The following equation is balanced for the combustion reaction for C6H6: 2C6H6 +15O2 --> 12CO2 + 6H20 + 6542kJ?
2016-02-29 7:29 pm
If 6.900 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 temperature of the water?
回答 (1)
2016-02-29 7:43 pm
Let T°C be the final temperature.
Molar mass of C₆H₆ = 12×6 + 1×6 = 78 g/mol
No. of moles of water formed = 6.900/78 mol
Heat produced from burning = (6.900/78) × (6542000/2) J
Heat gained by water = m c ΔT = 5691 × 4.18 × (T - 21)
Heat gained by water = Heat produced from burning
5691 × 4.18 × (T - 21) = (6.900/78) × (6542000/2)
T - 21 = 12.2
T = 33.2
Final temperature = 33.2°C
Molar mass of C₆H₆ = 12×6 + 1×6 = 78 g/mol
No. of moles of water formed = 6.900/78 mol
Heat produced from burning = (6.900/78) × (6542000/2) J
Heat gained by water = m c ΔT = 5691 × 4.18 × (T - 21)
Heat gained by water = Heat produced from burning
5691 × 4.18 × (T - 21) = (6.900/78) × (6542000/2)
T - 21 = 12.2
T = 33.2
Final temperature = 33.2°C
收錄日期: 2021-04-18 14:42:30
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