Can someone explain in detail the steps to do thisproblem? A quantity of 4.00 x 102 mL of 0.600MHNO3 is mixed with 4.00 x 102 mL of 0.300MBa(OH)2 in a constant-pressure calorimeter of negligibleheat capacity. The initial temperature of both solutions is thesame at 18.46oC. What is the final temperature of thesolution? (Use heat of neutralization = -56.2 kJ/mol) Can someone explain in detail the steps to do thisproblem? A quantity of 4.00 x 102 mL of 0.600MHNO3 is mixed with 4.00 x 102 mL of 0.300MBa(OH)2 in a constant-pressure calorimeter of negligibleheat capacity. The initial temperature of both solutions is thesame at 18.46oC. What is the final temperature of thesolution? (Use heat of neutralization = -56.2 kJ/mol)
Explanation / Answer
Balanced chemical equation : Ba(OH)2 + 2HNO3 ---------- >Ba(NO3)2 + 2 H2O 1 mol of barium hydroxide reacts with 2 mols of nitric acid. Number of mols of Ba(OH)2 = 0.4 Lx 0.300 M = 0.12 mols Number of mols of HNO3 = 0.4 L x 0.600 M =0.24 mols 0.12 mols of barium hydroxide neutralised by 0.24 mols ofnitric acid. For 1 mol heat of neutralization = -56.2 kJ For 0.24 mols of acid heat of neutralisation is -56.2kJ x 0.24 mols = -13.488 x 103 qsoln = m x s x T =800 g x 4.184 J / 0C g x ( T -18.46oC ) ( since density of water 1.0 / mL) q rxn = - q soln - 800 g x 4.184 J / 0C g x (T - 18.46oC ) = -13.488 x 103 J ( T - 18.46oC ) = -13.488 x 103 J/ - 800 g x 4.184 J / 0C g = 4.020C T = ( 4.02 + 18.46) 0C = 22.48 0C