Question

The reaction is as follows: CH4 + 202 + CO2 + 2H2O The enthalpy of reaction between methane ( 2 ) and oxygen ( 2 ) is exothermic (-882 kJ/mol) with respect to the dissipation of methane. It is of interest to generate 126799 kJ of energy from the combustion. How many kg of methane will need to be combusted? Molecular weight: C-12 kg/kmol H-1 kg/kmol 0 - 16 kg/kmol Select one: O a. 2.300 O b. 2300.209 O c. 1.725 O d. 0.009

Answer 1

2300j

Step-by-step explanation:

Answer 2

2300 kg of methane will need to be combusted.

Step-by-step explanation:

The enthalpy of this combustion is -882 kJ/mol CH4.

To generate 126799 kJ of energy, we need

`molCH_4=(126799kJ)/(882kJ/mol)= 143.76molCH_4`

The molecular weight of CH4 is (12+4*1)=16 g/mol

Then, the mass needed to generate 126799 kJ of energy is

`kgCH_4=143.76mol*16(g)/(mol)*(1kg)/(1000g)  =2300kgCH_4`