the reaction below is used to produce methanol:
CO(g) + 2H2(g) --> CH3OH(l)

H(rxn)= -128 kJ

(a) calculate the C-H bond energy given the following data

C(triple bonded)O: D=1072 kj/mol

H-H: D= 436 kj/mol

C-O: D=358 kj/mol

O-H: 463 kj/mol

(b) the tabulated value of the C-H bond energy is 413 kj/mol.explain why there is a difference between the number you havecalculated in (a) and the tabulated value.

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Nestor RutherfordLv2

31 Jul 2019

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Using Bond Energy data, What is deltaH for the followingreaction?

CH3OH(g) + H2S(g) ---> CH3SH(g) + H2O(g)

Bond	Bond Energy (kJ/mol)
C-H	413
C-O	358
O-H	463
C-S	259
S-H	339

A detailed explanation would be so very appreciated, I am havingso much trouble with this!

The reaction of coal with water at high temperatures produces synthesis gas, which is a mixture of carbon monoxide and hydrogen. Use the bond energies in the table below to estimate the enthalpy of the reaction C(g) + H2O(g) ? CO(g) + H2(g) Energy(kj/mol) c-o = 358 c=o = 770 c-triple bond-o = 1070 o-h = 465 h-h = 435

1.A system releases 691 kJ of heat and does 100 kJ of work on the surroundings.

What is the change in internal energy of the system? Express your answer to 2 sig figs.

2.If 1.7 g of matter were converted to energy, how much energy would be formed?

Express your answer using two significant figures.

3.Hydrogen gas reacts with oxygen to form water.

2H2(g)+O2(g)â2H2O(g)ÎH=â483.5kJ

Determine the minimum mass of hydrogen gas required to produce 524 kJ of heat.

Express your answer to three significant figures and include the appropriate units.

4. Calculate ÎHrxn for the following reaction:
5C(s)+6H2(g)âC5H12(l)
Use the following reactions and given ÎHâ²s.
C5H12(l)+8O2(g)â5CO2(g)+6H2O(g), ÎH= -3244.8 kJ
C(s)+O2(g)âCO2(g), ÎH= -393.5 kJ
2H2(g)+O2(g)â2H2O(g), ÎH= -483.5 kJ