The complete combustion of acetylene, c2h2(g), produces 1300. kj of energy per mole of acetylene consumed. how many grams of acetylene must be burned to produce enough heat to raise the temperature of 1.00 gal of water by 12.0°c if the process is 88.0% efficient? assume the density of water is 1.00 g/cm3.

The combustion of acetylene produces a tremendous amount of energy 3.34g of acetylene is required in the reaction.

Let us calculate the energy absorbed by the water, this will give us the theoretical amount of acetylene.

ΔH = mcθ

m = mass of water

c = heat capacity of water = 4.18 J/g/°C

θ = temperature rise = 12.0°C

Volume of water =  1.00 gal = 3785cm^3

Density of water = 1.00 g/cm3

Mass of water = 3785 g

Substituting values;

ΔH = 3785 g × 4.18 J/g/°C ×  12.0°C

ΔH = 189.86 KJ

If 1 mole of acetylene yield 1300. kJ of energy

x moles yields  189.86 KJ

x =   189.86 KJ ×  1 mole/ 1300. kJ

x =e = 0.146 moles

Mass of acetylene = 0.146 moles × 26 g/mol = 3.796 g

This is the theoretical mass of acetylene required.

Actual mass of acetylene required is obtained from;

88 = actual/3.796 g × 100/1

actual = 88 × 3.796 g/ 100

actual = 3.34g

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the answer is c i believe

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error