Le Chatelier’s Principle can be used to predict how a change in condition affects a chemical equilibrium.
Essay Topic: (Virtual Lab report) Life at high altitudes and haemoglobin production. More details about tasks is attached in document below: Length: 750 words (calculations are not included in the word limit) Topic: Virtual Lab Report requirements: - A minimum of 5 references. These can include journals, books, reput
I have a problem understanding the degrees of freedom for two binary diagrams because they have different degrees of freedoms in some parts of the diagram and I don't get why they have that. It would be great if you could explain if this is because of less chemical potential equilibrium or from less variables from the derivation
Given the following reaction: C0(g) + H2O(g) <> C02(g) + H2(g) (Please see the attachment for the properly formatted reaction). a) Write the equilibrium constant expression for this reaction. Note: gaseous-phase H20 is included in the equilibrium expressions, unlike liquid phase H20. b) The equilibrium constant for the reactio
Question #1 The gas reaction N2(g) + 3H2(g) <--> 2NH3 (g) has K- = 0.80 at 600 K and Kp = 0.15 at 650 K a) Is delta H greater than or less than zero? b) Is the reaction exothermic or endothermic? Question #2 The reaction N2 (g) + 3H2 (g) <---> 2HN3 (g) is at equlibrium a) The number of moles N2 present plus he numb
The standard free energies of formation of SO2(g) and SO3(g) are -300.4 and -370.4kJ mol-1, respectively. Calculate the value of the equilibrium constant at 25'C for the reaction 2SO2(g) + O2(g) <=======> 2SO3(g)
For the chemical system shown below, it was found that [N2] = [O2] = 0.70 mol/L and [NO] = 0.22 mol/L, at equilibrium. Suppose that enough N2 was added to increase its concentration temporarily to 1.00 mol/L. When the system reaches equilibrium, what will be the new equilibrium concentrations of N2, O2, and NO? N2(g) + O2(g) ?
1) Why is a mixture of ice and water, rather than ice alone, used in calibrating a thermometer? 2) Why does the boiling point of a liquid vary with the barometric pressure? 3) What does it mean to say that the normal boiling point of a pure liquid substance is a characteristic property of the liquid substance?
I have attached a problem I am not really sure how to approach. I would appreciate a complete explanation and work. ** Please see the attached file for the complete problem description **
Will 0.060 M in Pb(NO3) mixed with 0.020 M in NaBr form a precipitate? (Explain)
For the reaction: Kc = 255 at 1000k CO (g) +Cl2 (g) == COCI2 (g) If a reaction mixture initially contains a CO concentrations of 0.1500 M and a Cl2 concentration of 0.175 M at 1000 k, what are the equllibrium concentrations of CO, Cl2, and COCl2 at 1000 K?
General Chemistry Multiple Choice Questions with Answers and Explanations: Molarity, Acids, Bases, Equilibrium.
The minimum combined kinetic energy reactant particles must possess in order for their collision to result in a reaction is called the Answer A. collision energy. B. orientation energy. C. activation energy. D. dissociation energy. Question 2 The defini
1. What are the advantages and disadvantages of using ether as an extraction solvent? 2. Why must the stopper at the top of the separatory funnel be removed before liquid can be withdrawn through the stopcock? The detailed description of the above mentioned problem is described in the attached file.
Lead(II) carbonate is very insoluble in water, meaning that the equilibrium constant for the dissociation reaction is much less than 1: PbCO_3 (s) <-> Pb(2+) (aq) + CO_3(2-) (aq) Write reactions for each of the following and explain how the equilibrium reaction for the dissociation of lead(II) carbonate is affected. a.
What are the equilibrium constant expressions for the following? a) PCl 5 (g) <=> PCl 3 (g) + CI 2 (g) b) Cu (OH) 2 (s) <=> Cu 2+(aq) + 20H- (aq) c) [Cu (NH3)4]2+(aq) <=> Cu 2+(aq) + 4NH3 (aq) d) CH3 CH2 CH2COOH (aq) + H2O (l) <=> CH3 CH2 CH2COO- (aq) + H3O+(aq)
When an aqueous solution of an organic compound is shaken with an immiscible organic solvent, such as diethyl ether, the solute distributes itself between the two phases. When the two phases separate into two distinct layers, an equilibrium will have been established such that the ratio of the concentrations of the solute in eac
For the equilibrium: PCl5(g) PCl3(g) + Cl2(g) Kc = 4.0 at 228°C. Pure PCl5 is added to the reaction system. At equilibrium there is 0.16 M PCl5. What is the concentration of PCl3 in this system? Answer = .80M But what are the steps to get this answer?
