1) Using the table (see below), calculate the energy (in kJ) required to break all of the bonds in 9 mole(s) of methanol (CH3OH).

2) Use the table to calculate an approximate enthalpy or heat of reaction for the combustion of one mole of methane gas (CH4) to form gaseous H2O and CO2. What Volume (in L) of methane is needed to produce 2086 kJ of heat for methane gas at 20 oC and 5.19 atm pressure?

Question

1) Using the table (see below), calculate the energy (in kJ) required to break all of the bonds in 9 mole(s) of methanol (CH3OH).

2) Use the table to calculate an approximate enthalpy or heat of reaction for the combustion of one mole of methane gas (CH4) to form gaseous H2O and CO2. What Volume (in L) of methane is needed to produce 2086 kJ of heat for methane gas at 20 oC and 5.19 atm pressure?

yb1996 · Answer

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alphadxg · Answer

@yb1996 look at the bonds between them, you need to set it up to look at the bonds interacting

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