posted by Carrie on .
This is a lab I have, but have no clue what to do. Please do out the steps so i can understand.
Reactions and Data:
NaOH(s)--> Na1+(aq)+ OH1-(aq)
(Heat of solution of NaOH)
This reaction involves adding solid NaOH to water and watching the temperature change as it dissolves.
Trial 1: 1.98 g of solid NaOH is dissolved in 106.5 mL of water. The temperature goes from 22.00°C to 26.50°C.
Hints:Remember that you are heating water. Use the formula Q = C x M x DT. The volume of water used equals the volume of whatever solution you are using, be it NaOH or HCl. The volume must be converted to mass (1 mL of water has a mass of 1 g). The mass must be reported in kilograms.
Questions and Calculations
For each of the three reactions:
1) Calculate the heat evolved in each trial (Q).
2) Calculate the moles of NaOH used in each trial (mol).
3) Calculate how much heat would be evolved if 1 mole of NaOH was used for each trial (Q/mol).
4) Calculate the average heat per mole in each of the 3 reactions.
How can I help? The instructions are plain:
1. Calculate q from mass H2O x heat capacity H2O x delta T H2O.
2. moles NaOH = grams NaOH/molar mass NaOH.
3. q you found/moles NaOH will give you q/mol
4. Average the results of the trials.