Question

Methylhydrazine, CH6N2, is commonly used as a liquid rocket fuel. The heat of combustion of methylhydrazine is −1.30 × 103 kJ/mol. How much heat is released when 206.2 g of methylhydrazine is burned? If appropriate, express your answer in scientific notion. (Click on the answer box to show the pallet.)

Answer 1

Answer:

$-5.82\times 10^3\ kJ$

Explanation:

Given that:

The heat of combustion of methylhydrazine = $-1.30\times 10^3\ kJ/mol$

It means that:

1 mole of methylhydrazine on combustion, releases $1.30\times 10^3\ kJ$ of energy

Molar mass of ‎methylhydrazine = 46.072 g/mol

Means that, 1 mole of methylhydrazine contains 46.072 g of methylhydrazine

Thus,

46.072 g of methylhydrazine on combustion, releases $1.30\times 10^3\ kJ$ of energy

Also,

1 g of methylhydrazine on combustion, releases $\frac {1.30\times 10^3}{46.072}\ kJ$ of energy

206.2 g of methylhydrazine on combustion, releases $\frac {1.30\times 10^3}{46.072}\times 206.2\ kJ$ of energy

Heat released = $-5.82\times 10^3\ kJ$