Consider the following reaction:
2ch3oh(g)→2ch4(g)+o2(g)δh=+252.8kj< br /> calculate the amount of heat transferred when 27.0g of ch3oh(g) is decomposed by this reaction at constant pressure.

if someone could me with the steps i can figure it out on my own, you so much

Answer : The amount of heat transferred in the reaction is 213.4 kJ

Explanation :

Mass of = 27.0 g

Molar mass of = 32 g/mole

Enthalpy of reaction = +252.8 kJ

First we have to calculate the moles of .

Now we have to calculate the amount of heat transferred in the reaction.

The given balanced chemical reaction is:

From the reaction, we conclude that

As, 2 moles of transfer heat = 252.8 kJ

So, 0.844 moles of transfer heat = 0.844 × (252.8 kJ)

                                                                                      =  213.4 kJ

Therefore, the amount of heat transferred in the reaction is 213.4 kJ

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2