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.

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.

lol idk man i guess u gotta ask bill nye the science guy