Answer:
[tex]-5.82\times 10^3\ kJ[/tex]
Explanation:
Given that:
The heat of combustion of methylhydrazine = [tex]-1.30\times 10^3\ kJ/mol[/tex]
It means that:
1 mole of methylhydrazine on combustion, releases [tex]1.30\times 10^3\ kJ[/tex] 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 [tex]1.30\times 10^3\ kJ[/tex] of energy
Also,
1 g of methylhydrazine on combustion, releases [tex]\frac {1.30\times 10^3}{46.072}\ kJ[/tex] of energy
206.2 g of methylhydrazine on combustion, releases [tex]\frac {1.30\times 10^3}{46.072}\times 206.2\ kJ[/tex] of energy
Heat released = [tex]-5.82\times 10^3\ kJ[/tex]
