Calculate the standard enthalpy of combustion of a methane sample by using the standard enthalpies of formation.

Write the equation and balance it. CH4 + 2O2 --> CO2 + 2H2O Assign the enthalpies of formation and the sign of the energy value with the corresponding molecule (Will demonstrate my technique if needed). e.g. C(s) + 2H2(g) --> CH4(g) Delta H(f) = -74.87

Generate an equation will all assigned values and the single unknown Delta H(combustion/c). Rearrange for Delta H(c). Answer is - 890.63 KJ/mol.

AC
Answered by Axel C. Chemistry tutor

25879 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Phosphorus(III) chloride molecules are pyramidal with a bond angle less than 109.5°. Explain why a phosphorus(III) chloride molecule has this shape and bond angle.


How does Hydrogen bonding arise in Water?


State an explain the result of an increase in temperature on the following equilibria: N2 (g) + 02 (g) <-> 2 NO (g) (delta H = +180kJmol-1)


Methylpropene reacts with hydrogen bromide to form 2-bromo-2-methylpropane, draw the mechanism and state the major products.


We're here to help

contact us iconContact ustelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences