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3 years ago

Understanding the Cloning Process

Chemistry

2 answers:

Ratling [72]3 years ago

8 0

Answer:

A,B,D,E

Explanation:

Just had this question!

Nadusha1986 [10]3 years ago

4 0

The answer is 1, 2, 4, 5 or A, B, D, E

Explanation: I know this because I just did the Advances in Genetics Assignment on ed genuity

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A 150.0 mL sample of an aqueous solution at 25°C contains 15.2 mg of an unknown nonelectrolyte compound. If the solution has an

inysia [295]

Answer: The molar mass of the unknown compound is 223.2 g/mol

Explanation:

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

$\pi=iMRT$

where,

$\pi$ = osmotic pressure of the solution = 8.44 torr

i = Van't hoff factor = 1 (for non-electrolytes)

M = molarity of solute = ?

R = Gas constant = $62.3637\text{ L torr }mol^{-1}K^{-1}$

T = temperature of the solution = $25^oC=[273+25]=298K$

Putting values in above equation, we get:

$8.44torr=1\times M\times 62.3637\text{ L. torr }mol^{-1}K^{-1}\times 298K\\\\M=\frac{8.44}{1\times 62.3637\times 298}=4.54\times 10^{-4}M$

To calculate the molecular mass of solute, we use the equation used to calculate the molarity of solution:

$\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}$

We are given:

Molarity of solution = $4.54\times 10^{-4}M$

Given mass of unknown compound = 15.2 mg = 0.0152 g (Conversion factor: 1 g = 1000 mg)

Volume of solution = 150.0 mL

Putting values in above equation, we get:

$4.54\times 10^{-4}M=\frac{0.0152\times 1000}{\text{Molar mass of unknown compound}\times 150.0}\\\\\text{Molar mass of unknown compound}=\frac{0.0152\times 1000}{150.0\times 4.54\times 10^{-4}}=223.2g/mol$

Hence, the molar mass of the unknown compound is 223.2 g/mol

5 0

3 years ago

Difference between electroplating and sacrificial protection

Cerrena [4.2K]

Answer:

electroplating

Explanation:

Electroplating means coating a metal into zinc to protect from rust

Sacrificial protection is the protection of iron or steel against corrosion by using a more reactive metal

4 0

3 years ago

Ou encounter a solution that is acidic and you decide to test it by adding a small amount of a strong acid. the ph lowers slight

zimovet [89]

We can conclude that the solution is an acid buffer. A buffer system is when a weak acid is mixed with its salt. Its purpose is to resist changes in pH when small amounts of acid or base is added.

5 0

3 years ago

I want to produce 100 moles of N2. Now how many moles of NO do I need to start with?

cluponka [151]

Answer:

120 moles of NO

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

4NH₃ + 6NO —> 5N₂ + 6H₂O

From the balanced equation above,

6 moles of NO reacted to produce 5 moles of N₂.

Finally, we shall determine the number of mole NO needed to produce 100 moles of N₂. This can be obtained as follow:

From the balanced equation above,

6 moles of NO reacted to produce 5 moles of N₂.

Therefore, Xmol of NO will react to produce 100 moles of N₂ i.e

Xmol of NO = (6 × 100)/5

Xmol of NO = 120 moles

Therefore, 120 moles of NO is needed for the reaction.

5 0

3 years ago

Transmutation involves -nuclear change -chemical change -both a nuclear and a chemical change -neither a nuclear nor a chemical

SVEN [57.7K]

Answer: Option (a) is the correct answer.

Explanation:

Transmutation involves the conversion of one chemical element into another chemical element. This change occurs when an element or isotope passes through a number of reactions. It is a natural process and happens when there is a radioactive decay.

Hence, it is also a nuclear change as it occurs when there is a change in the nucleus of an atom. As this change can be due to the nuclear decay so as a result there will be some change in energy also. It is the process where one element converts into another using bombardment with high energy particles.

Thus, we can conclude that transmutation involves is a nuclear change.

3 0

3 years ago

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