A scientist measures the standard enthalpy change for the following reaction to be -1051.8 kJ 2H2S(g)+3 O2(g)- 2H2O(g) +2 SO2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(g) is kJ/mol Submit Answer Retry Entire Group 9 more group attempts remaining

A scientist measures the standard enthalpy change for this reaction to be 296.0 kJ/mol: H₂S(g) + 2 H₂O(l) 3H₂(g) + SO₂(g) Based on this value and the standard formation enthalpies for the other substances, the standard formation enthalpy of H₂S(g) is kJ/mol. Submit Answer Retry Entire Group 1 more group attempt remaining

A scientist measures the standard enthalpy change for the following reaction to be 184.8 kJ:Fe3O4(s) + 4 H2(g) 3Fe(s) + 4 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of Fe3O4(s) is kJ/mol.

a) Using standard enthalpies of formation (in Appendix G in your text), calculate the standard enthalpy change (AH°) for the following reaction shown below. (Show all work.) b) Based on your calculation, is the reaction exothermic or endothermic? 2 H2S(g) + SO2(g) --> 3/8 S8(s) + 2 H20(g)

Use the References to access important values if needed for this question. A scientist measures the standard enthalpy change for the following reaction to be -103.2 kJ: 4HCl(g) + O2(g) → 2H₂O(g) + 2Cl₂ (g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of HCl(g) is I kJ/mol red Species AH (kJ/mol) H₂O(g) -241.8 Cl₂(g) 0.0 0₂ (9) 0.0

Consider the balanced reaction 4 A + 9 B → 8 C + 8 D and the enthalpies of formation provided in the table below. AH Compound (kJ/mol) A 170.8 231.1 D -98.4 Suppose that the AH of the overall reaction is -2,029.3 kJ/molxn. Calculate the value of the AHf of C in kJ/mol. Report your answer to three decimal places (ignore significant figures).

How much did our sodium-in-water demonstration raise the temperature of water in the dessicator jar?  The reaction we performed was:                   Na(s) + H2O(l)    NaOH(aq) + 1/2H2(g)                               qreaction = rHo = -184 kJ/mol-rxn Assuming the dessicator jar is well insulated (like our coffee-cup calorimeter), the energy balance is:                  0 = qsystem = qreaction + qwater    qreaction = -qwater                  qreaction = -mwater*Cwater*Twater The data from the demonstration was:  (a) 1.0 kg water, (b) 22.0oC, (d) Cwater = 4.18 J/g-K, (e) mNa = 0.21 g How many moles of sodium were added to the water (in moles)?

The standard enthalpy change for the following reaction is 84.7 kJ at 298 K. C2H6(g) 2 C(s.graphite) + 3 H2(g) AH° = 84.7 kJ What is the standard enthalpy change for this reaction at 298 K? 2 C(s.graphite) + 3 H2(g) - CH6(g) kJ Submit Answer Retry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical S