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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Calculate ΔH for the following reaction:
2 H2S + 3 O2 → 2 SO2 + 2 H2O ΔH = ??
Given the following:
H2 + 1/2 O2 → H2O ΔH = -241 kJ
SO2 + 3 H2 → H2S + 2 H2O ΔH = 35 kJ
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- Consider the following thermochemical equations (Note: HA is a weak acid)H+(aq) + OH-(aq) → H2O(l) ΔH1HA(aq) → H+(aq) + A-(aq) ΔH2HA(aq) + OH-(aq) → A-(aq) + H2O(l) ΔH3Choose the equation that shows the correct relationship between their enthalpy changes. A.) ΔH1 = ΔH3 - ΔH2 B.) ΔH2 = ΔH1 + ΔH3arrow_forward1. What is 4-H for this reaction: 3C(s) + 4H2(g) → C3H8(g) given the following reactions: C3H8(g) +502(g) → 3CO2(g) + 4H2O(g) C(s) + O2(g) → CO2(g) 4-H = -2043 kJ/mol AH = -393.5 kJ/mol 4,H= -483.6 kJ/mol 2H₂(g) + O2(g) → 2H₂O(g) (a) -4191 kJ/mol (b) 1166 kJ/mol (c) 378 kJ/mol (d) -105 kJ/molarrow_forwardFind the ΔH (kJ) for the reaction below, given the following reactions and subsequent ΔH values: N2(g) + 2O2(g) → 2NO 2(g) N2(g) + 3H2(g) → 2NH3(g) ΔH = -115 kJ 2NH3(g) + 4H2O(l) → 2NO2(g) + 7H2(g) ΔH = -142.5 kJ H2O(l) → H2(g) + 1/2O 2(g) ΔH = -43.7 kJ (Supply answer up to the 1st decimal point)arrow_forward
- Consider the following thermochemical equations (Note: HA is a weak acid)H+(aq) + OH-(aq) → H2O(l) ΔH1HA(aq) → H+(aq) + A-(aq) ΔH2HA(aq) + OH-(aq) → A-(aq) + H2O(l) ΔH3Choose the equation that shows the correct relationship between their enthalpy changes.arrow_forwardUse the standard reaction enthalpies given below to determine Hᵒrn for the following reaction: Given: 2 NO(g) + O2(g) → 2 NO2(g) N2(g) + O2(g) → 2NO(g) 1/2N2(g) + O2(g) → NO2(g) -150. kJ -117 kJ -333 kJ +115 kJ +238 kJ AH° rxn = ? AHᵒrxn = +183 kJ AH°rxn = +33 kJarrow_forwardCalculate the ΔH°rxn for the following reaction SO2Cl2 + 2H2O → 2HCl + H2SO4 using the enthalpy of formations ΔH°f Given: SO2Cl2 = -364 kJ/mol H2O = -286 kJ/mol HCl = -92 kJ/mol H2SO4 = -814 kJ/molarrow_forward
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