Answer:
THE ENTHALPY OF REACTION IN KJ/MOL OF CH4 IS 7.07 KJ/MOL.
Explanation:
Mass of H2 = 3 g
Molar mass of H2 = 2 g/mol
Heat released = 53.3 kJ
Equation of the reaction:
C(s) + 2H2(g) -------> CH4(g)
First:
Calculate the number of moles of H2 that was used:
Number of moles = mass / molar mass
Number of moles = 3g / 2g
Number of moles = 1.5 moles
So therefore, when 53.3 kJ of heat was released from the reaction, 1.5 moles of hydrogen was used.
From the equation of the reaction, one mole of carbon reacts with two moles of hydrogen to form one mole of methane.
For 3 g of hydrogen, 1.5 mole of hydrogen is involved.
It means:
1.5 moles of hydrogen reacts with 0.75 moles of carbon and produces 0.75 moles of methane. This is so because the reaction occurs in 1: 2: 1 in respect to carbon, hydrogen and methane respectively.
So we can say that the production of 0.75 mole of methane will evolve 53.3 kJ of heat.
0.75 mole of methane releases 53.3 kJ of heat.
1 mole of methane will release ( 53.3 kJ * 1 / 0.75 )
= 71.0666 kJ of heat
In conclusion, the enthalpy of the reaction in kJ/ mole of CH4 is 71.07 kJ/mol.
