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4 years ago

How did qualitative chemical and enzyme tests help avery identify dna as the transforming principle?

2 answers:

7 0

Qualitative chemical and enzyme tests helped Avery identify DNA as the transforming principle by conducting <span>a series of tests to find out if the transforming principle was DNA or a protein and the result is that </span>no protein was present but that DNA was present. Hope this answers your question.

kvv77 [185]4 years ago

5 0

Answer:

Qualitative chemical and enzyme tests help Avery to identify DNA as the transforming principle as they clarify the chemical nature of genes, that they are form of nucleic acids.

Explanation:

One of Avery’s qualitative chemical test result was that the transforming principle could precipitate with alcohol, so this demonstrate it was not a carbohydrate.

The enzyme test demonstrated that proteases (enzymes that digest protein) and lipases (enzymes that digest lipids) did not destroy the transforming principle, so the scientist concluded that it was neither a protein nor a lipid.

The bacteriologist found out that the transforming principle was formed of nucleic acids so they tested the sample with ribonuclease (enzyme that digest RNA) but it did not inactivate the substance. And finally he tested it with deoxyribonuclease and it was enzymatically destroyed. So he concluded that the isolated transforming principle was DNA.

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How well can you apply Charles’s law to this sample of gas that experiences changes in pressure and volume? Assume that pressure

anzhelika [568]

Answer:

A: 384

B: 0.85

C: 1.1

D: 221

Explanation:

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3 years ago

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This is due at 4:00 P.M. and I do not want to make a 76%, so please help MEEEEEEEEEEEEE!!!

Ann [662]

Answer:

Hi, There!...

<h2>Answer</h2>

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Explanation:

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3 years ago

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How many moles ar Li are in 9.53x^24 atoms of Li?

Anna35 [415]

Answer: 15.83 mol

Explanation:

To convert from atoms to moles, we will need to use Avogadro's number.

Avogardo's number: 6.022×10²³ atoms/mol

$9.53*10^{24} atoms*\frac{1mol}{6.022*10^2^3 atoms} =15.83 mol$

Now, we know that there are 15.83 moles.

5 0

3 years ago

A chemist wants to extract copper metal from copper chloride solution. The chemist places 0.25 grams of aluminum foil in a solut

mrs_skeptik [129]

Answer: The correct answer is about 0.20 grams of copper (II) is formed, and some aluminum is left in the reaction mixture.

Explanation:

To calculate the number of moles, we use the formula:

$Moles=\frac{\text{Given mass}}{\text{Molar mass}}$

<u>Moles of Aluminium:</u>

Molar mass of aluminium = 27 g/mol

Given mass of aluminium = 0.25g

Putting values in above equation, we get:

$Moles=\frac{0.25g}{27g/mol}=0.00925mol$

<u>Moles of Copper chloride:</u>

Molar mass of copper chloride = 134.45 g/mol

Given mass of copper chloride= 0.40g

Putting values in above equation, we get:

$Moles=\frac{0.40g}{134.45g/mol}=0.00297mol$

For the given chemical equation:

$4Al(s)+3CuCl_2(aq.)\rightarrow 2Al_2Cl_3(aq.)++3Cu(s)$

By Stoichiometry,

3 moles of Copper chloride reacts with 4 moles of aluminium

So, 0.00297 moles of copper chloride will react with = $\frac{4}{3}\times 0.00297$ = 0.00396 moles of Aluminium.

As, the required moles of aluminium is less than the given moles of aluminium. Hence, it is considered as the excess reagent.

Copper chloride is the limiting reagent in the given chemical reaction because it limits the formation of products.

By Stoichiometry of the reaction:

3 moles of copper chloride produces 3 moles of copper metal.

So, 0.00297 moles of copper chloride will produce = $\frac{3}{3}\times 0.00297$ = 0.00297 moles of copper metal.

Now, to calculate the given mass of copper metal, we use the equation required to calculate moles:

Molar mass of copper = 63.5 g/mol

Putting values in that equation, we get:

$0.00297mol=\frac{\text{given mass}}{63.5g/mol}$

Given mas of copper metal = 0.188grams (approx 0.20grams)

For the given reaction, some of the aluminum is left behind because it is the excess reagent in the reaction.

Hence, the correct answer is about 0.20 grams of copper (II) is formed, and some aluminum is left in the reaction mixture.

6 0

3 years ago

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Balance the following oxidation-reduction reaction: Fe(s)+Na+(aq)→Fe2+(aq)+Na(s) Express the coefficients as integers separated

aliina [53]

Answer:

The answer to your question is: 1, 2, 1, 2

Explanation:

1 Fe(s) + 2 Na⁺(aq) → 1 Fe²⁺(aq) + 2 Na(s)

Fe⁰ - 2e⁻ ⇒ Fe⁺² Oxidases

Na⁺ + 1 e⁻ ⇒ Na⁰ Reduces

1 x ( 1 Fe⁰ ⇒ 1 Fe⁺²) Interchange number of

2 x ( 2Na⁺ ⇒ 2 Na⁰ ) electrons

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3 years ago