Question

How much heat was released during the combustion of 1.00 g of dimethylphthalate?

Answer 1

Answer:

The problem provides you with the thermochemical equation that describes the combustion of methane, CH4

CH4(g)+2O2(g)→CO2(g)+2H2O(g) ΔH=−802.3 kJ mol−1

The enthalpy change of combustion, given here as ΔH, tells you how much heat is either absorbed or released by the combustion of one mole of a substance.

In your case, the enthalpy change of combustion

ΔH=−802.3 kJ mol−1

suggests that the combustion of one mole of methane gives off, hence the minus sign, 802.3 kJ of heat.

Your strategy here will be to use the molar mass of methane to convert your sample from grams to moles

Answer 2

Explanation:

The problem provides you with the thermochemical equation that describes the combustion of methane, CH4

CH4(g)+202(g)+CO2(g)+2H2O(g) AH=-802.3 kJ mol-1

The enthalpy change of combustion, given here as AH, tells you how much heat is either absorbed or released by the combustion of one mole of a substance.

In your case, the enthalpy change of combustion

AH -802.3 kJ mol-1

The enthalpy change of combustion, given here as AH, tells you how much heat is either absorbed or released by the combustion of one mole of a substance.

In your case, the enthalpy change of combustion

AH=-802.3 kJ mol-1

suggests that the combustion of one mole of methane gives off, hence the minus sign, 802.3 kJ of heat.

Your strategy here will be to use the molar mass of methane to convert your sample from grams to moles