Heat of solution per mole of compound kJ/mol Heat of Neutralization Initial temp

Question

Heat of solution per mole of compound kJ/mol Heat of Neutralization Initial temperature of HCl solution Initial temperature of NaOH solution Final temperature of neutralized mixture Change in temperature. Delta t (use the average of the initial temperatures of HCl and NaOH) q_H_2O (assume 50.0 mL of solution and use average density of 1.02 g/mL) Total Delta H for the neutralization reaction Delta H per mole of H^+ and OH^- ions reacting kJ/mol The value of Delta H will be approximate tor several reasons. One is that we do not include the amount of heat absorbed by the solute. This effect is smaller than the likely experimental error, and thus we will ignore it.

Explanation / Answer

Density = 1.02 g/mL

then mass of 50.0 mL of solution = 1.02 * 50.0 = 51 g.

Then, moles of solution = 51.0 / 18 = 2.83 mol

Therfore, delta H = q / n

Delata H = 2899.25 / 2.83 = 1024.47 J

HCl (aq.) + NaOH (aq.) -------------> NaCl (aq.) + H2O (l)

H+ (aq.) + OH- (aq.) -------------> H2O (l)

Delta H per mole of H+ and OH- ions reacting = 1024.47 J

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