Determine the enthalpy of reaction for 2CH2(g) → C₂H4(g) + 2H₂(g) using the equations: 2C₂H6(g) + 70₂(g) → 4CO₂(g) + 6H₂O(l) AH° = -3120.8 kJ/mol CH₂(g) + 20₂(g) → CO₂(g) + 2H₂O(1) AH° = -890.3 kJ/mol C₂H4(g) + H₂(g) → C₂H6(g) AH° = -136.3 kJ/mol H₂ + 1/2O2(g) → H₂O(1) AH° = −285.8 kJ/ mol

Use the indicated average bond enthalpies to estimate the change in enthalpy, ΔHo, for the reaction between methane and iodine to produce iodomethane and hydrogen iodide: CH4(g)  +  I2(g)  →  CH3I(g)  +  HI(g)       ΔHo = ? It may be helpful to draw the Lewis electron dot structure for each reactant and product; all reactants and products have single bonds. average bond enthalpies (kJ) C - H  413   ,   C - I  240   ,   H - I  299   ,   I - I  151 Express your answer in units of kilojoules, but do not include the units on your submitted answer.

Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H₂(g) →C₂H₂(g) AH = -125.6 kJ (2) C₂H₂(g)2C(s) + H₂(g) AH = -226.7 kJ what is the standard enthalpy change for the reaction: (3) 2C₂H₂(g) + 3H₂(g)-CH₁0(g) AH° = ?

What is the enthalpy change when  2.00 mol of oxygen (O2) react? C12H22O11(s)   + 12 O2(g) →    12 CO2(g)  +    11 H2O(l)        ΔH = -5644 kJ