If 5.400 g of c6h6 is burned and the heat produced from the burning is added to 5691 g of water at 21 °c, what is the final temp
2 answers:
The final temperature of the water : <u>30.506 °C</u>
<h3>Further explanation </h3>The law of conservation of energy can be applied to heat changes, i.e. the heat received / absorbed is the same as the heat released
Qin = Qout
Heat can be calculated using the formula:
Q = mc∆T
m = mass, g
∆T = temperature difference, °C / K
From reaction:
2C₆H₆ (l) + 15O₂ (g) ⟶12CO₂ (g) + 6H₂O (l) +6542 kJ, heat released by +6542 kJ to burn 2 moles of C₆H₆
If there are 5.400 g of C₆H₆ then the number of moles:
mol = mass: molar mass C₆H₆
mol = 5.4 : 78
mol C₆H₆ = 0.0692
so the heat released in combustion 0.0692 mol C₆H₆:
the heat produced from the burning is added to 5691 g of water at 21 C
So :
Q = m . c . ∆T (specific heat of water = 4,186 joules / gram ° C)
226353 = 5691 . 4.186.∆T
the difference between temperature and heat
Specific heat
relationships among temperature, heat, and thermal energy.
When heat is added to a substance
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