Hydrogen gas will react with either acetylene, C2H2, or ethylene, C2H4, gas. The thermochemical equations for these reactions are provided below. Calculate the ΔH° of the conversion of acetylene into ethylene by hydrogen gas.   C2H2(g) + 2H2(g) → C2H6 ΔH° = –311 kJ   C2H6 → C2H4(g) + H2(g) ΔH° = 136 kJ

Using standard heats of formation (∆Hfo), calculate ∆H for the following reactions:  7O2(g) + 4NH3(g) → 4NO2(g) + 6H2O(l) CaCO3(s) → CaO(s) + CO2(g)

Given the standard enthalpy changes for the following two reactions: (1) 2C(s) + 2H2(g) C2H4(g) AH° = 52.3 kJ (2) 2C(s) + 3H2(g) C2H6(g) AH° = -84.7 kJ what is the standard enthalpy change for the reaction: (3) C2H4(g) + H2(g) C2H6(g) AH° = ? kJ

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

Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)   3 C(s) + 4 H2(g) → C3H8(g)           ΔH = – 118.2 kJ C(s) + O2(g) → CO2(g)                   ΔH = – 62.4 kJ H2(g) + 1/2 O2(g) →  H2O(g)          ΔH = – 182.5 kJ

The enthalpy change for the following reaction is given below. Pb (s) + CO2 (g) → PbO (s) + CO (g) ΔH° = +131.4 kJ Using the standard enthalpies of formation (∆Hf°) of CO2(g) = −393.5 kJ/mol, and CO(g) = −110.5 kJ/mol, determine the standard enthalpy of formation of PbO(s) A. −151.6 kJ ∕ mol B. −283.0 kJ ∕ mol C. +283.0 kJ ∕ mol D. −372.6 kJ ∕ mol E. +252.1 kJ ∕ mol

The balanced thermochemical equation for the combustion of exactly one mole of propane is: C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O(l) ΔH = -2220 kJ/mol What is the enthalpy change for the reaction: 1.5 CO2 (g) + 2 H2O(l)  → 0.5 C3H8 (g) + 2.5 O2 (g) ΔH = ?

Consider the following information: A + B → C + D AH° = -15 kJ mol-1 C + D → E AH° = +5 kJ mol-1 Calculate the enthalpy for the following reaction: 2A+2B → 2E

Given the following combustion reaction and its molar enthalpy of reaction: 2NO(g) + O2(g) 2NO2(g) AH° = -112 kJ What is the heat (q) associated with the combustion of 2.00 mole of NO(g)? O -112 kJ O -224 kJ +56.0 kJ -56.0 kJ O +112 kJ