I have two questions:
1. A quantity of 4.00 multiplied by 102 mL of 0.600 M HNO3 is mixed with 4.00 multiplied by 102 mL of 0.300 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 17.31°C. What is the final temperature of the solution? (Assume that the densities and specific heats of the solutions are the same as for water (1.00 g/mL and 4.184 J/g·°C, respectively). Use -56.2 kJ/mol for heat of neutralization.)

2. Butane, when completely reacted with oxygen, forms carbon dioxide and water:
2 C4H10 (g) + 13 O2

Question

I have two questions:
1. A quantity of 4.00 multiplied by 102 mL of 0.600 M HNO3 is mixed with 4.00 multiplied by 102 mL of 0.300 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 17.31°C. What is the final temperature of the solution? (Assume that the densities and specific heats of the solutions are the same as for water (1.00 g/mL and 4.184 J/g·°C, respectively). Use -56.2 kJ/mol for heat of neutralization.)

2. Butane, when completely reacted with oxygen, forms carbon dioxide and water:
2 C4H10 (g) + 13 O2

anonymous · Answer

2 C4H10 (g) + 13 O2 (g) 8 CO2 (g) + 10 H2O (l) ΔH = - 5314 kJ
 How much butane must be reacted to produce 6375 kJ of heat? 

(question 2 got cut off)