Moles of benzene burnt = mass / molar mass = 6.5 / 78 = 0.0833 moles
Heat released on burning 2 moles = 6542 KJ
Moles obtained by burning 0.0833 moles = 0.0833 * 6542 / 2 = 272.47 KJ
Heat = mass of water * Specific heat of water * Temperarture change
272.47 * 103 = 5691 * 4.184 * (T - 21)
Solving, T = 21+11.44 = 22.44 0C
The balanced combustion reaction for CH is | 2C,H,(1) + 150,(g) – 12 CO,(g) + 6...
The balanced combustion reaction for C H is 2C,H,)+150,(g)12 CO,(g) +6H,O) +6542 kJ If 7.800 g C, H, 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? C final temperature
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Attempt 4 Question 8 of 16 The balanced combustion reaction for C,H, is 2C,H,)+150,(g)12CO, (g)+6 H,O0)+6542 kJ w If 6.200 g C,H 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? final temperature: 18.76 °C privacy policy tems of use contact us help about un careen etv 24 MacBook Pro Q Search or enter website name & 7 8 6 5 3...
The balanced combustion reaction for C6H6 is 2 C6H6(l) + 15 O2 (g) -----> 12 CO2 (g) + 6 H2O(l) + 6542 kJ If 8.800 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? final temperature= ___________ C