Answer:
1. The balanced thermochemical equation for the reaction is;
2C4H10 (g) + 13O2 (g) -----------> 8CO2 (g) + 10H20 (g)
2. Heat when 200g of butane is burned is 9925.65 kJ of heat
Explanation:
2 moles of butane reacts with oxygen in excess to produce carbon iv oxide and water
If 1 mole releases 2877kJ of heat
2 moles will release (2 * 2877kJ) of heat
= 5754 kJ of heat.
The mass of butane used is 200g and converting it to moles we have;
n = mass / molar mass
molar mass of butane = (12 *4 + 1 *10) = 58 g/mol
So therefore n = 200 g/ 58 g/mol
n= 3.45 moles of butane.
If 1 mole of buatne releases 2877 kJ of heat
3.45 moles will release ( 3.45 * 2877 kJ ) of heat
= 9925.65 kJ of heat
9925.65 kJ of heat is released when 200 g of butane is burned.
