I apologize, but I don't have access to specific tables or pages. However, I can provide you with the general steps to solve this problem using the molar enthalpy of formation of methane.
The balanced chemical equation for the combustion of methane is:
CH4 + 2O2 -> CO2 + 2H2O
The molar enthalpy of formation of methane (CH4) is -74.8 kJ/mol (according to my data source; refer to your table for more accurate values).
To find the mass of methane required to liberate 12,880 kJ of heat, we will use the following steps:
1. Determine the molar enthalpy change for the combustion of methane:
ΔH = -74.8 kJ/mol
2. Convert the given heat energy to joules:
12880 kJ = 12880000 J
3. Calculate the number of moles of heat energy released:
moles of heat = heat energy (J) / ΔH (kJ/mol)
4. Convert the moles of heat to moles of methane:
moles of methane = moles of heat
5. Convert the moles of methane to grams of methane:
grams of methane = moles of methane * molar mass of methane
The molar mass of methane (CH4) is:
C = 12.01 g/mol
H = 1.008 g/mol
Calculate the molar mass of methane:
Molar mass of CH4 = (12.01 g/mol) + (4 * 1.008 g/mol)
Plug in the values and solve the equation to find the mass of methane required to liberate 12,880 kJ of heat.
What mass of methane (CH4) must be burned in order to liberate 12,880 kJ of heat? Refer to Table 15.3 on page 529
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