Enter your answer in the provided box. A quantity of 5.70 x 10 mL of 0.900 MHNO,
ID: 696424 • Letter: E
Question
Enter your answer in the provided box. A quantity of 5.70 x 10 mL of 0.900 MHNO, is mixed with 5.70 x 10 mL of 0.450 M Ba(OB), in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 18.46°C. The heat of neutralization when 1.00 mol of HNO, reacts with 0.500 mol Ba(OH)2 is-56.2 kJ/mol. Assume that the densities and specific heats of the solution are the same as for water ( 1.00 g/mL and 4.184 J/g·°C, respectively). What is the final temperature of the solution?Explanation / Answer
no of mol of Ba(OH)2 added = 570*0.45/1000 = 0.2565 mol
no of mol of HNO3 = 570*0.9 = 0.513 mol
Ba(OH)2(aq) + 2HNO3(aq) ---> Ba(NO3)2(aq) + 2H2O(l)
1 mol Ba(OH)2(aq) = 2 mol HNO3(aq)
heat liberated = 56.2*0.513/1 = 28.83 kj
heat liberated = m*s*DT
28.83*10^3 = (570+570)*4.184*(x-18.46)
x = final temperature = 24.5 C
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