Explore BrainMass
Share

# Chemical Equilibrium

### Equilibrium Concentration of Gas: Example Problem

The equilibrium constant for Kc for the reaction shown is 54.3 at 430 degrees C. H2(g) + I2(g) --> 2 HI(g) At the start if the reaction there are 0.714 moles of H2, 0.984 mole of I2 and 0.886 mole of HI in a 2.00 liter reaction chamber. At equilibrium, what are the concentrations of the gases-

### Nitric oxide air polution

The equilibrium constant (Kp) for the formation of the air pollutant nitric oxide (NO) in an automobile engine at 530 degree C is 2.9 x 10 to the minus eleventh N2(g) + O2 (g) = 2 NO (g) What is the partial pressure of NO under these conditions if the partial pressures of nitrogen and oxygen are 3

### Equilibrium Constant for the Decomposition of Compounds

1. What is the equilibrium constant for the decomposition of NO: 2NO ---> N2 + O2 at room temperature? For NO: DHf° = 90.25kJ/mol and DGf° = 86.57kJ/mol 2. Using the data in problem 1, find the temperature, if any, at which the equilibrium constant for the decomposition of NO would be 1.

### Equilibrium Concentration for BaSO4

The Ksp for BaCO3 is 5.1 x 10-9, while that for BaSO4 is 1.1 x 10-10. What would be the equilibrium concentrations of CO3-2 and SO4-2, if solid BaSO4 were placed in a 0.01M CO3-2 solution?

### Calculating PH Concentration

The formation constant for zinc tetraammine ion [ Zn(NH3)4+2] is 4.1 x 108. What is the concentration of free Zn+2 in a solution of 3M NH3 (total ammonia) buffered to a pH of 9.0 if the total zinc concentration is 0.1M? The Kb for NH3 is 1.8 x 10-5

### Calculating the concentration of ion at equilibrium

Please help with the following problem. Provide step by step calculations. Consider a solution that is 0.10 M in a weak triprotic acid that is represented by the general formula H3A with the following ionization constants: For H3A: Ka1= 1.0 x 10 ^-3 Ka2= 1.0 x 10 ^-8 Ka3= 1.0 x 10 ^-12 What is the concentration of

### For the water-gas reaction (Problem 43 attached) Kc = 0.111

For the water-gas reaction (Problem 43 attached) Kc = 0.111 at about 1100 K. If 0.100 mol H2) (g) and .100 mol H2 (g) are mixed with excess C(s) at this temperature and equilibrium is established, how many moles of CO (g) will be present? No CO (g) is present initially.

### Isomers of D-glucose

4. Start with an open-chain model of glucose then form the hemi-acetal using the carbon #5 -OH and the carbonyl at carbon 1 then reverse the process and remake the open-chain form. 5. Reclose the ring making sure that you come up with a different product. a. Did you build the alpha or beta anomer? b. Based on your models,

### In a sealed 10.5-L vessel at 184C, equilibrium is established

In a sealed 10.5-L vessel at 184C, equilibrium is established... Ammonium carbamate See attached file for full problem description.

### Chemical Equilibrium

1. Define dynamic equilibrium state in terms of a) reaction rates b) change in observable properties c) energy and entropy state 2. In which of these closed containers is the vapour pressure the greatest? Explain the choice. a) a 1 L container with 5 mL of water held at 20&#730;C b) a 1 L container with 15 mL of water

### Calcium sulfate is sometimes added to wine both to clarity and to percipitate dissolved lead. Given the following Ksp values, what [Pb^2+] remains in wine that is saturated with CaSO4? (Ksp CaSO4=9.1*10^-6, Ksp PbSO4= 1.6*10^-8)

Calcium sulfate is sometimes added to wine both to clarity and to percipitate dissolved lead. Given the following Ksp values, what [Pb^2+] remains in wine that is saturated with CaSO4? (Ksp CaSO4=9.1*10^-6, Ksp PbSO4= 1.6*10^-8)

### Tautomerism and non-bonding electrons

The following tautomerism has been observed. Add any non-bonding electrons. Use arrows to push electrons and show how the structure on the left can be transformed to the structure on the right. Which side of the equilibrium is favored? Why? (see diagram in attached file) ---

### Titration of Borax with HCl

1. Would the experimental values of Ksp, (see attachment for formatting); be affected if the samples titrated contained large amounts of solid borax? If so, would the experimental values be falsely high or falsely low? Explain 2. Does the equilibrium constant change as the temperature changes? If so, explain why the equi

### Ksp & Molar Solubility - Ionic Equilibria

1. The solubility of silver dichromate at 15C is 8.3 x 10-3 g/100mL solution. Calculate its Ksp. 2. Calculate the molar solubility of Ca(IO3) 2 in 0.060 M NaIO3.

### Equilibrium, Basic, Acidic, and Neutral Salts

1. Complete the following equilibrium with the most likely products: NaSH + NH3 <===> 2. Label each of the salts as basic, acidic, or neutral: NaF KOAc KBr NaH2PO4 NH4OCl Pb(NO3)2.

