In: Chemistry
Find ∆H and ∆S for the following data.
Calculate percent errors for the enthalpy and entropy of reaction using the following literature values: ∆H = 110 kJ/mol, ∆S = 380J/mol*K
Standardized HCl = .5087M
Ksp = [Na^+]^2[Borox^2-]
ln(Ksp) = -∆H/RT + ∆S/R
Temperature of solution;Amount of HCl needed to titrate borox;Volume aliquot
Trial 1 - 295K;2.50mL;5.8mL
Trial 2 - 316K;5.76mL;5.4mL
Trial 3 - 309K;4.57mL;5.6mL
Trial 4 - 305K;4.34mL;6.5mL
Trial 5 - 311K;7.70mL;5.8mL
Trial 6 - 310K;7.73mL;6.1mL
After I calculated everything and graphed it, I got ∆S to be 14.5495 J and I got ∆H to be 4,306 J.
My R^2 value was .415
My equation for best fit line was y = -5.18E+02x + 1.75E+00.
Please help me with this problem as I feel like I've done it totally wrong.