Posted by Dylan on Monday, March 5, 2012 at 6:51pm.
I am assuming from the way the problem is stated that dH is +252.8 kJ for the reaction as written. Then
252.8 kJ x (26/2*molar mass CH3OH) = ?
For a given sample of CH3OH, the enthalpy change during the reaction is 82.6 kJ. How many grams of methane gas are produced?
2*16 x (82.6 kJ/252.8 kJ) = ? making the same assumption as above.
yes all of these parts are derived from the same problem
How many kilojoules of heat are released when 38.4 g of CH4 (g) reacts completely with O2 (g) to form CH3OH (g) at constant pressure?
I've done two for you. Surely you don't need help on another one. They're all done the same way.
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