1) when a 3.25 g sample of solid sodium hydroxide wasdissolved in a calorimeter
ID: 687663 • Letter: 1
Question
1) when a 3.25 g sample of solid sodium hydroxide wasdissolved in a calorimeter in 100.0 g of water, the temperaturerose from 23.9 C to 32 C. calculate H ( in kj/mol NaOH) forthe solution process. NaOH(s)-----Na +(aq) + OH(aq) Assume it's a perfect calorimeter and thatthe specific heat of the solution is the same as that of purewater. 1) when a 3.25 g sample of solid sodium hydroxide wasdissolved in a calorimeter in 100.0 g of water, the temperaturerose from 23.9 C to 32 C. calculate H ( in kj/mol NaOH) forthe solution process. NaOH(s)-----Na +(aq) + OH(aq) Assume it's a perfect calorimeter and thatthe specific heat of the solution is the same as that of purewater.Explanation / Answer
here heat gained/lost is = mc(T2-T1)
where, m is the mass
c is the specific heat capacity i.e 4.186 J/K-gm in case ofwater
T2-T1 is the temperature change occuring
so heat gained = 100*4.186*(32-23.9) J = 3390.66 J = 3.390 KJ now molecular weight ofsodium hudroxide is = 23+ 16 + 1 = 40 gm so no of moles of itwhen 3.25 gm is taken = 3.25/40 = 0.08125 moles so now H (inKj/mol) = 3.390/0.0821 = 41.72 KJ/mol = 3390.66 J = 3.390 KJ now molecular weight ofsodium hudroxide is = 23+ 16 + 1 = 40 gm so no of moles of itwhen 3.25 gm is taken = 3.25/40 = 0.08125 moles so now H (inKj/mol) = 3.390/0.0821 = 41.72 KJ/mol
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.