CHEM 1040 Lecture Notes - Lecture 13: Gibbs Free Energy, Intermolecular Force, Arrhenius Equation

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erinsalmon14

11 Dec 2016

School

University of Guelph

Department

Chemistry

Course

CHEM 1040

Professor

Abdelaziz(aziz) Houmam

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Document Summary

Chemical reactions require different lengths of time for completion. How reaction rates change under varying conditions. What molecular events occur during the overall reaction. However in some reactions, rate is unaffected. Catalyst (a substance that increases the reaction rate without being consumed) Does not disappear in the balanced equation. Reaction usually speeds up when the temp increases. Surface area of a solid reactant or catalyst. The amount of product formed / reactant used up per unit time. The increase in molar concentration of product of a reaction or the decrease in molar concentration of reactant per unit time. *rate calculation does not depend on the total quantity of reaction mixture used e. g 2n2o5(g) 4no2(g) + o2(g) rate can be found by: 1). [o2] / t (if time interval is long, this equation gives the average rate) (if time interval is short, this equation gives the instantaneous rate)

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Need help with 5. âCalculate molar concentrations of KIO3 and NA2SO3 for solutions A-Gâ on page 113 please!! Solution #1 (KIO3) and solution #2 (Na2SO3) were both diluted with distilled water to 50mL and mixed together to form solution.....density of KIO3=4.28g/L and Na2SO4=1.01g/L. Thank you!!

For a reaction aA rightarrow Products, [A]_o = 13 M, and the first two half-lives are 35 and 70 minutes, respectively, a) Write the rate law for this reaction. b) Calculate k. c) Calculate [A] at t = 335 minutes The Model of Chemical Kinetics represents the reaction rate constant as: k = (2p) times exp(-Ea/RT). What does each variable in the equation mean- that is, in regard to their contribution towards the reaction rate constant? In other words, what does each variable actually mean/refer to? Chemists commonly use a rule of thumb that an increase of 10 K in temperature doubles the rate of a reaction. What must the activation energy be for this statement to be true for a temperature increase from 63 degree C to 73 degree C? ln(k_2/k_1) = E_a/R(1/T_1 - 1/T_2) (i) What is a catalyst? (ii) What are the two types of catalysts? Explain specifically why they are different? (iii) What is one example of each type of catalyst? (i) What does it mean when a reaction is in chemical equilibrium? Specifically, within the context of reactants? products, and the forward and reverse reaction rates, what does chemical equilibrium mean? (ii) What is Le Chateleir's Principle? Within the context of reactant/product concentration, temperature, and pressure, how does Le Chatelier's Principle predict a reaction will respond to variations in reactant, product concentration, temperature, and pressure. (i) For the given reactions: N_2(g) + 3H_2(g) harr 2NH_3(g), H_2O(g) + CO(g) harr H_2(g) + CO_2(g), HCN(aq) harr H^+(aq) + CN^-(aq), 2KClO3(s) harr 2KCl(s) + 3O_2(g) and 2H_2 O(l) harr 2H_2(g) + O_2(g). Write the equation that governs each of their equilibrium rate constant K (ii) If N_2(g) + 3H_2(g) harr 2NH_3(g)'s (at 25 degree C) has K = 25, what would K be (at 25 degree C) for 2NH_3(g) harr N_2(g) + 3H_2(g)? (iii) What would K be if [5 times (N_2(g)+3H_2(g) harr 2NH_3(g)]? (i) For N_2(g) + 3H_2(g) harr 2NH_3(g): P_NH3: 1.9 times 10^-1 atm, P_N2 = 8.9 times 10^-2 atm, P_H2 = 1.9 times 10^-2 atm, what is K_p? (ii) Using K_p, calculated in the previous step, what is K at 45 degree C, where K_p = K(RT)^Delta n? (R = 0.08206 L atm/mol K). What is the difference between homogeneous and heterogeneous? (ii) If K is larger than 1, does the equilibrium life farther to the right (favoring the production of products) or to the left (favoring reactant formation)? (iii) If K is less than 1, does the equilibrium life farther to the right (favoring the production of products) or to the left (favoring the production of reactants)?

