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Ahat [919]
3 years ago
6

If a gas's temperature doubles and its volume remains constant, then what happens to its pressure?

Chemistry
1 answer:
Semenov [28]3 years ago
6 0

Answer : The pressure become doubles.

Explanation :

Gay-Lussac's Law : It is defined as the pressure of the gas is directly proportional to the temperature of the gas at constant volume and number of moles.

P\propto T

or,

\frac{P_1}{T_1}=\frac{P_2}{T_2}

where,

P_1 = initial pressure

P_2 = final pressure

T_1 = initial temperature

T_2 = final temperature = 2T_1

Now put all the given values in the above equation, we get:

\frac{P_1}{T_1}=\frac{P_2}{2T_1}

\frac{P_2}{P_1}=2

From this we conclude that, as the temperature of gas doubles then the pressure of gas become doubles because pressure is directly proportional to the temperature of gas.

Hence, the pressure become doubles.

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A chemical reaction can theoretically produce 137.5 grams of product, but in actuality 112.9 grams are
Butoxors [25]
<h3>Answer:</h3>

82.11%

<h3>Explanation:</h3>

We are given;

  • Theoretical mass of the product is 137.5 g
  • Actual mass of the product is 112.9 g

We are supposed to calculate the percentage yield

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Thus;

% yield = (Actual mass ÷ Experimental mass) × 100%

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7 0
3 years ago
A pharmaceutical company is making a large volume of nitrous oxide (NO). They predict they will be able to make a maximum amount
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Answer:

The answer is "Option B"

Explanation:

From the query, the following knowledge is derived:  

Yield in percentage = 47%  

Performance of theory = 4860 g  

Actual yield Rate =?  

The percentage return is defined simply by the ratio between both the real return as well as the conceptual return multiplied by the 100. It's also represented as numerically:

Rate = \frac{Existing \ Rate} {Theoretical \ Rate} \times 100

Now We can obtain the percent yield as followed using the above formula:  

\text{Yield in percentage}= \frac{Actual \ yield \ Rate} {Theorical \ Rate} \times  100

47\% = \frac{Actual \ yield \ Rate}{4860}

The value of the Actual yield Rate =47\% \times 4860

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3 years ago
Which of the following statements is incorrect? A. Molecular mass is expressed in atomic mass units. B. Formula mass compares th
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Answer:

  • The incorrect statement is the choice <em>C. Atomic mass has units of grams per atom.</em>

Explanation:

<u>1) Choice A.</u><em><u> Molecular mass is expressed in atomic mass units</u></em><u>.</u>

Correct. Atomic mass units (a.m.u) is the standard unit used to express the mass of the atoms and the molecules.

Since, one atom, molecule, or formula unit is a tiny amount of material, it has a ver, very low mass, and the unit mass of a molecule is referred to one mole (6.022 × 10²³ units).

<u>2) Choice B. </u><em><u>Formula mass compares the mass of one formula unit of a substance to the mass of one atom of carbon-12</u></em><u>.</u>

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<u>3)  Choice C. </u><em><u>Atomic mass has units of grams per atom.</u></em><u> </u>

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<u>4) Choice D. </u><em><u>Both molecular mass and formula mass use carbon-12 as a reference standard.</u></em>

Correct. As stated when explaining the option B, the mass of atoms, molecules, and formula units are referred to carbon-12 standard.

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Correct. The reason is that ionic compounds form large structures (crystals) and, since there is not such thing as one molecule of them, they are said to have formula weight (or mass) but not a molecular weight.

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