6. Write the equilibrium constant expression and calculate the value of the equilibrium constant for each of the following reactions at 298K, using data in your Appendix B. a) NaHCO3 (s) [pic] NaOH (s) + CO2 (g) b) 2 HBr (g) + Cl2 (g) [pic] 2 HCl (g) + Br2 (g) c) 2 SO2 (g) + O2 (g) [pic] 2 SO3
If the reaction is first order, its graphical representation is seen as ln[A] (natural log of concentration) vs. time, and the slope of its like is also the negative rate constant. Finally, for a second order reaction the graph is shown as 1/[A] (inverse of concentration) vs. time, and the slope of its given line is the positive rate constant. By understanding the rate law and finding the value of the correct rate constant with respect to the order of the reaction, one can determine the half-life of the crystal violet. This is because the crystal violet undergoes a decay reaction with the sodium hydroxide. According to Beer's Law, the absorbance of crystal violet is proportional to its concentration.
Abstract The interaction at equilibrium between acids and bases during a titration can be used to determine several characteristics of the acid or the base. In this experiment 0.05 M of KHP titrate with the strong base NaOH. From the plot of pH versus the volume of sodium hydroxide added was found that acid ionization constant Ka for KHP at half point was equal to 8.3176x10-6, also the dissociation constant Kb for conjugate base of weak acid was equal to 1x10-9. This value was established by observing the pH versus volume of NaOH graph. The equivalence point of titration occurred at a volume of 31 mL 0.081M NaOH (aq).
Ashley Peccatiello Experiment 7 – Dehydration of 2-Methylclyclohexanol, Tests for Unsaturation, and Gas Chromatography Date Performed: October 25, 2012 Date Written: October 29, 2012 Purpose: To dehydrate 2-methylclyclohexanol to obtain two isomers. To separate the products by simple distillation. To analyze the sample by introducing the technique of gas chromatography and unsaturation tests. Reaction: Figure 1. Overall reaction of the acid-catalyzed dehydration of 2-methylcyclohexanol Figure 2.
The relative reactivity of the hydrogens H1, H2, H3 , and H4 were 0.37, 1.4, 2.9, and 1.0 respectively. The radical chlorination of 1-chlorobutane follows the radical reaction mechanism. Abstraction of hydrogen from 1-chlorobutane by the chlorine radical occurs in the first part of the propagation step. Depending on which hydrogen is abstracted by the chlorine radical, determines which product is formed. Hydrogens on the alkene have different reactivity which determines which isomer is favored.
| | | An Activity Series 1/9/13 Makieya DunhamPartners: Jasmine Lewis and Danielle Anderson | | | Problem Statement: In this lab we determined the activity series for five metals and for three halogens. In the first part of the lab we used a microscale technique to rank the metals that reacted with the other metal nitrates from most reactive to least reactive. The metal that reacts with another metal nitrate, then the solid metal have reduced the other metal ion and is the more reactive metal of the two. In the second part of the lab we used the solvent extraction technique to derive an activity series for the halogens. Safety Precautions: When in the lab we wore goggles, an apron, and gloves the entire time.
Empirical formula: CH5N Steps for molecular formula: 1- Calculate the molar mass of the empirical formula. 2- Divide the known (given) molar mass by the calculated empirical formula molar mass to get a whole number 3- Multiply that whole number through subscripts of the empirical formula to obtain the molecular formula. Example CH5N 12.01 g C x 1 C= 12.01 g/mol 1.008 g H x 5 H = 5.040
William Flores-Paz Monitoring Acid-Base Titrations with a pH meter October 30, 2013 Introduction The purpose of this experiment was to record the volume of HCl and acetic acid with a NaOH with a known molarity. This data would allow us to create a graph so we could compare the two titration curves. We would then use these curves to calculate the unknown molarities. HCl + NaOH >H2O + NaCl This equation shows the relationship between the acid and the base then the reaction goes forward and they are titrated creating salt and water. This particular reaction is a strong acid and a strong base which means that when the reaction reaches the equivalence point, the moles of the acid and the base are equal and the solution is neutral so the pH should be around 7.0 depending on the final volume of each solution.
Name: ___________________________________ Date: ______________ Practice Test #3 ____ 1. When a precipitation reaction occurs, the ions that do not form the precipitate A) evaporate B) are cations only C) form a second insoluble compound in the solution D) are left dissolved in the solution E) none of these 2. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)? A) B) C) D) E) ____ 3.
For example, if you mix aqueous solutions of AgNO3 and NaCl, there are two new combinations of ions possible. The silver nitrate solution contains Ag+(aq) and NO3-(aq). The sodium chloride contains Na+(aq) and Cl-(aq). Possible new combinations of these ions are AgCl and NaNO3. Note: these formulas would have been written in the upper right hand corner of each box before beginning the lab.