Using the following information and the fact that the average c―h bond enthalpy is 414 kj/mol, estimate the standard enthalpy of formation of methane (ch4). c(s) → c(g) δh o rxn = 716 kj/mol 2h2(g) → 4h(g) δh o rxn = 872.8 kj/mol

The standard enthalpy of formation of methane is -67.2 kJ/mol.

Explanation:

...[1]

...[2]

...[3]

Since, the bond formation is taking place energy will release that id reaction will be an exothermic reaction

...[4]

Using Hess's law:

[4] = [1] + [2] + [3]

The standard enthalpy of formation of methane is -67.2 kJ/mol.

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explanation:

in scientific notation, the value of the  speed of light in a vacuum

  will be written as 2.995 * 10^8. when this value is represented in the form of

  a * 10^b, then, a = 2.995 and b = 8.

the value of the speed of light in a vacuum given above can also be rounded up to approximately 300000000. in this case, the scientific notation will be written as 3 *10^8.