How much heat will be produced when 16grams of C2H6 burns? The reaction is

2 C2H6 + 7 O2 --> 4CO2 + 6 H20 triangle heat = -350kJ

To find out how much heat will be produced when 16 grams of C2H6 (ethane) burns, we need to use stoichiometry and the given reaction equation.

The reaction equation states that 2 moles of C2H6 react with 7 moles of O2 to produce 4 moles of CO2 and 6 moles of H2O, with the release of 350 kJ of heat.

First, we need to find the number of moles of C2H6 in 16 grams. To do this, we use the molar mass of ethane (C2H6), which is 30.07 g/mol (based on the atomic masses of carbon and hydrogen).

Number of moles = Mass / Molar mass
Number of moles = 16 g / 30.07 g/mol = 0.532 mol (rounded to 3 decimal places)

Since the stoichiometric ratio between C2H6 and the heat released is 2:350 (moles of C2H6:kJ of heat), we can set up a proportion to find the heat produced when 0.532 moles of C2H6 react.

Proportion: 2 moles C2H6 / 350 kJ = 0.532 moles C2H6 / x kJ

Cross-multiplying and solving for x, we get:

x kJ = (0.532 moles C2H6 * 350 kJ) / 2 moles C2H6
x kJ = 92.8 kJ

Therefore, when 16 grams of C2H6 burns, it will produce approximately 92.8 kJ of heat.