zannasheayarrow
Member
Hi guys, I am having trouble with what should really be an easy question. I think I am just missing something because I'm getting half what the answers say it is. It is from the Conquering Chemistry HSC textbook:
When 25mL of a solution at 23.2 degrees C containing 5.00 x 10^-3 mol NaOH was mixed with 50mL of a solution also at 23.2 degrees C that contained 6.00x10^-3 mol HCl in a light plastic beaker, the final temperature of the mixture was 24.1 degrees c. Calculate the heat released and hence the enthalpy change per mole for this neutralisation reaction. Take the density and specific heat capacity of all solutions involved as 1.00g/mL and 4.2 J K^-1 g^-1 respectively, assume that the container had negligible heat capacity and that heat losses to the surroundings were negligible.
Thanks!
When 25mL of a solution at 23.2 degrees C containing 5.00 x 10^-3 mol NaOH was mixed with 50mL of a solution also at 23.2 degrees C that contained 6.00x10^-3 mol HCl in a light plastic beaker, the final temperature of the mixture was 24.1 degrees c. Calculate the heat released and hence the enthalpy change per mole for this neutralisation reaction. Take the density and specific heat capacity of all solutions involved as 1.00g/mL and 4.2 J K^-1 g^-1 respectively, assume that the container had negligible heat capacity and that heat losses to the surroundings were negligible.
Thanks!