Heats of combustion of cycloalkane homologues
Have a look at this table from Organic Chemistry by Wade and Simek [1, p. 134]:


  


Every time a $\ce{-CH2}$ group is added, the heat of combustion is increased by almost 650 kJ/mol; whereas the maximum relief in ring strain attained by adding that $\ce{-CH2}$ group is not more than 25 kJ/mol.

So there is no competiton between increase in heat of combustion due to more number of carbon atoms and decrease in it caused by ring stability. Everytime you see two hydrocarbons with different number of carbon atoms, be assured that the one with more carbon will realease more heat on combustion.

P.S. If in case you are unfamiliar with how ring strain is quantitatively measured [1, p. 133]:


  The molar heat of combustion of cyclohexane is nearly twice that of cyclopropane, simply because cyclohexane contains twice as many methylene ($\ce{-CH2}$) groups per mole. To compare the relative stabilities of cycloalkanes, we divide the heat of combustion by the number of methylene ($\ce{-CH2}$) groups. The result is the energy per $\ce{-CH2}$ group. These normalized energies allow us to compare the relative amounts of ring strain (per methylene group) in the cycloalkanes. The reference value of 658.6 kJ (157.4 kcal) per mole of $\ce{-CH2}$ groups comes from an unstrained long-chain alkane.


References


Wade, L. G.; Simek, J. W. Organic Chemistry, 9th ed.; Pearson: Glenview, IL, 2017. ISBN 978-0-321-97137-1.