Use the following equations to calculate the heat of the reaction for the synthesis of diborane. 2B(s) + 3/2 O2(g) → B2O3(s)   ∆ Ho = -1273 kJ B2H6(g) + 3 O2(g) → B2O3(s) + 3H2O(g)   ∆ Ho = -2035 kJ H2(g) + 1/2 O2(g) → H2O(l)   ∆ Ho = -286 kJ H2O (l) → H2O (g)   Δ Ho = 44 kJ Calculate ∆Ho for the following reaction: 2B(s) + 3H2(g) → B2H6(g)

The flame in a torch used to cut metal is produced by burning acetylene (C2H2) in pure oxygen. Assuming the combustion of 1 mole of acetylene releases 1251 kJ of heat, what mass of acetylene is needed to cut through a piece of steel if the process requires 90.8  × 104kJ of heat?

Determine the enthalpy of reaction: 2NH3+2CH4+302=2HCN+6H2O

Given that 2.5 x 10^-2 moles of a hydrocarbon experience full combustion, resulting in the release of 104.1 kJ of heat, what is the molar enthalpy of combustion for said hydrocarbon?

What is the enthalpy change for the reaction MgO(s) + 2HCl(g) →MgCl2(s) + H2O(l)? Enthalpies of formation are −601.7 kJ/mole for MgO, −92.3 kJ/mole for HCl, −641.6 kJ/mole for MgCl2, and −285.8 kJ/mole for H2O(l).

Calculate the enthalpy of the following reaction: HCl + NaOH → NaCl + H2O ΔH HCl= -92.3 kJ/mol NaOH= -426.7 kJ/mol NaCl= -411 kJ/mol H2O= -286 kJ/mol Reaction: ΔH=    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.

The enthalpy (or heat) of combustion of acetone, (CH3)2CO, is - 1657.8 kJ. The reaction is (CH3)2CO (1) +4 0₂ (g) →3 CO₂(g) + 3 H₂O (g). Given the values of AH-393.5 kJ/mol for CO₂ (g) and AH-241.8 kJ/mol for H₂O(g), the calculated value of AH; for acetone O equals - 3563.7 kJ/mol O equals - 1022.5 kJ/mol O equals-248.1 kJ/mol O equals 1202.7 kJ/mol

Determine the heat involved in the combustion of liquid hydrazine by using the following reactions. 2NH3(g) + 3N2O(g) → 4N2(g) + 3H2O(ℓ)      ΔH°= –1013 kJ/molN2O(g) + 3H2(g) → N2H4(ℓ) + H2O(ℓ)      ΔH°= –317 kJ/mol2NH3(g) + ½O2(g) → N2H4(ℓ) + H2O(ℓ)      ΔH°= –142.9 kJ/molH2(g) + ½ O2(g) → H2O(ℓ)       ΔH°= –285.8 kJ/mol Then, Launching a small spacecraft to study Jupiter required approximately 28 million kJ. Assume that hydrazine was the only fuel. What mass of hydrazine, in kilograms, was needed for the launch?

With a platinum catalyst, ammonia will burn in oxygen to give nitric oxide, NO. 4NH3 (9) + 502 (g) → 4NO(9) + 6H20(g) AH = -906 kJ What is the enthalpy change for the following reaction? NO(9) + H2O(9) → NH3 (9) + O2(g) Enthalpy change : kJ