Ketones also undergo the aldol condensation although a successful reaction often requires "enhanced" conditions, as the addition involves an unfavorable equilibrium constant. This is the situation in the reaction in which 4-nitrochalcone is synthesized. With the odds against it, why is the reaction successful in this case?
I need help with the following problem with steps included: Consider the following reaction: N2(g) + O2(g)ï? 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.15 atm, 0.33 atm, abd 0.50 atm, respectively, at 2200oC what is Kp? I have also attached the problem if you need to see the correct form
Water must be excluded from the reaction that generates 4-hydroxycoumarol. In the first step of this reaciton, formation of 4-hydroxycoumarin, what is the purpose of removing the ethanol generated in the reaction?
A stoppered flask at 25 C contains 250 mL water, 200 mL octanol, and 50 mL of air. An unknown mass of o-xylene is added to the flask and allowed to partition among the phases. After equilibrium has been established, 5.0 mg of o-xylene are measured in the water. What is the total mass (g) of o-xylene present in the flask?
At 1130oC the equilibrium constant (Kc)for the reaction: 2H2S(g) <----->2H2(g) + S2(g) Is 2.25 X10-4, if [H2S]=4.84 X10-3 M and [H2]=1.50X10-3 M, calculate [S2]. ( need help with the following problem with the steps)
Questions: 1.) Show what compounds result from hydrolysis of the following compound. 2.) Draw the major product of the following reaction (after aqueous workup). Please see the attachment for the visual components. Thanks for all of your help!
Find the value of Ke for the reaction, A(g) + 2B (g) ---> 2C(g) + D(g) In which it was found that at equilibrium, [A] = 0.200 mol/L, [B] = 0.200 mol/L, [C] = 0.0500 mol/L, and [D] = 0.0750 mol/L.
The Kb for methylamine, CH3NH2, is 4.4 x 10-4 at 25°C a) write a chemical equation for the equilibrium that corresponds to Kb b) by using the value of Kb, calculate ΔG° for the equilibrium in part (a) c) what is the value ΔG at equilibrium ? d) What is the value of ΔGwhen [H+] = 1.5 x 10-8 M, [CH3NH3+] = 5.5 x 10-4 M, a
Can you show me how to do this one? Thank you at 1600°C. Br2(g) = 2 Br(g) When 1.05 moles of Br2 are put in a 0.980 L flask, 1.20 percent of the Br2 undergoes dissociation. Calculate the equilibrium constant Kc for the reaction.
Do I just plug in the numbers to get the answer? Do I convert the temp to Kelvin? N2(g) + O2(g) = 2 NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.15 atm, 0.33 atm, and 0.050 atm, respectively, at 2200°C, what is KP?
Just when I thought I was catching on.... then I missed this question by more than a factor of 10.....Help! For the reaction given below at 700°C, Kc = 0.534. H2(g) + CO2(g) = H2O(g) + CO(g) Calculate the number of moles of H2 that are present at equilibrium if a mixture of 0.297 moles of CO and 0.297 moles of H2O is
2CO(g)+O2(g)=2CO2(g) If Kc is 2.24 e22 at 1273 degrees C what is Kp I know it must seem silly, but I still can't figure out how to set it up. Can you show me again?
The equilibrium constant (Kc) for the reaction shown below is 4.17x 10-34 at 25°C. 2 HCl(g) = H2(g) + Cl2(g) What is the equilibrium constant for the following reaction at the same temperature? H2(g) + Cl2(g) = 2 HCl(g) Why isn't it the same Kc? Is it the inverse?
This is one of the ones that I didn't get right. Can you show me how to do it? H2(g) + Br2(g) = 2 HBr(g) Begining with 2.50 moles at 730 degrees C in a 12.o liter vessel, if the Kc is 2.18 e6 ............what are the concretration of H2, Br2 and HBr at equilibrium