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kherson [118]
3 years ago
9

The Earth’s atmosphere contains about 0.04% (or 400 parts per million) carbon dioxide. Although most of the carbon dioxide is in

the form 12CO2, which is not radioactive, a specific fraction of the total is made up of radioactive 14CO2.
A) True
B) False
Chemistry
1 answer:
MArishka [77]3 years ago
7 0

Answer:

True

Explanation:

Yes the given statement is true

Most of the carbon dioxide preset in the atmosphere is C12 isotope and a very small fraction of The atmosphere is made up by C14 isotope which is radioactive in nature

C14 makes about 1 to 1.5 atoms per 10^{12} atoms of carbon in the atmosphere.

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In the preparation of a certain alkyl halide, 10 g of sodium bromide (NaBr), 10 mL distilled water (H20), and 9 mL 3-methyl-1-bu
Novosadov [1.4K]

Percentage yield shows the amount of reactants converted into products. The percentage yield of the reaction is 51.7%.

The equation of the reaction is sown in the image attached. The reaction is 1:1 as we can see.

Number of moles of NaBr = 10 g/103 g/mol = 0.097 moles

We can obtain the mass of 3-methyl-1-butanol from its density.

Mass = density × volume

Density of 3-methyl-1-butanol =  0.810 g/mL

Volume of  3-methyl-1-butanol = 9 mL

Mass of 3-methyl-1-butanol = 0.810 g/mL × 9 mL

Mass of 3-methyl-1-butanol = 7.29 g

Number of moles of 3-methyl-1-butanol =  mass/molar mass =  7.29 g/88 g/mol = 0.083 moles

Since the reaction is 1:1 then the limiting reagent is 3-methyl-1-butanol

Mass of product 1-bromo-3-methylbutane = number of moles × molar mass

Molar mass of 1-bromo-3-methylbutane = 151 g/mol

Mass of product 1-bromo-3-methylbutane = 0.083 moles × 151 g/mol

= 12.53 g

Recall that % yield = actual yield/theoretical yield × 100

Actual yield of product = 6.48 g

Theoretical yield = 12.53 g

% yield = 6.48 g/12.53 g × 100

% yield = 51.7%

Learn more: brainly.com/question/5325004

7 0
2 years ago
3 H2 (g) + N2 (g) 2 NH3 (g)
ale4655 [162]

Answer:

Mass = 0.697 g

Explanation:

Given data:

Volume of hydrogen = 1.36 L

Mass of ammonia produced = ?

Temperature = standard = 273.15 K

Pressure = standard = 1 atm

Solution:

Chemical equation:

3H₂ + N₂       →      2NH₃

First of all we will calculate the number of moles of hydrogen:

PV  = nRT

R = general gas constant = 0.0821 atm.L/mol.K

1atm ×1.36 L = n × 0.0821 atm.L/mol.K × 273.15 K

1.36 atm.L = n × 22.43 atm.L/mol

n = 1.36 atm.L / 22.43 atm.L/mol

n = 0.061 mol

Now we will compare the moles of hydrogen and ammonia:

                 H₂         :          NH₃

                  3          :            2

                0.061     :         2/3×0.061 = 0.041

Mass of ammonia:

Mass = number of moles × molar mass

Mass = 0.041 mol × 17 g/mol

Mass = 0.697 g

4 0
3 years ago
Help help help help please
Sav [38]

Explanation:

what is the end of the question???

4 0
3 years ago
ether has a density of 0.736 g/cm^3 at 20 degrees C. what is the volume, in liters, of 225.0 grams of ether?
polet [3.4K]
D = m / V

0.736 = 225.0 / V

V = 225.0 / 0.736

V = 305.7 cm³
5 0
2 years ago
If a 0.10 M solution of a colored substance has a maximum absorbance at 500 nm and an absorbance of 0.26 M at this wavelength, w
Mashcka [7]
Absorbance is related to the concentration of a substance using the Beer-Lambert's Law. According to this law, absorbance is linearly related to concentration. However, this is only true up to a certain concentration depending on the substance. For this case, we assume that the said law is applicable.

A = kC
Using the first conditions, ewe solve for k.
0.26 = k (0.10)
k = 2.6

A = kC
A = 2.6 (0.20) = 0.52

Therefore, the absorbance at a concentration of 0.20 M and wavelength of 500nm is 0.52.
7 0
2 years ago
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