In a solution of FeSO4, solution of .02 KMnO4 was added until the combination of the solution turned pink. The change of the color pink indicates that the reaction is complete. The process that was undergone with FeSO4 and KMnO4 is called titration. In chemistry, titration is a procedure used to determine the molarity of two or more solutions. Molarity is the number of moles in a compound in a solution over the number of liter in the solution.
[2] to determine the Activation Energy. This equation is simply the equation of a line (y = mx + c) and from the graph the Activation Energy can easily be calculated. Procedure: As per lab manual. [3] Calculations: 0.4977 M sodium thiosulphate 1.01ml rough 1.04ml final volume of Na2S2O3 0.4977 mole/L -> 0.004977mol/ml x 1.04ml = 5.176 x 10-4 moles =
* A large value of Keq indicated that the equilibrium mixture contants more products than reactants. * A small value for the equilibrium constant means that the equilibrium lies toward the reactant side. * The equilibrium constant expression and the equilibrium constant of the reverse of a reaction are the reciprocals of those of the forward reaction. Section 3 * Equilibria for which all substances in the same phase are called homogeneous equilibria. * In heterogeneous equilibria two or more phases are present.
Acid and Base Titration Aim: To determine the concentration of a dilute solution of sodium hydroxide which is approximately 0.1 mol dm-3 Introduction: Titration is an example of redox reaction and is a process of chemical analysis in which the quantity of some constituent of a sample is determined by adding to the measured sample an exactly known quantity of another substance with which the desired constituent reacts in a definite, known proportion. The process involves the gradual adding of standard solution of titrating reagent from a burette. The addition is stopped when the equivalence point is reached. From this point an exact equivalent of titrant will be added to the earlier solution. The completion of the reaction is marked by some signal; this signifies the end point.
Calculate the yield? m(ester)=8.64 g M(ester)=88.048 〖gmol〗^(-1) n=8.64/88.048≈0.098 mol Since the ratio between the limiting reactant and ester is 1:1 they have the same amount. So these are the theoretical calculations. n(ester)=0.1628 mol M(ester)=88.048 〖gmol〗^(-1) m=0.1628×88.048=14.33 percentage yeild=(experimental yeild)/(theoretical yeild)×100=8.64/14.33×100≈60.3% The reaction is at equilibrium with Kc approximately 4. What substances do we have in the rb flask when heating is turned off?
Molecules at higher temperature have more thermal energy. Introduction Chemical Kinetics, also known as reaction kinetics, is the study of rates of chemical processes. Chemical kinetics includes investigations of how different experimental conditions can influence the speed of a chemical reaction and yield information about the reaction’s mechanism and transition states, as well as the construction of mathematical models that can describe the characteristics of a chemical reaction (Clarke, 1974). Chemical kinetics deals with the experimental determination of the reaction rates from which rate laws and rate constants are derived. Relatively simple rate laws exist for zero-order reactions (for which concentration rates are independent of concentration), first-order reactions and secondorder reactions, and can be derived for others.
One of the applications of Hess' Law is to determine the enthalpy change for a reaction by combining other reactions to get the desired reaction, then combining the enthalpy changes for the reactions to get delta H for the reaction under consideration. An exothermic enthalpy change is always Assessed Practical: Planning Introduction: The aim of this experiment is to find the enthalpy change for the decomposition of sodium hydrogen carbonate. 2NaHCO = Na2CO3 + CO2 + H2O Using the enthalpy change of the following reactions. Sodium Hydrogen Carbonate: NaHCO3 + HCl = NaCl + CO2 + H2O Sodium carbonate: Na2CO3 + 2HCl = 2NaCl + CO2 + H2O Apparatus Sodium hydrogen carbonate Sodium carbonate Polystyrene Cup x 2 Measuring cylinder 50cm³ x 2 Weighing scale Weighing boats Thermometer degrees Spatula HCl acid 2M Prediction Background Information Hess' Law states that the enthalpy change for a reaction is the same whether the reaction occurs directly or in steps. This is a direct consequence of the fact that enthalpy, is a state function.
For instance, the neutralization of HCl by NaOH is written as: HCI + NaOH -----------> NaCl + HOH Equations for neutralization reaction are balanced so that the amount of H+ will be equal to the amount of OH-. The addition of a specific amount of base required to neutralize an acid in a sample involves a titration. An indicator in a sample will change color when all the H+ from an acid has been neutralized. The addition of a base should be stopped when the indicator changes color which therefore determines the endpoint. At this point the volume of base used to neutralized the acid can be determined.
Which way will the following equilibrium shift if the total pressure on the system is decreased? 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(g) Answer________________ 4. Hydrogen peroxide is decomposed as follows: H2O2(l) → H2(g) + O2(g) H = +187 kJ Predict the direction of equilibrium shift by each of the following imposed changes: a) Increase the [H2] ........................................Answer ______________________ b) Decrease the [O2] .......................................Answer ______________________ c) Decrease the total pressure ........................Answer ______________________ d) Increase the temperature............................Answer ______________________ e) Add MnO2 as a catalyst.............................. Answer ______________________ 5. Consider the following reaction at equilibrium: H2(g) + I2(g) → 2HI(g) a) Addition of more H2 gas to the container will do what to the rate of the forward reaction? Answer ________________________ b) If, for a while, the rate of the forward reaction is greater than the rate of the reverse
The data collected supports the original hypothesis. As vapor pressure went up, so did the temperature. One can also infer that increasing the temperature and thus, kinetic energy, increases the vapor pressure and the rate at which random interactions occur. Using this information, one would predict that raising the temperature in a bottle of soda causes the vapor pressure to increase and more molecules to escape faster, leading the soda to go “flat” at a much faster rate. Based on the results, methanol and ethanol exhibit different kinds of intermolecular forces and different vapor pressures.