(g) Li2O(s)...
Part A Calculate Δ Han for the following reaction: C(s) +H2O(g)CO(g)+H2() Use the following reactions and given ΔΗ values: C(s) + O2 (g)- CO2 (g), ΔΗ-393.5 kJ 2CO (g) + O2 (g)--2CO2 (g), ΔΗ-566.0 kJ 2H2 (g) +02 (g)-2H3O(g). Ан :-483.6 kJ Express your answer using four significant figures. kJ Submit Request Answer
ΔS is negative for the reaction ________. 2H2O (g) → 2H2 (g) + O2 (g) LiOH (aq) → Li+ (aq) + OH– (aq) CH3OH (l) → CH3OH (g) Sr(NO3)2 (aq) + 2LiOH (aq) → Sr(OH)2 (s) + 2LiNO3 (aq) C6H12O6 (s) → 6C (s) + 6H2 (g) + 3O2 (g)
Find the change in enthalpy for the reaction below, given the following reactions and change in enthalpy values: C2H2(g)+ 5/202(g)-2CO2(g) + H2O(g) ΔΗ ? Use: C2H6(g) → C2H2(g) + 2H2(g) ΔΗ : 283.5 kJ H29) 1/2029) H20(g) AH--213.7 kJ 2CO2(g) + 3H2O(g)-C2H6(g) + 7/2O2(g) ΔΗ = 849 kJ
7. Calculate the AHReaction for the reaction 2H2(g) + CO(g) → CH3OH() Using the following equations: CH3OH(1) + O2(g) → C(s) + 2H2O(1) C(s) + O2 (g) — CO(g) H2(g) + O2(g) → H2O(1) AH = -333.00 kJ AH =-111.52 kJ AH = -285.83 kJ
Part C Given the following reactions 2H2 (9) + O2(g) → 2H20 (9) AH = - 483.64 kJ 2H20 (1) ► 2H2(g) + O2 (9) AH = 571.66 kJ Calculate the enthalpy for the condensation of water vapor to liquid, given by this reaction: H2O(g) + H20 (1) +44.01 kJ +88.02 kJ 0 -44.01 kJ -88.02 kJ Submit Request Answer
C(s) + O2(g) + CO2(g) AH° = -393.5 kJ (5 pts) Given the following enthalpy values for reactions at 25°C, what is AH at 25°C for the following reaction: C3H3(g) + 502(g) + 4H2O(g) + 3CO2(g) AH = -2043 kJ 3C(s) + 4 H2(g) → C3H8 (g) 2H2(g) + O2(g) + 2H2O(g) AH° = -483.6 kJ
Calculate ΔHrn for the following reaction 50(s) + 6H2(g) → C5H12(1) Use the following reactions and given AH's. C5H12(1) + 802 (g) → 5CO2(g) + 6H20(g), ΔH=-3244.8 kJ C(s) + O2(g) → CO2 (g), ΔH=-393.5 kJ 2H2 (g) + O2 (g) → 2H2O(g), ΔH=-483.5 kJ Express your answer to for significant figures kJ
Calculate ΔHrxn for the following reaction: 5C(s)+6H2(g)→C5H12(l) Use the following reactions and given ΔH′s. C5H12(l)+8O2(g)→5CO2(g)+6H2O(g), ΔH= -3244.8 kJ C(s)+O2(g)→CO2(g), ΔH= -393.5 kJ 2H2(g)+O2(g)→2H2O(g), ΔH= -483.5 kJ Express your answer to for significant figures.
Calculate ΔHrxn for the following reaction: 5C(s)+6H2(g)→C5H12(l) Use the following reactions and given ΔH values: C5H12(l)+8O2(g)→5CO2(g)+6H2O(g), ΔH= -3244.8 kJ C(s)+O2(g)→CO2(g), ΔH= -393.5 kJ 2H2(g)+O2(g)→2H2O(g), ΔH= -483.5 kJ
Given the equilibrium constants for the following reactions: 2H2(g) + O2(g) → 2H2O(g) K1 = 3.74 x 1026 H2(g) + Cl2(g) → 2HCl(g) K2 = 9.73 x 1012 calculate the equilibrium constant for the reaction below. 4HCl(g) + O2(g) → 2Cl2(g) + 2H2O(g)