General Chemistry Ii - Midterm 1 Answ Essay example

The initial concentrations of the reactants in Table 1—that is, [Fe3+] and [SCN–] prior to any reaction—can be found by a dilution calculation based on the values from Table 2 found in the procedure. Once the reaction reaches equilibrium, we assume that the reaction has shifted forward by an amount, x. Notice from Table 1 that the value of x is simply equal to the equilibrium concentration of FeSCN2+(aq), or that x = [FeSCN2+] at equilibrium. The equilibrium value of [FeSCN2+] is determined spectroscopically using Beer’s Law. Its initial value in the table is zero because no FeSCN2+(aq) is added to the initial solution. Finally, the equilibrium concentrations of the reactants, Fe3+(aq) and SCN–(aq), are found by subtracting the equilibrium concentration of FeSCN2+(aq) from the initial concentrations of Fe3+(aq) and SCN–(aq), as shown in the table above. Once all the equilibrium values are

There are three stages of the overall reaction. Reaction 1 is the rate determining reaction whereby iodide ions from Potassium Iodide (KI) are oxidised by Hydrogen Peroxide (H₂O₂) in an acidic solution. This reaction utilises the Hydrogen ion from Sulfuric acid (H₂SO₄) to form triiodide ions and water as products (B Z. Shackhashiri, 1992).

The rate of a chemical reaction often depends on reactant concentrations, temperature, and if there’s presence of a catalyst. The rate of reaction for this experiment can be determined by analyzing the amount of iodine (I2) formed. Two chemical reactions are useful to determining

9. Discared the solutions. The next step is to analyze the data graphically to see if the reaction is zero, 1st or 2nd order with respect to crystal violet. The reaction is

Is this a linear relationship? What happens to the initial reaction rate as substrate concentration increases?

2. SN1 and E1 reactions both involved the initial formation of a carbocation intermediate. In this experiment, why is the SN1 product favoured over the E1 product?

ii) does not evaporate or react upon heating.The moles ratio will decrease because since all the

(b) Calculate the initial rate of absorption ofC12H26Sfrom a 1 mM solution at 20 °C ifits initial sticking coefficient is 1×10–6.6.A gas phase reaction between atomA and a diatomic molecule BC has a positive activationenergy to reach a collinear transition state. Describe how the reaction to form AB occurs.Suggest a plausible explanation for why the product AC is not formed.7.Calculate thecollision rateof waterwith a surface ifthe surfaceis exposed to (a) water vaporwith a pressure of 1 atm and (b) liquid water?The system is held at 350 K.8.The forward and reverse rate constants have been measured for the gas-phase reactionH2(g) +I2(g)2HI(g).The reaction is bimolecular in both directions with Arrhenius parametersA=4.45×105dm3mol–1s–1,Ea=170.3kJ mol–1(forward reaction)A'=5.79×101dm3mol–1s–1,Ea' =117.6kJ mol–1(reverse reaction)Computek,k' (rate constant for the reverse reaction),K,ΔrG°,ΔrH°, andΔrS° at

This is the rate limiting step as it is dependent only upon the concentration of alkyl halide and not the concentration of the base2. Thus, a strong base is not required in this type of reaction as the leaving group is not removed (Master Organic Chemistry, 2017). Also, there is no need of stereochemistry, but there is a barrier that needs to be crossed (Master Organic Chemistry, 2017). For an E2 reaction, it is characterized as being bimolecular, because the rate it proceeds at is proportional to the concentration of both the alkyl halide and base added to make the product2.

How does the arrangement of particles in a gas differ from the arrangements in liquids and solids? -Gas particles are very widely separated from each other. 6. Which requires the

Cl] + [–6] = 0 O.N. of Cl = 6 – 1 = +5 Q. 12: Find the oxidation no nitrogen in HNO3 if oxidation no of hydrogen and oxygen is +1 and -2. Ans: Sum of all oxidation number is zero. [O.N of H] + [O.N of N]+3[O.N of

E.g. 3L Hydrogen(gas)+1L Nitrogen(gas) = 2L Ammonia(gas) (Simple Ratios) • “Recount Avogadro’s law and describe its importance in developing the mole concept”

The experiment was interesting to say the least. There were errors involved and the calculations don’t seem 100% correct. Activation energy should have units of Joules only but when calculated the activation energy, it had units of Joules per moles times seconds. There was probably and error in the calculations or possibly just missing a step. There were also errors when recording time as the lab manual was not followed correctly. Assuming that all experiments that took place were 1st order reactions doesn’t seem correct. R2 was higher compared to the 0th order but only barely and I was unable to determine which was the correct order of the reaction. The results seem to make sense in terms of activation energy. As temperature is being increased

2) Calculate the a mean rate constant using orders of reactions and the rate equation allowing for the overall order or reaction to be found.

Kinetics of chemical reactions is how fast a reaction occurs and determining how the presence of reactants affects reaction rates. In this experiment the rate of reaction for Fe+3 and I- is determined. Because the rate of chemical reactions relates directly to concentration of reactants, the rate law is used to find the rate constant, and calculated with specified temperatures.