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PolarNik [594]
3 years ago
8

Why does reducing oil pollution in the oceans require an international effort?

Chemistry
1 answer:
vitfil [10]3 years ago
8 0

Answer:

Half of Earth’s oceans are not owned by any particular country.

Explanation:

Reducing oil pollution requires an international effort because ocean waters do not have boundaries and there are certain portion of the ocean that are not owned by any nation.

  • Oil pollution is a serious environmental issue.
  • Oil spills can be carried by ocean currents from one place to another.
  • They affect the aquatic ecosystem within a locality thereby reducing the biodiversity of life.

International collaborations are sought to combat any issue of oil spillage due to global undertone to it.

You might be interested in
______ is a way to slow down the reactions that spoil milk
MAVERICK [17]

Answer:

b. keeping milk cold

Explanation:

The cool temperature in the fridge will stop it from going to any further reactions so it won't get spoilt

6 0
3 years ago
If light with a wavelength of 515 nm is shown on a metal surface, and photoelectrons (electrons ejected from the surface) have a
Debora [2.8K]

The binding energy of the electrons (also known as the work function of the surface) is determined as 2.43 x 10⁻¹⁹ J.

<h3>Binding energy of the electrons</h3>

The binding energy of the electrons is also known as work function of the metal and it is calculated as follows;

Ф = E - K.E

where;

Ф = hf - 86.2 kJ/mol

Ф = hc/λ - 86.2 kJ/mol

Ф = (6.63 x 10⁻³⁴ x 3 x 10⁸ )/515 x 10⁻⁹   -  86.2 kJ/mol

Ф = 3.86 x 10⁻¹⁹ J - (86200 J/mol)/(6.02 x 10²³)

Ф = 3.86 x 10⁻¹⁹ J - 1.43  x 10⁻¹⁹ J

Ф = 2.43 x 10⁻¹⁹ J

Learn more about work function here: brainly.com/question/19427469

#SPJ1

4 0
2 years ago
1.) Calculation: If 9.02 x 1024 particles of vinegar (HC2H3O2)HC2H3O2) are added to 16.5 moles of eggshell (CaCO3) and 6.35 mole
blsea [12.9K]

The theoretical yield of acetate is 2607 g. The actual yield of acetate is 1066.8 g. The percentage yield of acetate is 41%.

If 1 mole of vinegar contains 6.02  x 10^23 particles

x moles of vinegar contains 9.02 x 10^24 particles

x = 1 mole x 9.02 x 10^24 /6.02 x 10^23

x = 15 moles of vinegar

The reaction is as follows;

2HC2H3O2 + CaCO3 -----> Ca(C2H3O2)2 + H2O + CO2

Since 2 moles of vinegar reacts with 1 mole of carbonate

x moles of vinegar reacts with 16.5 moles of carbonate

x =  2 moles x 16.5 moles/ 1 mole

x = 33 moles of vinegar

We can see that the vinegar is the reactant in excess hence the carbonate is the limiting reactant.

Theoretical yield = 16.5 moles x 158 g/mol = 2607 g

Actual yield = 6.35 moles  x 158 g/mol = 1066.8 g

Percent yield = 1066.8 g/2607 g × 100/1

= 41%

Learn more: brainly.com/question/13440572?

7 0
3 years ago
Calculating the Molecular Weight and Subunit Organization of a Protein From Its Metal Content The element molybdenum (atomic wei
Deffense [45]

Answer:

Dimer of two peptide chains with 1 mole of molybdenum metal each.

Explanation:

Percentage of molybdenum in protein = 0.08%

Molecular mass of nitrate reductase = 240,000 g

Mass of molybdenum = x

0.08\%=\frac{x}{240,000 g}\times 100=192 g

Moles of molybdenum =\frac{192 g}{95.95 g/mol}=2.00 mol

Each peptide chain of nitrate reductase contain 1 mole of molybdenum.

This means that nitrate reductase is composed of to two peptide chains. And in each peptide there is a single mole of molybdenum metal.

4 0
4 years ago
The chemical formula for lithium fluoride is lif . a chemist determined by measurements that 0.035 moles of lithium fluoride par
Mnenie [13.5K]
Answer:
mass = 0.907865 grams

Explanation:
From the periodic table:
molar mass of Li = 6.941 grams
molar mass of F = 18.998 grams
Therefore:
molar mass of LiF = 6.941 + 18.998 = 25.939 grams/mole

number of moles can be calculated as follows:
number of moles = mass / molar mass
We have:
number of moles = 0.035 moles
molar mass = 25.939 grams/mole

Substitute in the equation to get the mass as follows:
0.035 = mass / 25.939
mass = 0.035 * 25.939 = 0.907865 grams

Hope this helps :)
3 0
3 years ago
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