Heat energy produced by combustion of 6.05 g of Benzene ( C6H6 ):
(6.05 g C6H6) / (78.11236 g C6H6/mol) x (3.27 x 10^6 J/mol) = 253269.7 J
This heat enegy is absorbed by the water . Thus the tempature raised is
delta T = Q / mc
(253269.7 J ) / (4.183 J/g·°C) / (5690 g) = 10.6 °C
Thus, the temperature of water will be
21.0°C + 10.6 °C = 31.6°C
When one mole of C_6 H_6 is burned, 3.27 MJ of heat is produced. When the...
When one mole of CH is burned, 3.27 MJ of heat is produced. When the heat from burning 5.55 g of C, H, is added to 5.69 kg of water at 21.0 °C, what is the final temperature of the water?
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The balanced combustion reaction for C6H6 is 2C6H6(l)+15O2(g) --> 12CO2(g)+6H2O(l)+6542kJ If 8.000 g C6H6 is burned and the heat produced from the burning is added to 5692 g of water at 21 C, what is the final temperature of the water? final temperature: _________________ C
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The balanced combustion reaction for C6H6 is 2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6542 kJ If 5.500 g 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?
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Combustion of the reaction for one mole of liquid Acetone DeltarH= -1755 kj/mol DeltarU=-1753 kj/mol C3H6O + 4O2 (g) -> 3CO2 (g) + 3H2O a) If you were using a bomb calorimeter , what mass of the Water could be heated form 21.0 celsius to 61.0 celsius by burning 0.6g of Acetone in the calorimeter. The specific heat of the Water is 4.184 j/g c b) What would the heat capacity of the calorimeter as whole if the burning of...
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