Answer Happy

1. You place 25.0 mL of 0.500 M NaOH in a coffee-cup calorimeter at 26.00°C and add 75.0 mL of 0.500 M HCI, also at 26.00°C) After stirring, the final temperature is 28.45°C. [Assume that the total volume is the sum of the individual volumes and that the final solution has the same density (1.00 g/mL) and specific heat capacity as water (4.184 J/g*°C).] a. First find qsoin for this reaction. Remember that qsoin = mass of reactants * specific heat capacity* AT. [5 points] b. Write a balanced equation for this reaction (reactants are NaOH and HCI, products are NaCl and H₂O). [5 points] c. Find the molar amounts of each reactant (remember, M=mol/L!) [5 points] d. Find how many moles of water are produced in this reaction (first find the limiting reagent, then calculate how much water could form using your balanced equation) [5 points] e. Calculate AHxn. Remember: qn = -Qsoln. AHxn=Qxn/mol H₂O formed. [5 points] f. BONUS: Is this an endo pr exothermic process? How do you know? [2 points]