The two were mixed together at exactly 400 min in calorimeter and the

The two were mixed together at exactly 400 min in

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The two were mixed together at exactly 4.00 min in calorimeter and the temperature was obtained and recorded for a duration of 4.50 min with at least 8 readings. After collecting the readings, a graph was created to obtain the final temperature (Tf) of the reaction mixture. To obtain the final temperature of the reaction, the graph was used. The linearly declining temperature points after the maximum temp was used to capture the equation of the line for the selected data. The equation, Temp=mt+b was used to calculate what the temperature should have been at the time of mixing (4.00 min). The heat of neutralization per mole of water formed- H(rxn/dissolution)=5.7KJ/mol For trial #2 , HN O 3 ( aq ) + NaOH (aq) NaNO3 (aq) + H2O (l) (Heat of Neutralization) Repeat the procedure for trials #1 using 1.0 M HNO3 instead of HCL. The heat of neutralization per mole of water formed- H(rxn/dissolution)=(-66.96 kj/mol)
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3 For trial #3, NaOH(s) NaOH(aq) (Heat of Solution) 50.0 ml of deionized water was carefully measured and put into the calorimeter to obtain initial temperature readings at 30 -second intervals for 3 minutes. After turning on the stirrer bar, at the 4rth minute the carefully measured 2g of solid NaOH was added and continued to collect the temperatures of the reactants at 9 minutes. A graph was used just like trail #1 and #2 to obtain the final temperature of the solution from the equation. The heat of solution per mole of NaOH was calculated to be (-0.04936 kj/mol)
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