Chemical engineering question

A synthesis gas containing 6.4% CO₂, 0.2% O₂, 40.0% CO and 50.8% H₂ (the remainder is N₂) is burned with 40 % excess dry air (assume 21 % O₂ and 79 % N₂).

i)Identify the reactions occurring during combustion of this syngas.

ii)Calculate the amount of air added per 100 mol of syngas.

iii)If complete combustion occurs, then calculate the composition of the flue gas on a weight basis.

Pre-Laboratory Questions (An Acid Base Titration)

1. Show the reaction between HCl and NaOH. Label the acid, base, and each of the products.

2. What occurs at the equivalence point?

3. Consider the titration of 10.00 mL of 0.10 M HCl with 0.10 M NaOH

a.) What salt is formed during this reaction?

b.) Do you expect the salt solution at the equivalence point to be acidic, neutral, or basic?

4. Consider the titration of 10.00 mL of 0.10 M acetic acid (CH3COOH) with 0.10 M NaOH

a.) What salt is formed during this reaction?

b.) Do you expect the salt solution at the equivalence point to be acidic, neutral, or basic?

5. Calculate the pH of the solution in question 4 at the equivalence point.

Deterime the % of Acetic Acid in vinegar in your kitchen. Show how to determine it in words and make up random numbers to calculate it also.

Determine the purity of an Aluminum can. In words how would you determine the purity? Also, make up random numbers to calculate how to find the purity of an Aluminum can.

Identifiy the ions present in a sample possibly containing Ag+ Pb2+ Br2+ Na+ Ca2+. Construct a flowchart using these ions.

Write and balance the equation for the complete combustion of ethane, C2H6.

The OH radical is important in the daytime chemistry reactions in the formation of air pollutants.(which one is correct?)

A.it is formed from nitrous acid

B. it reacts with hydrocarbons

C. it is formed from hydrogen peroxide

D it is formed from ozone

E. it is formed only in the early morning hours.

The reaction SO2(g)+2H2S(g) ⇌ 3 S(s)+2H2O(g) is the basis of a suggested method for removal of SO2, a pollutant that irritates airways causing coughing, from power-plant stack gases. The values below may be helpful when answering questions about the process.

Question: Using Le Châtelier's principle, determine how the process is affected after each of the following temperature or pressure changes. Consider that a more effective reaction produces more product or more product in a shorter amount of time.

Drag the appropriate items to their respective bins.

a) Temperature increases while maintaining the container size.

b) Pressure increases by decreasing the container size

c) Pressure decreases by increasing the container size.

d) Temperature decreases while maintaining the container size.

place the above under category of More Effective, Less Effective or Equally Effective.

During the metabolism of amino acids, amino groups are often switched from one organic compound to another through a process called transamination. The following are two examples of transamination reactions with their corresponding free energy changes:

glutamate + pyruvate ---> α-ketoglutarate + alanine              ∆G^o' = - 1.00 kJ/mol

glutamate + oxaloacetate ---> α-ketoglutarate + aspartate      ∆G^o' = - 4.81 kJ/mol

Answer the following questions about transamination.

a. Using the two equations given above, write an equation for the net formation of alanine and oxaloacetate from aspartate and pyruvate.

b. Calculate the standard free energy change for this overall reaction and indicate whether it will go spontaneously in the direction indicated.

c. Suppose that under steady state conditions in a cell at 37 ^oC, the actual concentrations of pyruvate and aspartate are 1.2 x 10^-2 M, the concentration of alanine is 1.5 x 10^-4 M, and the concentration of oxaloacetate is 1.9 x 10^-5 M. Using the equation that ∆G = ∆G^o' + RT ln [products]/[reactants] and the gas constant of R = 8.315 J/mol K, calculate the actual free energy change and determine if the reaction is spontaneous

1. Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory to standardize strong base solutions. It has the unwieldy formula of KHC₈H₄O₄. This is often written in shorthand notation as KHP.

How many grams of KHP are needed to exactly neutralize 23.2 mL of a 0.557 M potassium hydroxide solution ?

2. Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory to standardize strong base solutions. It has the unwieldy formula of KHC₈H₄O₄. This is often written in shorthand notation as KHP.

What volume of a 0.458 M potassium hydroxide solution is needed to exactly neutralize 2.67 grams of KHP ?

3. A student is asked to standardize a solution of barium hydroxide. He weighs out 1.04 g potassium hydrogen phthalate (KHC₈H₄O₄, treat this as a monoprotic acid).

It requires 37.9 mL of barium hydroxide to reach the endpoint.

A. What is the molarity of the barium hydroxide solution?

This barium hydroxide solution is then used to titrate an unknown solution of hydrobromic acid.

B. If 21.7 mL of the barium hydroxide solution is required to neutralize 13.0 mL of hydrobromic acid, what is the molarity of the hydrobromic acid solution?

4. A student is asked to standardize a solution of calcium hydroxide. He weighs out 1.04 g potassium hydrogen phthalate (KHC₈H₄O₄, treat this as a monoprotic acid).

It requires 32.9 mL of calcium hydroxide to reach the endpoint.

A. What is the molarity of the calcium hydroxide solution?  M

This calcium hydroxide solution is then used to titrate an unknown solution of hydroiodic acid.

B. If 16.2 mL of the calcium hydroxide solution is required to neutralize 20.4 mL of hydroiodic acid, what is the molarity of the hydroiodic acid solution?  M

(a) Calculate the percent ionization of 0.00710 M butanoic acid (Ka = 1.5e-05). % ionization = % (b) Calculate the percent ionization of 0.00710 M butanoic acid in a solution containing 0.0210 M sodium butanoate. % ionization = %

1. If 14.95 mL of a 0.1250 M HCl solution is added to reach the endpoint of a titration, how many moles of HCl have been added?

QUESTION 2

A buret is read to how many decimal places?

QUESTION 3

As the endpoint nears what happens to the color?

QUESTION 4

A 20.00 mL sample of 0.1015 M nitric acid is introduced into a flask, and water is added until the volume of the solution reaches 250. mL. What is the concentration of nitric acid in the final solution?

QUESTION 5

If 25.0 mL of an unknown concentration of sodium hydroxide is added to a flask and then titrated with 0.1025 M HCl. If 24.69 mL of the acid was added, what is the concentration of sodium hydroxide?

For toluene determine:
a) Vapor pressure at 100 ° C.
b) Its boiling temperature at a pressure of 530 torr.
c) Draw the liquid-vapor equilibrium curve from 13 to 136 ° C.

Consider the titration of 39.2 mL of 0.260 M HF with 0.215 M NaOH. Calculate the pH at each of the following points.

A. Calculate the pH after the addition of 9.80 mL of base

B.Calculate the pH at halfway to the equivalence point.

C. Calculate the pH at the equivalence point.

Why does krypton form crystals at sufficiently low temperatures despite having no
permanent dipole moments?

Explain tactility using poly(acrylonitrile) as an example.

A solution is 5 mM in each of the following ions:

Indicate which of the metal ions would precipitate (or start to precipitate) at each of the following pH values. Indicate your answer with the number of the ion. Use 0 to indicate no precipitate. If more than one precipitate is expected, list the numbers in increasing order and separate them with commas. For example, 3,4,5 is ok but 5,4,3 is not.

pH = 5.00:

pH = 9.00:

What is the pH to the nearest 0.1 pH unit at which Mg(OH)₂ begins to precipitate?

pH =