Answer:
23.7 kg is the mass of H₂O that can be heated
Explanation:
First of all, we need to determine the heat used.
891 kJ per mol of methane is released in the combustion, but we don't have 1 mol, we have 143 g
We convert the mass to moles → 143 g . 1mol / 16 g = 8.93 moles
Now, a rule of three:
1 mol of CH₄ release a heat of 891 kJ
8.93 moles of CH₄ will release (8.93 . 891 kJ) / 1 = 7956.63 kJ
If we convert to J → 7956.63 kJ . 1000 J / kJ = 7956630 Joules
Now we determined the heat released, we can apply the calorimetry formula
Q = m . C . (Final T° - Initial T°)
7956630 J = mass . 4.184 J/g°C ( 95°C - 15°C)
7956630 J / 4.184 J/g°C . 80°C = mass
23771 g = mass
If we convert from g to kg → 23771 g . 1kg / 1000 g = 23.7 kg
