0.00512g ZnI2/mL of solution 0.00512g/319.18 g/mol=1.6*10-5 mol 1.6*10-5 mol/(1*10-3L)=0.016M c. 0.00806 moles of ZnI2/500 mL of solution 0.00806mol/(500*10-3)L=0.016M d. 0.0161 moles of ZnI2/L of solution 0.0161mol/1L=0.016M Exercise 4: a. The moles of ZnI2: 0.25M*(250*10-3)L=0.0625mol b. 0.25M*(250*10-3)L=0.0625mol The mass of ZnI2: 0.0625mol*319.18 g/mol=19.95g c. 0.25M*(500*10-3)L=0.125mol 0.125mol*319.18 g/mol=39.9g ZnI2 d. 0.0125mol/0.25M=0.05L Exercise 5: a. 0.125M*(100*10-3)L=0.0125mol b. 0.0625mol/0.125M=0.5L=500mL Calculation for preparing the EDTA solution Exercise 6 a.
Trang Nguyen Lab Report Chemistry 162: Reaction Kinetics Lab The purpose of this experiment: In this experiment, students aim to determine the rate law of the reaction by finding the time for each trial of different runs occurring. Upon studying initial reaction rates at varied reactant concentration, students will give out conclusion about the effect of the concentration towards the reaction rate. Next, the effect of the metal ion catalyst on the reaction rate will be studied by adding a dilute Cu(NO3)2 to the reaction. Finally, students will determine the effect of temperature on the reaction rate by carrying out the reaction at different hot and temperature, then calculate the activation energy. The procedure: Cabasco-Cebrian, T.; Loftus, C.; Schulz, J.; Villarba, M.; Wick, D. “Lab Manual for CHEM 162” Winter 2011, Department of Chemistry, Seattle Central Community College, pp.
Comparing the rate of appearance of C and the rate of disappearance of A, we get[pic]. A) [pic] B) [pic] C) [pic] D) [pic] E) [pic] Answer: A Diff: 1 Page Ref: Sec. 14.2 A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) →B(g). The following data are obtained for [A] as the reaction proceeds: [pic] 5) The average rate of disappearance of A between 10 s and 20 s is __________ mol/s. A) [pic] B) [pic] C) [pic] D) 454 E) [pic] Answer: A Diff: 1 Page Ref: Sec.
Chemical kinetics Date: 20th, Aug., 2010 Name: Huang Shiqi A0078026E Email address: firstname.lastname@example.org Class No. : Fr1 Lab partner: Jerome Lime A0073046L Abstract: The stated objectives of the experiment were to determine the reaction orders and rate constant of a chemical reaction, using the method of initial reaction rates and to determine the activation energy from the temperature dependence of the reaction rate based on Arrhenius’ theory. The chemical reaction used was iodide-persulfate reaction. Based on the equation: R = k [I-]n[ S2O82-]m and Arrhenius equation, the orders, rate constant (k) and activation energy can be calculated. The orders of the reaction were 2(n=m=1), k was 0.004174 L mol-1s-1 and the activation energy was 82.577kJ/mol.
So, qwater = qmetal Using the formula qmetal = m × c × ΔT, calculate the specific heat of the metal. Use the data from your experiment for the metal in your calculation. Part II: Calculate the energy change (q) of the surroundings (water) using the enthalpy equation qwater = m × c × ΔT. We can assume that the specific heat capacity of water is 4.18 J / (g × °C) and the density of water is 1.00 g/mL. Show ALL your work.
From these equilibrium concentrations, the equilibrium constant for the reaction can be determined. The purpose of this experiment is to determine the equilibrium constant for the following hydrolysis of an ester reaction: CH3COOCH2CH3 (aq) + H2O (l) CH3CH2OH (aq) + CH3COOH (aq) Ethyl Acetate Water Ethanol Acetic Acid (EtAc) (EtOH) (HAc) The equilibrium constant, Kc, for the reaction will have the following expression: Several reaction mixtures will be prepared with different initial amounts of ethyl
How do you go from calculated/measured values to accomplishing stated purpose? (4 pts) The purpose of this lab is to determine the exact concentration of an unknown acetic acid solution. Titrations for two different reactions will be performed. Controlled volumes of one reagent are added to a flask containing the other reagent until the equivalence point of the reaction is reached, one between sodium hydroxide (NaOH) and potassium hydrogen phthalate (KHP) and the other between NaOH and acetic acid (CH3COOH). NaOH (aq) + KHP (aq) —› Na+ (aq) + K + (aq) + P2- (aq) + H2O (l) NaOH (aq) + CH3COOH (aq) —› Na+ (aq) + CH3COO- (aq) + H2O (l) The titration of NaOH with KHP will identify the concentration of the NaOH provided.
Reaction of Iron Filings with an Aqueous Solution of Copper (II) Sulfate Purpose: There were many reasons that we conducted this reaction as a lab. The main objective of the lab was to observe a reaction of Iron and Copper (II) Sulfate. This lab presented a good opportunity to work with numbers using moles and Stoichiometry. This lab was also good for practice using Bunsen burners, glass, and handling hot objects. Lastly, we got to witness and test the Law of Conservation of Mass through the reaction in this experiment.
Computer Additivity of Heats of Reaction: Hess’s Law 18 (1) Solid sodium hydroxide dissolves in water to form an aqueous solution of ions. (2) Solid sodium hydroxide reacts with aqueous hydrochloric acid to form water and an aqueous solution of sodium chloride. NaOH(s) + H+(aq) ) + Cl–(aq) → H2O(l) + Na+(aq) + Cl–(aq) ∆H2 = ? OBJECTIVES • • • • In this experiment, you will Combine equations for two reactions to obtain the equation for a third reaction. Use a calorimeter to measure the temperature change in each of three reactions.
EXTRACTION: DETERMINATION OF ITS EFFICIENCY AND CALCULATION OF THE DISTRIBUTION COEFFICIENT Group#4: Wassim Abdel Naby and Bianca Francisco Bachelor of Science degree in Chemistry De La Salle University ABSTRACT The objective of this experiment is to demonstrate the concepts of extraction and to calculate the distribution coefficient. In the process of extraction, amount of acetic acid was the one to be determined, and this was done through the process of titration, indicator used was phenolphthalein and the titrant used was Sodium hydroxide. First, 20 ml aliquot portion of diluted acetic acid in a 125 mL Erlenmeyer flask titrated with Sodium hydroxide. Next, the second flask containing another 20 mL of acetic acid extracted by 20 mL portion toluene, this was done twice due to over titration in the first trial. Lastly, the third 20 mL aliquot portion acetic acid underwent the same procedures with flask 2 but this time with two 10 mL portions of toluene.