Each test yielded its own unique set of observations, calculations and results. In order to determine these various values through calculation, the experimental data as well as the chemical reaction of calcium hydroxide was used for all calculations. The chemical equation is displayed below:
The first experiment determined the molarity of OH- and Ca2+, the Ksp and the ΔG for saturated calcium hydroxide at 21°C. In order to determine these values, the experimental data as well as the chemical reaction of calcium hydroxide was used. The molarity of OH- and Ca2+ was discovered to be 0.028 M and 0.014 M respectively. The Ksp was found to be 1.144 x 10-5 and ΔG was discovered to be 27.470 KJ/ mol. The second experiment determined the molarity of OH- and Ca2+, the Ksp and the ΔG for saturated calcium hydroxide at 60°C. The molarity of OH- and Ca2+ was discovered to be 0.029 M and 0.014 M respectively. The Ksp was found to be 1.316 x 10-5 and ΔG was discovered to be …show more content…
The ΔG is our y-value, the T is our x value and therefore the slope of the line acts as the entropy of the calcium hydroxide and the y-intercept of the line acts as our enthalpy. Based upon literature values, entropy for calcium hydroxide is 83.4 J/K mol and if entropy is converted to the correct units, this displays a value of 119.3 J/K mol (Thermodynamic quantities for substances and ions at 25˚C). Possible explanations for a greater experimental data value than true value will be discussed the Conclusions section of this report. Based on the literature values, enthalpy for calcium hydroxide is -986.1 KJ/ mol (Thermodynamic quantities for substances and ions at 25˚C). The value appears to be off by a factor of 100 according to experimental data value of entropy which is -7.9384 KJ/ mol. Possible explanations for a significantly lower experimental data value than true value will be discussed in the Conclusions section of this
The first experiment determined the molarity of OH- and Ca2+, the Ksp and the ΔG for saturated calcium hydroxide at 21°C. In order to determine these values, the experimental data as well as the chemical reaction of calcium hydroxide was used. The molarity of OH- and Ca2+ was discovered to be 0.028 M and 0.014 M respectively. The Ksp was found to be 1.144 x 10-5 and ΔG was discovered to be 27.470 KJ/ mol. The second experiment determined the molarity of OH- and Ca2+, the Ksp and the ΔG for saturated calcium hydroxide at 60°C. The molarity of OH- and Ca2+ was discovered to be 0.029 M and 0.014 M respectively. The Ksp was found to be 1.316 x 10-5 and ΔG was discovered to be …show more content…
The ΔG is our y-value, the T is our x value and therefore the slope of the line acts as the entropy of the calcium hydroxide and the y-intercept of the line acts as our enthalpy. Based upon literature values, entropy for calcium hydroxide is 83.4 J/K mol and if entropy is converted to the correct units, this displays a value of 119.3 J/K mol (Thermodynamic quantities for substances and ions at 25˚C). Possible explanations for a greater experimental data value than true value will be discussed the Conclusions section of this report. Based on the literature values, enthalpy for calcium hydroxide is -986.1 KJ/ mol (Thermodynamic quantities for substances and ions at 25˚C). The value appears to be off by a factor of 100 according to experimental data value of entropy which is -7.9384 KJ/ mol. Possible explanations for a significantly lower experimental data value than true value will be discussed in the Conclusions section of this