### Calculate Eqiulibrium Constant

Calculate the value of the equilibrium constant for each of the following reactions ( we abbreviate citric acid as H3Cit) using the Ka values for citric acid and for carbonic acid: H3Cit + HCO3- <--> H2Cit- + H2O +CO2 H3Cit + 3HCO3- <--> Cit3- + 3H2O +3CO2 Given Ka1 of H3Cit =8.4x10-4; Ka2 of H3Cit = 1.8x10-5; Ka3 of H3Ci

### Equilibrium

I am enclosing a problem is causing me some doubt. As you will read from the problem wording, It seems that the value should be 0.3 mole as well. However, it is not within the options. (See attached file for full problem description) --- When 2.0 mol of carbon disulfide and 4.0 mol of chlorine are placed in a 1.0 Liter fl

### Equilibrium Constant in Half-Reactions

What is the Ecell and the equilibrium constant, Kc, for the cell represented by the combination of the following half-reactions? 2 Hg2+(aq) + 2e- equilibrium Hg2 2+(aq) E= 0.92V Cr3+(aq) + 3e- equilibrium Cr(s) E= -0.74 V

### The hemoglobin molecule carries oxygen in the blood

Please help answer the following problems. Include references in the solution. The hemoglobin molecule carries O2 in the blood from the lungs to the cells, where the O2 is released for metabolic processes. The molecule can be represented as Hb in its unoxygenated form and as Hb.O2 in its oxygented form. One reason CO is to

### Equilibrium Concentration Functions

3. A complex ion forms between Ag+ and CN- to give [Ag(CN)2]- with a formation constant of 1.3 x 10 to the 21. To a 0.5 M aqueous solution of silver nitrate you and sufficient HCN to make it 2 M. The Ka for HCN is 6.03 x 10 negative 10. What are the equilibrium concentrations of Ag+, [Ag(CN)2]-2, H+, and HCN?

### Pressure's Effect on Equilibrium

When hydrogen gas reacts with Iodine as a gas, Hydrogen Iodine is produced in its gaseous form. The equilibrium concetrations for both reactants were found to be 0.86 M and the product was found to be 0.27. Calculate the value of the equilibrium constant. How would pressure effect the equilibrium of this reaction?

### Chemistry Calculations and Concepts

Determination of the Molar Mass and Ionization Constant of a Weak Monoprotic Acid Acetic Acid + Water yields Conjugate Base + Hydronium Ion Or HA + H20; H30+ + A- Calculation of the ionization constant for acetic acid from the measured pH of acetic acid samples: Acetic Acid titrated with Sodium Hydroxide and the followin

### Gas Reaction Explanation

Step by Step Explanation Ethylene, C2H4, will react with hydrogen gas under appropriate conditions to form ethane, C2H6. A 10.0-liter vessel is charged with 1.5 atm of hydrogen and 1.0 atm of ethylene at 25°C. The reaction is allowed to proceed to completion. Determine the total pressure in the vessel at 25° at the completi

### Calculating Values of Equilibrium Constants

Question states: In the reaction of ammonium chloride (as a solid) dissociating to produce ammonia and hydrogen chloride (both as gases), the equilibrium concentration of each product was found to be 3.71x10^-3 (they each have the same concentration, ammonia is 3.71x10^-3 and hydrogen chloride is 3.71x10^-3). Calculate the v

### Chemistry Equilibria Example Problem

Of the following equilibria, only _______ will shift to the left in response to a decrease in volume. a. H2 (g) + CL 2 (g) <-> HCL (g) b. 2SO3 (g) <-> 2SO2 (g) + O2(g) c. Ns (g) = 3H2 (g) <-> 2NH3 (g) d. 4Fe (s) = 3O2 (g) <-> 2Fe2O3 (s) e. 2HI (g) <-> H3(g) + I3 (g)

### Equilibrium & Buffers

1. You have a 0.087565 M solution of a weak acid, HA, pH=4.18177. How many grams of NaA (molar mass = 62.476 g/mol) would you have to add to this solution (assume that there is no change in volume) to have a solution with a pH of 7.40000. Would this new solution be a good buffer? Please explain. 2. You have a mixture of

### Reaction Kinetics - Equilibrium

A.) Consider the reaction: 4HCl (aq) + MnO2 (s) <--> Cl2 (g) + 2 H2O (l) + MnCl2 (aq) Delta (H)degree The equilibrium is displaced to the left if: a. Catalyst is added b. pressure is lowered c. temp is lowered d. H2O is added e. none of these b.) Consider the following gas phase reaction at 25 oC. N2 (g) + C2H2

### Some Chemistry Problems

A.) For the reaction: 2Cl2 (g) + 2H2O(g) <----> 4HCl(g) + O2 (g), Kp = 6.4 x 10-6 at 500 K. If a fixed volume is filled with initial concentrations of these gases at 227 oC such that [Cl2] = 0.5 M, [H2O] = 0.40 M, [HCl] = 0.5 M, and [O2] = 0.015 M, in which direction will the reaction proceed? b.) 4.00 mol chlotine and 2.00 m

### General Chemistry

1. 4CuO(s) + CH4(g) CO2(g) + 4Cu(s) + 2H2O(g) The value of Kc for this reaction is 1.10 at 25.0°C. What is the value of Kp for this reaction? (R = 0.0821 L-atm/K-mol) a. 4.63 b. 26.9 c. 658 d. 37.2 e. 1.52 x 10-3 2. At a certa

### Complex ion equilibria

Complex-Ion Equilibria. When sufficient ammonia is added to a 0.00500 M silver nitrate solution to initially give 0.100 M aqueous ammonia, what is the molarity of the silver ion (Ag+) after the complex ion Ag(NH3)2+ has been formed at equilibrium? Ag+(aq) + 2 NH3(aq) = Ag(NH3)2+(aq)