All categories

3 years ago

Question 12 of 25

Chemistry

1 answer:

NISA [10]3 years ago

8 0

Answer:

B. Equal amounts of all gases have the same volume at the same

conditions

Explanation:

Amedo Avogadro found the relationship between volume of a gas and the number of molecules contained in the volume.

The law states that "equal volumes of all gases at the same temperature and pressure contains equal number of molecules or moles".

The law describes the behavior of gases when involve in chemical reactions. It enables one to change over at will in any statement about gases from volumes to molecules and vice versa.

So, the right option is B which implies that equal amounts of all gases have the same volume at the same conditions.

You might be interested in

Scientific Notation expresses a value as the product of a number between 1 and 10 and

Bezzdna [24]

... and a power ot ten.

For example: 1,3x10^21 is in scientific notation, but 13x10^20 is not in scientific notation.

8 0

3 years ago

Fill in the blanks <br> At rest the frog breathes through________

Mama L [17]

Answer:

a process called predominate?

5 0

3 years ago

Read 2 more answers

Cuantos Electrones gano o perdió si pasa de -1 a +5

icang [17]

I dont speak spanish.

3 0

3 years ago

`Remember that an acid is something that donates hydrogen ions. So, when considering the formula HC2H3O2 (acetic acid), which of

tiny-mole [99]

Answer:

The H in the carboxyl group.

Explanation:

Acetic acid can be written as CH₃COOH, where -COOH is the functional group carboxyl, responsible for the acidity of organic acids. The H in the carboxyl group is the one that is donated in the acid reaction.

CH₃COOH(aq) + H₂O(l) ⇄ CH₃COO⁻(aq) + H₃O⁺

Acetic acid is a weak acid, so just a small fraction of the molecules undergo this reaction to donate their hydrogen.

5 0

3 years ago

g What is the half-life for a particular reaction if the rate law is rate = (1291 M⁻¹*min⁻¹)[A]² and the initial concentration o

Gnoma [55]

Answer:

$t_{1/2}=3.10x10^{-3}min=0.186s$

Explanation:

Hello,

In this case, for the calculation of the half-life for the mentioned reaction we first must realize that considering the units of the rate constant and the form of the rate law, it is a second-order reaction, therefore, the half-life expression is:

$t_{1/2}=\frac{1}{k[A]_0}$

Therefore, we obtain:

$t_{1/2}=\frac{1}{1291\frac{1}{M*min}*0.250M}\\\\t_{1/2}=3.10x10^{-3}min=0.186s$

Regards.

4 0

4 years ago