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aalyn [17]
4 years ago
10

How many atoms are in 0.075 mol of Carbon (C)?

Chemistry
1 answer:
lidiya [134]4 years ago
5 0
The amount of atoms in 1 mole of carbon is 6.022 X 10^3 so with it being 0.075 mole it will be option A 4.5 X 10^22 atoms
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A researcher was attempting to quantify the amount of dichlorodiphenyltrichloroethane (DDT) in spinach with gas chromatography u
devlian [24]

Answer:

0.0136mg DDT / g spinach

Explanation:

Quantification in chromatography by internal standard has as formula:

RF = Aanalyte×Cstd / Astd×Canalyte <em>(1)</em>

<em>Where RF is response factor, A is area and C is concentration</em>

Replacing with first experiment values:

RF = 5019×3.20mg/L / 8179×6.37mg/L

RF = 0.308

In the next experiment, final concentration of chloroform was:

11.45mg/L × (1.25mL / 25.00mL) = <em>0.5725mg/L</em>

From (1), it is possible to write:

Aanalyte×Cstd / Astd×RF = Canalyte

Replacing:

6821×0.5725mg/L / 14061×0.308 = Canalyte

Canalyte = <em>0.9017mg/L</em>

as the sample was made from 0.750mL of extract. Concentration of extract is:

0.9017mg/L × (25.00mL / 0.750mL) = 30.06mg/L. As the extract has a volume of 2.40mL:

30.06mg/L × 2.40x10⁻³L = <em>0.07213mg of DDT in the extract</em>

As the extract was made from 5.29g of spinach:

0.07213mg of DDT in the extract / 5.29g spinach = <em>0.0136mg DDT / g spinach</em>

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3 years ago
How does particle model explain a change of state of matter?
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5 0
4 years ago
What is the overall charge of the electron cloud of the atom? Explain.​
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Which scientific discipline best links the use of titanium and plastics in artificial bone and joint replacements?
yarga [219]
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4 0
3 years ago
Read 2 more answers
Consider the reaction below in a closed flask. At 200 o C, the equilibrium constant (Kp) is 2.40 × 103 . 2 NO (g)  N2 (g) + O2
olga55 [171]

Explanation:

Since, the given reaction is as follows.

       2NO(g) \rightleftharpoons N_{2}(g) + O_{2}(g)

Initial:    36.1 atm                 0          0

Change:    2x                      x           x

Equilibrium: (36.1 - 2x)       x            x

Now, expression for K_{p} of this reaction is as follows.

            K_{p} = \frac{[N_{2}][O_{2}]}{[NO]^{2}}

As the initial pressure of NO is 36.1 atm. Hence, partial pressure of O_{2} at equilibrium will be calculated as follows.

              K_{p} = \frac{[N_{2}][O_{2}]}{[NO]^{2}}

        2.40 \times 10^{3} = \frac{x \times x}{(36.1 - 2x)^{2}}

                 x = 18.1 atm

Thus, we can conclude that partial pressure of O_{2} at equilibrium is 18.1 atm.

5 0
3 years ago
Read 2 more answers
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