3. Butane (C4H10) releases 2877 kJ per mole during a standard combustion reaction in air.

a. What is the balanced thermochemical equation for this reaction?

b. How much heat will be released when 200.0 g of butane is burned?

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.

d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong

let that person have a turn to speak : )