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erma4kov [3.2K]
2 years ago
5

Two species, A and B, are separated on a 2.00 m long column which has 5.000 x 103 plates when the flow rate is 15.0 mL/min. A sp

ecies that is non-absorbing and known not to interact with the stationary phase, elutes in 30.0 s. Compound A elutes from the column in 5.00 min and Compound B elutes in 12.00 min.calculate the peak widths (in seconds) for Compounds A and B,
Chemistry
1 answer:
sergiy2304 [10]2 years ago
4 0

Explanation:

The given data is as follows.

         t_{m} = 30.0 sec,     t_{r1} = 5 min = 5 \times 60 sec = 300 sec

         t_{r2} = 12.0 min = 12 \times 60 sec = 720 sec

Formula for adjusted retention time is as follows.

      t'_{r} = t_{r} - t_{m}

                 = 300 sec - 30.0 sec

                 = 270 sec

   t'_{r2} = 720 sec - 30 sec

                            = 690 sec

Formula for relative retention (\alpha) is as follows.

          \alpha = \frac{t'_{r2}}{t'_{r1}}

                     = \frac{690 sec}{270 sec}

                     = 2.56

Thus, we can conclude that the relative retention is 2.56.

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Sulfur and oxygen react to produce sulfur trioxide. In a particular experiment, 7.9 grams of SO3 are produced by the reaction of
shutvik [7]

Answer:

  • <u>79%</u>

Explanation:

<u>1) Balanced chemical equation:</u>

  • 2S + 3O₂ → 2SO₃

<u>2) Mole ratio:</u>

  • 2 mol S : 3 mol O₂ : 2 mol SO₃

<u>3) Limiting reactant:</u>

  • Number of moles of O₂

        n = 6.0 g / 32.0 g/mol = 0.1875 mol O₂

  • Number of moles of S:

         n = 7.0 g / 32.065 g/mol = 0.2183 mol S

  • Ratios:

        Actual ratio: 0.1875 mol O₂ / 0.2183 mol S =0.859

        Theoretical ratio: 3 mol O₂ / 2 mol S = 1.5

Since there is a smaller proportion of O₂ (0.859) than the theoretical ratio (1.5), O₂ will be used before all S be consumed, and O₂ is the limiting reactant.

<u>4) Calcuate theoretical yield (using the limiting reactant):</u>

  • 0.1875 mol O₂ / x = 3 mol O₂ / 2 mol SO₃

  • x = 0.1875 × 2 / 3 mol SO₃ =  0.125 mol SO₃

<u>5) Yield in grams:</u>

  • mass = number of moles × molar mass = 0.125 mol × 80.06 g/mol =  10.0 g

<u>6) </u><em><u>Percent yield:</u></em>

  • Percent yield, % = (actual yield / theoretical yield) × 100
  • % = (7.9 g / 10.0 g) × 100 = 79%
6 0
2 years ago
Consider the ammonolysis of benzoyl chloride by adding concentrated ammonium hydroxide to form the final product, benzamide. Rea
gizmo_the_mogwai [7]

Answer:

Explanation: see attachment below

4 0
2 years ago
A chemist wants to extract copper metal from copper chloride solution. The chemist places 1.50 grams of aluminum foil in a solut
Lisa [10]

Answer: d. More than 6.5 grams of copper (II) is formed, and some copper chloride is left in the reaction mixture.

Explanation: 2Al+3CuCl_2\rightarrow 2AlCl_3+3Cu

As can be seen from the chemical equation, 2 moles of aluminium react with 3 moles of copper chloride.

According to mole concept, 1 mole of every substance weighs equal to its molar mass.

Aluminium is the limiting reagent as it limits the formation of product and copper chloride is the excess reagent as (14-7.5)=6.5 g is left as such.

Thus 54 g of of aluminium react with 270 g of copper chloride.

1.50 g of aluminium react with=\frac{270}{54}\times 1.50=7.5 gof copper chloride.

3 moles of copper chloride gives 3 moles of copper.

7.5 g of copper chloride gives 7.5 g of copper.

8 0
2 years ago
Read 2 more answers
How many moles of koh are contained in 750. ml of 5.00 m koh solution?
Marat540 [252]
Molarity is one of  the method of expressing concentration of solution. Mathematically it is expressed as,
 Molarity = \frac{\text{number of moles of solute}}{\text{volume of solution (l)}}

Given: Molarity of solution = 5.00 M
Volume of solution = 750 ml = 0.750 l

∴ 5 = \frac{\text{number of moles}}{.750}
∴ number of moles = 3.75

Answer: Number of moles of KOH present in solution is 3.75.
4 0
2 years ago
A 32.5 g piece of aluminum (which has a specific heat capacity of 0.921 J/g°C) is heated to 82.4°C and dropped into a calorimete
N76 [4]

Answer:

The mass of water = 219.1 grams

Explanation:

Step 1: Data given

Mass of aluminium = 32.5 grams

specific heat capacity aluminium = 0.921 J/g°C

Temperature = 82.4 °C

Temperature of water = 22.3 °C

The final temperature = 24.2 °C

Step 2: Calculate the mass of water

Heat lost = heat gained

Qlost = -Qgained

Qaluminium = -Qwater

Q = m*c*ΔT

m(aluminium)*c(aluminium)*ΔT(aluminium) = -m(water)*c(water)*ΔT(water)

⇒with m(aluminium) = the mass of aluminium = 32.5 grams

⇒with c(aluminium) = the specific heat of aluminium = 0.921 J/g°C

⇒with ΔT(aluminium) = the change of temperature of aluminium = 24.2 °C - 82.4 °C =  -58.2 °C

⇒with m(water) = the mass of water = TO BE DETERMINED

⇒with c(water) = 4.184 J/g°C

⇒with ΔT(water) = the change of temperature of water = 24.2 °C - 22.3 °C = 1.9 °C

32.5 * 0.921 * -58.2 = -m * 4.184 * 1.9

-1742.1 = -7.95m

m = 219.1 grams

The mass of water = 219.1 grams

8 0
2 years ago
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