Use the following reaction with their enthalpy values: C + O2 -> CO2    H = -231 kJ 2H2 + O2 -> 2H2O  H = -148 kJ C4H9OH + 6O2 -> 4CO2 + 5H2O  H = -358 kJ To get the enthalpy for the following reaction: 8C + 10H2 + O2 -> 2C4H9OH  H = ?

Calculate the enthalpy change for the following reaction, _C₂H4 (9) + using the following standard heats of formation: AH(C₂H4) = +52.5 kJ/mol; AH(CF4) =-933.0 kJ/mol; AH (HF) =-271.6 kJ/mol _F₂(g) → _CF4(g) + _HF(g)

For the reaction below (which will be labeled reaction A), the reaction enthalpy is unknown:                                                   2 B    + 3 H2    B2H6    HA  = ? Use the following thermochemical data to calculate the reaction enthalpy ΔHA: Reaction 1:       4 B + 3 O2 → 2 B2O3                               ΔH1 = –2509 kJ Reaction 2:       2 H2 + O2 → 2 H2O                          ΔH2 = –572 kJ Reaction 3:       B2H6 + 3 O2 → B2O3 + 3 H2O   ΔH3 = –2,159 kJ Calculate the enthalpy of reaction A (in kJ) and enter the numerical value in the answer box. Do not write units in the answer box. Clearly show on a paper how each reaction can be combined to equal reaction A  (multiply or reverse  each of the above reactions).complete work must be uploaded

Use Hess’s law to calculate the enthalpy change for the reaction WO3(s) + 3H2(g) —> W(s) +3H2O(g) from the following data: 2W(s) + 3O2(g) —> 2 WO3(s) H=-1685.4 2H2(g) + O2(g) —> 2H2O(g) H=-477.84

Given the following reactions: N2 (g) + O2 (g) → 2NO (g) AH = +180.7 kJ 2N20 (g) → O2 (g) + 2N2 (g) AH = -163.2 kJ the enthalpy of reaction for 2N20 (g) → 2NOo (g) + N2 (g) is kJ. -343.9 343.9 -145.7 145.7 O 17.5

In the laboratory, a student dilutes 17.8 mL of a 9.80 M hydrobromic acid solution to a total volume of 125.0 mL. What is the concentration of the diluted solution? Concentration = 0.78 M

Use Hess’s law to obtain the enthalpy change for this reaction: H2(g)  + 1/8 S8(rhombic) -> H2S(g) from the following enthalpies:H2S(g) + 3/2 O2(g) à H2O(g)  +  SO2(g)      ΔH = -518 KJH2(g)  + ½ O2(g)  à  H2O(g)                       ΔH = -242 KJ1/8 S8(rhombic)  + O2(g)  à SO2(g)              ΔH = -297 KJ

Using standard heats of formation, calculate the standard enthalpy change for the following reaction.H2S(g) + 2H2O(l)3H2(g) + SO2(g)

Calculate the enthalpy of formation of 1 mole SO₂(g) from the standard enthalpy changes of the following reactions: 2SO3(g)2SO₂(g) + O₂(g) 2S (s) +30₂(g) → 2SO3(g) →→ SO₂(g) S(s) + O₂(g) kJ ΔΗ AH rxn 1=+196 kJ rxn 2 = -790 kJ AHO rxn 3 = ? k

Using standard heats of formation, calculate the standard enthalpy change for the following reaction.H2S(g) + 2H2O(l)3H2(g) + SO2(g)