When 2.5g of NaOH were dissolved in 49.0g water in a calorimeter at 24.0 C, the temperature of the solution went up to 37.1 C.
a. Is the solution reaction exothermic?
Why? The temperature or the water went from 24.0 to 37.1 which is an increase. If the solution of NaOH in water made the temperature of the water go up, do you think the NaOH + H2O gave off heat (exothermic) or took in heat (endothermic)?
b. Calculate q h2o, using eq. 1. Its tough to know what you did when you don't supply equation 1.
c. Find delta H for the reaction as it occured in the calorimeter (eq. 5).See comment to part b.
d. Find delta H for the solution of 1.00g NaOH in water. The delta H you found was for 2.5g. What would it be for 1.0g?
Find delta H for the solution of 1 mole NaOH in water. The delta H you found for part d was for 1.0g. A mol of NaOH is 40g. Just convert from 1.0g to 40g.
f. given that NaOH exists as Na+ and OH- ions in solution, write the equation for the reaction that occurs when NaOH is dissolved in water. NaOH(s) ==> Na+(aq) + OH-(aq) + heat
g. Using ethalpies of formation as given in thermodynamic tables, calculate delta H for the reaction in part f and compare your answer with the result obtained in Part e. You must look up the delta Hf.
Please explain how to do. All of this is new to me. Thank you so much!
When 2.5g of NaOH were dissolved in 49.0g water in a calorimeter at 24.0 C, the temperature of the solution went up to 37.1 C.
a. Is the solution reaction exothermic?
Why?
b. Calculate q h2o, using eq. 1.
c. Find delta H for the reaction as it occured in the calorimeter (eq. 5).
d. Find delta H for the solution of 1.00g NaOH in water.
Find delta H for the solution of 1 mole NaOH in water.
f. given that NaOH exists as Na+ and OH- ions in solution, write the equation for the reaction that occurs when NaOH is dissolved in water.
g. Using ethalpies of formation as given in thermodynamic tables, calculate delta H for the reaction in part f and compare your answer with the result obtained in Part e.
1 answer