Question

In: Chemistry

Find ∆H and ∆S for the following data. Calculate percent errors for the enthalpy and entropy...

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.

Solutions

Expert Solution


Related Solutions

for a diatomic perfect gas , derive the equation for entropy S , enthalpy H ,...
for a diatomic perfect gas , derive the equation for entropy S , enthalpy H , Gibbs energy G . and Helmholtz energy A
1. Calculate the standard reaction entropy, enthalpy and Gibbs free energy for the following reactions a)...
1. Calculate the standard reaction entropy, enthalpy and Gibbs free energy for the following reactions a) N2(g) + NO2(g) ---> NO(g) + N2O(g) and b) 2F2(g) +2H2O(l) ---> 4HF(aq) + O2(g)
Use standard enthalpy and entropy data from Appendix G to calculate the standard free energy change...
Use standard enthalpy and entropy data from Appendix G to calculate the standard free energy change for the reaction shown here (298 K). What does the computed value for ΔG° say about the spontaneity of this process? C2 H6(g) ⟶ H2(g) + C2 H4(g)
Calculate the enthalpy and entropy of the saturated vapor of isobutane at 360 K from the...
Calculate the enthalpy and entropy of the saturated vapor of isobutane at 360 K from the following information: 1. Table 6.1 provides the compression factor information (Z values) for isobutane vapor. 2. The vapor pressure of isobutane at 360 K is 15.41 bar. 3. Consider H0g = 18 115.0 J mol ^ -1 and S0g = 295.976 J mol ^ -1* K ^ -1 for the reference state of an ideal gas at 300 K and 1 bar. 4. The...
Calculate the standard enthalpy of formation of solid AlCl3 from the following data: 2 Al(s) +...
Calculate the standard enthalpy of formation of solid AlCl3 from the following data: 2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g)                  ΔHo = -1048 kJ HCl(aq) → HCl(g)                  ΔHo = 75 kJ Cl2(g) + H2(g) → 2 HCl(g)                      ΔHo = -186 kJ AlCl3(s) → AlCl3(aq)                                                       ΔHo = -323 kJ
Using the standard values of enthalpy changes (ΔH°) and entropy change (ΔS°) to calculate the Gibbs...
Using the standard values of enthalpy changes (ΔH°) and entropy change (ΔS°) to calculate the Gibbs free energy change for the production of following metallic elements from their ore sources: (a) 2ZnO(s) 2Zn(s) + O2(g) (b) 2CaO(s) 2Ca(s) + O2(g) (c) 2Al2O3(s) 4Al(s) + 3O2(g) (d) 2MgO(s) 2Mg(s) + O2(g)
calculate the molar enthalpy Zn+2HCl→ZnCl2+H2 -80.7kj/mol Zn+1/2O2→ZnO ? ZnO​(s)​ + H+​ ​ ​→​ H​2O​ ​(l)​ +...
calculate the molar enthalpy Zn+2HCl→ZnCl2+H2 -80.7kj/mol Zn+1/2O2→ZnO ? ZnO​(s)​ + H+​ ​ ​→​ H​2O​ ​(l)​ + Zn2​ +​(aq) and using 1 g of solid zinc oxide (with enough acid) only gives 0.235 kJ of heat. And finally, the heat of formation of liquid water is -285.9 kJ/mol.
Calculate the enthalpy, entropy, and Gibbs free energy of mixing when 1.00 mol hexane is mixed...
Calculate the enthalpy, entropy, and Gibbs free energy of mixing when 1.00 mol hexane is mixed with 1.00 mol heptane at 298 K. You may treat this solution as ideal. Sketch the plot of entropy of mixing vs. mole fraction, and then sketch another plot for entropy vs. mass fraction. Calculate the mass fractions of hexane and heptane that would provide the greatest entropy of mixing.
Calculate the change of enthalpy for: 4S + 6O2= 4SO3 Delta H= ___ kJ
Calculate the change of enthalpy for: 4S + 6O2= 4SO3 Delta H= ___ kJ
Calculate enthalpy for the following reaction Ca(s) + 1/2O2 + CO2 = CaCo3 Given the following...
Calculate enthalpy for the following reaction Ca(s) + 1/2O2 + CO2 = CaCo3 Given the following reactions: Ca(s) + 1/2 O2 = CaO (s) H= -635.1 kj CaCo3 = CaO (s) + CO2 H= 178.3 kj
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT