Chemistry

consider the following reaction:
2CH3OH(g) yields 2CH4(g) + O2(g) change in enthalpy= 252.8kJ

Calculate the amount of heat transferred when 26.0 g of {\rm CH_3OH} (g) is decomposed by this reaction at constant pressure.

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  1. 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) = ?

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  2. For a given sample of CH3OH, the enthalpy change during the reaction is 82.6 kJ. How many grams of methane gas are produced?

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  3. 2*16 x (82.6 kJ/252.8 kJ) = ? making the same assumption as above.

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  4. 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?

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  5. 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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  6. beads?

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