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A quantity of 2.30 × 102 mL of 0.900 M HNO3 is mixed with 2.30...

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Chemistry

A quantity of 2.30 × 102 mL of 0.900 M HNO3 is mixed with 2.30 ×102 mL of 0.450 M Ba(OH)2 in a constant-pressure calorimeter ofnegligible heat capacity. The initial temperature of both solutionsis the same at 18.46°C. The heat of neutralization when 1.00 mol ofHNO3 reacts with 0.500 mol Ba(OH)2 is −56.2 kJ/mol. Assume that thedensities and specific heats of the solution are the same as forwater (1.00 g/mL and 4.184 J/g · °C, respectively). What is thefinal temperature of the solution? (in C)

Answer & Explanation Solved by verified expert
4.3 Ratings (857 Votes)
Final temperature of the solution 2450 oC Explanation molarity HNO3 0900 M volume HNO3 230 mL 0230 L moles HNO3 molarity HNO3 volume HNO3 in Liter moles HNO3    See Answer
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