Question

How many kcal are produced when 32.0g of CH4 react? CH4 + 2O2 = CO2 + 2H2O + 218 kcal

Answer 1

Answer:

mass of 1 mole  

=number of moles*molar mass  

=1*(12+4*1)  

=16g  

So twice as much methane is reacted than the equation, so twice as much energy is released.  

Therefore, the answer is (e) 436kcal

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Answer 2

Answer:

On burning 32g of methane 436kcal energy will be released.

Explanation:

Molecular mass of methane ($CH_4$) = 16g/mol

Given the mass of methane ($CH_4$) = 32g

Moles of methane ($CH_4$) = $\frac{32}{16}$ moles

Moles of methane ($CH_4$) = 2 moles

According to the reaction:

$\[C{H_4} + 2{O_2} \to C{O_2} + 2{H_2}O + 218kcal\]$

On the burning of one mole of methane 218kcal energy is released.

On the burning of 2 moles of methane 2×218kcal energy will be released.

Therefore, 436kcal energy will be released on the burning of 2 moles of methane.