A quantity of 3.30 × 102 mL of 0.500 M HNO3 is mixed with 3.30 × 102 mL of 0.250 M Ba(OH)2 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 HNO3 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?

asked by Brandon

2 years ago

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1 answer

q = mass H2O x specific heat H2O x Tfinal-Tinitial)
56,200 J = 660 g x 4.184 J/g*C x (Tfinal-18.46)
Solve for Tfinal. Post your work if you get stuck.

answered by DrBob222

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Question

A quantity of 3.30 × 102 mL of 0.500 M HNO3 is mixed with 3.30 × 102 mL of 0.250 M Ba(OH)2 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 HNO3 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?

1 answer

q = mass H2O x specific heat H2O x Tfinal-Tinitial)
56,200 J = 660 g x 4.184 J/g*C x (Tfinal-18.46)
Solve for Tfinal. Post your work if you get stuck.

DrBob222 · Answer

q = mass H2O x specific heat H2O x Tfinal-Tinitial) 56,200 J = 660 g x 4.184 J/g*C x (Tfinal-18.46) Solve for Tfinal. Post your work if you get stuck.