Question

CH4 + 2O2 → CO2 + 2H2O, ΔH = -890 kJ/mol How much energy is released when 59.7 grams of methane (CH4) reacts with oxygen?

Answer 1

Answer: I also believe that the negative sign indicates the heat is released. So, 3321 kJ of heat is released by the combustion of 59.7 grams of methane.

Answer 2

Answer:- 3321 kJ of heat is released.

Solution:- The given balanced equation is:

`CH_4+2O_2\rightarrow CO_2+2H_2O, \Delta H=-890(kJ)/(mol)`

From this balanced combustion equation, 890 kJ of heat is released by the combustion of 1 mol of methane.

We could convert given grams of methane to moles and multiply by the delta H value of the reaction to get the total heat released by the combustion of 59.7 grams of methane as:

`59.7gCH_4((1mol)/(16g))((-890kJ)/(1molCH_4))`

= -3321 kJ

The negative sign indicates the heat is released. So, 3321 kJ of heat is released by the combustion of 59.7 grams of methane.