A student carefully measures out 100.0 mL of an aqueous solution of 1.0 M HCl in

Question

A student carefully measures out 100.0 mL of an aqueous solution of 1.0 M HCl in a coffee cup calorimeter. She then carefully adds 100.0 mL of 1.0 M NaOH to the calorimeter. The initial temperature for both solutions is 20.0

A student carefully measures out 100.0 mL of an aqueous solution of 1.0 M HCl in a coffee cup calorimeter. She then carefully adds 100.0 mL of 1.0 M NaOH to the calorimeter. The initial temperature for both solutions is 20.0 degree C. Assume that the density and specific heat of the solutions is that of water. What is the final temperature of the solution? For this problem, assume that the calorimeter is a perfect insulator, and ignore the material out of which the calorimeter is made. HCl(aq)+ NaOH(aq) ?NaCl(aq)+H2O(l) ?H = -55.0 kJ/mol PLEASE EXPLAIN

Explanation / Answer

moles of naoh+ HCL

5500/(200*4.1858)=6.569

Tempearture final =20+6.569=26.569

Approx == 26.6

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