Hi, I have a lab and have provided the information below and the data calculated at the end. Please help in prelab questions and postlab questions. WIll rate really good if it's correct. Thanks a lot.

DATA (The total liquid should be 50ml, not more than that)

SNO.	NACLO (intial temperature)	THE (B) Liquid temperature	NaClo(g)	The B solution(g)	FINAL temperature(together)
1	21.7	21.5	10ml	40ml	30.4
2	none	21.5	0ml	50ml	21.5
3	21.8	none	50ml	0ml	21.8
4	21.9	21.7	20ml	30ml	38.4
5	21.9	21.7	30ml	20ml	37.4
6	22.0	21.7	40ml	10ml	28.8
7	22.1	21.9	25ml	25ml	42.2

Mole ratio lab v3b Rukes APChemistry Determination of the mole ratio of a chemical reaction The method of continuous variations is a means of determining the stoichiometric mole ratio of the reactants in a chemical reaction. The stoichiometric ratio, as given by the coelficients in the balanced chemical equation, represents the ratio at which chemicals must be combined to produce al product with no excess rcactant. Sincc there is no âwasted" reactant, the maximum amount of product is made for the given amount of both reactants. In themethod of continuous variations, several trials are performed. In each trial, there is a fixed amount of total reactant (measured by moles or volume or mass, etc.), but with the two reactants mixed together in different ratios. Some measure of the amount of product is made for each trial (volumc of gas produccd, mass of precipitate, color of product solution, etc.). When the amount of product is maximized, the stoichiometric ratio has been used. A similar technique fixes the amount of one reactant and increases the other until the maximum amount of product is reached In this lab the two chemicals being mixed are solutions of known molarity. The total volume of solutions is kept constant over several trials. The chemicals will release heat when mixed together and raise the temperature of the mixture. Since the volume of the solutions mixed is held constant, the temperaturc changc recorded wl be proportional to the amount of heat produced and therefore also the "anount of reaction" that occurred. Objectives - To graphically determine the stoichiometric mole ratio of a reaction. CAUTIONS: All solutions are basic and can be harmful to skin and eyes. Sodium hypochlorite can also bleaclh clothing. Wear goggles, gloves and aprons. ï¸µ Pre-lab: complete on a separate sheet. 1. Accurately graph the following data gathered from an experiment which mixes 0.5 M solutions of AgNO3 and K2CrO4. The x-axis should plot the volume of AgNO3 reading Irom lef to right (or the volume of K2CrO4 reading from right to left.) Draw two best fit lincs, one for the "up" slope and one for the "down" slope... see example to the right of the data. (Also consult your graphing skills handout if you have not yet drawn a graph) trial mL AgNO3 mL K2CrO mass of precipitate (g) 45 35 25 20 15 10 shape of graph 15 25 30 35 40 45 5.0 4 10.0 9.9 6.6 3.3 a) Use the intersection of best fit lines to find the theoretical maximum amount of product. b) Use the x-values to find the stoichiometric volume ratio c) Use the answer from b) and given molarities to find the stoichiornetric mole ratio d) How many values were used to plot your "up" line? How many values were used to plot your "down" line? 2. What single temperature change should be recorded if 10 mL of solution A at 20Â°C is mixed with 10 mL of 3. What single temperature change should be recorded if 10 mL of solution A at 20Â°C is mixed with 30 mL of 4. List four dependent variables that are often used for the method of continuous variations. Are these enough values to plot a good line? solution B at 24.0Â°C and the final temperature reaches 28.0Â°C? solution B at 24.0Â°C and the final temperature reaches 28.0Â°C?

CHEM 1040 Lecture Notes - Lecture 13: Gibbs Free Energy, Intermolecular Force, Arrhenius Equation

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