Consider the following reaction: 2ch3oh(g)  2ch4(g) + o2(g) δh = +252.8 kj a) calculate the amount of heat transferred when 24.0 g of ch3oh(g) is decomposed by this reaction at constant pressure. b) for a given sample of ch3oh, the enthalpy change during the reaction is 82.1 kj. how many grams of methane gas are produced?

For a: The amount of heat transferred for the given amount of methanol is 94.6736 kJ.

For b: The mass of methane gas produced will be 10.384 g.

Explanation:

For the given chemical reaction:

To calculate the number of moles, we use the equation:

......(1)

Given mass of methanol = 24.0 g

Molar mass of methanol = 32.04 g/mol

Putting values in above equation, we get:

By Stoichiometry of the reaction:

For every 2 moles of methanol, the amount of heat transferred is +252.8 kJ.

So, for every 0.749 moles of methanol, the amount of heat transferred will be =

Hence, the amount of heat transferred for the given amount of methanol is 94.6736 kJ.

By Stoichiometry of the reaction:

252.8 kJ of energy is absorbed when 2 moles of methane gas is produced.

So, 82.1 kJ of energy will be absorbed when = of methane gas is produced.

Now, calculating the mass of methane gas from equation 1, we get:

Molar mass of methane gas = 16 g/mol

Moles of methane gas = 0.649 moles

Putting values in equation 1, we get:

Hence, the mass of methane gas produced will be 10.384 g.

since electrons are negative the answer is neagtaive