Lets number the reaction as 1, 2, 3, 4 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 4 = +1 * (reaction 1) +1 * (reaction 2) -1 * (reaction 3)
So, ΔHo rxn for required reaction will be:
ΔHo rxn = +1 * ΔHo rxn(reaction 1) +1 * ΔHo rxn(reaction 2) -1 * ΔHo rxn(reaction 3)
= +1 * (-571.6) +1 * (-1937.0) -1 * (-2220.0)
= -288.6 KJ
Answer: -288.6 KJ
6. Given that: 2H2(8)Oag)2H200) C3HalE) +40(8)3co2(B)+2H20() AHP-1937 kJ CaHs(8) +502(g) 3CO2lg)+ 4H20U) AHo- -2220 kJ AHo...
1. Balance the following equation in acid: 2. Consider the following reaction; how many Kj are released for 1 mol c2h2 3. Calculate delta H for the reaction 1. Balance the following equation in acid: 2. Consider the following reaction: 2C2H2(g)+502(g)- 4C028)+2H20(g) AH--2511 kJ How many kJ are released for 1 mol C2H2? 3. Given the following data: 3C(gr) + 4H2 (g) C3Hs(g) AH--103.85 kJ C(gr) + O2(g)-Co2(g) AH--393.67 kJ 2H2(g) +02(g)-> 2H20() ΔΗ-,-571.5 kJ Calculate AH for the following...
2. Determine 2. Determine AH for the reaction C3H4(g) + 2H2(g) -> information; (3 Hy+aha a) H2(g) +H202()→ H2O() b) C3H4(e) + 4028) 3C029) + 2H2O c) C3H8(g) + 502(8)> 3CO2(g) + 4H20m) for derestin. Selain has siven the fi C3H8(e) given the following (z Hg AH = -285.8 kJ AH = -1941 kJ AH = -2219.9 kJ
6) Given the following reactions H20 (1) H20 (8) AH = 44.01 kJ AH = -483.64 kJ 2H2 (8) + O2(g) +2H20 (g) the enthalpy for the decomposition of liquid water into gaseous hydrogen and oxygen 2H20 (1) +2H2 (g) + O2(g) _kJ.
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
Given the following equations and AH' values: C(s) + O2(g) + CO2(g) AH = -393.5 kJ H2(g) + 1/2O2(g) - H20 (1) AH = -285.8 kJ 2C2H2 (8) + 5O2(g) + 4CO2(g) + 2H20 (1) AH'= -2598 kJ Determine the heat of reaction (in kJ) at 298 K for the reaction: 2C(s) + H2(8) C2H2 (8) 0-136.8 0-219.8 0-109.9 O-167.1 +226.2
Given the standard enthalpy changes for the following two reactions:(1) \(2 \mathrm{C}(\mathrm{s})+2 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g}) \quad \Delta \mathrm{H}^{\circ}=\mathbf{5 2 . 3} \mathrm{kJ}\)(2) \(2 \mathbf{C}(\mathbf{s})+\mathbf{3 H}_{\mathbf{2}}(\mathbf{g}) \longrightarrow \mathbf{C}_{\mathbf{2}} \mathbf{H}_{\mathbf{6}}(\mathbf{g}) \quad \Delta \mathrm{H}^{\circ}=-\mathbf{8 4 . 7} \mathrm{kJ}\)what is the standard enthalpy change for the reaction:(3) \(\mathbf{C}_{\mathbf{2}} \mathbf{H}_{\mathbf{4}}(\mathbf{g})+\mathbf{H}_{\mathbf{2}}(\mathbf{g}) \longrightarrow \mathbf{C}_{\mathbf{2}} \mathbf{H}_{\mathbf{6}}(\mathbf{g}) \quad \Delta \mathrm{H}^{\circ}=?\)Given the standard enthalpy changes for the following two reactions:(1) \(\mathrm{N}_{2}(\mathrm{~g})+2 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NO}_{2}(\mathrm{~g}) \quad \Delta \mathrm{H}^{\circ}=66.4 \mathrm{~kJ}\)(2) \(2 \mathbf{N}_{2} \mathrm{O}(\mathrm{g}) \longrightarrow \mathbf{2 N}_{2}(\mathbf{g})+\mathbf{O}_{2}(\mathrm{~g}) \quad \Delta \mathrm{H}^{\circ}=-\mathbf{1 6...
10. Given the following table: Compound NO: (g) N:O (g) AHP (J mol) AGP (J mol) 51.84 33.85 9.66 98.29 For the reaction: N:Oa (g) eo 2NO: (g) (a) Use the information in the Table to calculate AG for the reaction (b) Use the information in the Table to calculate AH" for the reaction (c) Calculate K, at 25 C. (d) Calculate K, at 1600 °C. (Assume AH to be temperature independent) (e) Calculate the degree of dissociation, a, of...
7) At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) → 키.4x10-7. Calculate AG)for this reaction at 1500°C A) 105 kJ/mol B)-105 kJmol C)1.07 kJ/molD) CH,011(g) has the value K, D)255 8) Determine the equilibriurn constant K, at 25°C for the reaction Nag) + 3H2(g) → 2NHO 3 kJ/mol A) 1.52 x 106 B) 6.60 x 10 9) Predict the sign of AS for the reaction 02(g) → 20(g). C) 828 x 10D) 2.60 A) Negative B) zero...