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maxonik [38]
2 years ago
5

A gas under constant pressure has a volume of 30.57 m and a

Chemistry
1 answer:
gregori [183]2 years ago
6 0

Considering the relationship between volume and temperature, a gas under constant pressure can only have its volume reduced as a result of a decrease in its temperature.

According to Charles law, at constant pressure, the volume of a gas is directly proportional to its absolute temperature. Thus:

V1/T1 = V2/T2 where V1 = intial volume, V2 = final volume, T1 = initial temperature, and T2 = final temperature.

In this case, T1 = 59.0, V1 = 30.57, and V2 = 21.14

T2 = 21.14 x 59/30.57

                 = 20.05 K

It can be seen that the temperature of the gas has reduced from 59.0 K to 20.05K.

More on gas laws can be found here: brainly.com/question/1190311

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Answer:

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Explanation:

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<h3>Hope this helps</h3>
6 0
3 years ago
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Investigate: Note the empty jars on the shelf that can be filled by using the slider. Set the amount to 2.000 moles of carbon (m
balandron [24]

Answer:

The molar mass of carbon

Explanation:

Before the mass (in grams) of two moles of carbon can be determined, <u>the molar mass of the element would be needed.</u>

<em>This is because the number of mole of an element is the ratio of its mass and the molar mass</em>. That is,

number of mole = mass/molar mass

Hence, the mass of elements can be obtained by making it the subject of the formular;

mass = number of mole x molar mass

<em>Therefore, the molar mass of carbon would be needed before the mass of 2 moles of the element can be determined.</em>

3 0
2 years ago
Calculate the percent by mass of carbon in CO2 (carbon dioxide). Please show all work.
anygoal [31]
%C= 12/12 + 2·16=0,273=27,3%.
6 0
3 years ago
Calculate the pH of the solutions: [H^+]= 1.6 x 10^-3 M
Yuliya22 [10]

Answer:

A) pH = 2.8

B) pH = 5.5

C) pH = 8.9

D) pH = 13.72

Explanation:

a) [H⁺]  = 1.6 × 10⁻³ M

pH = -log [H⁺]

pH = -log [1.6 × 10⁻³ ]

pH = 2.8

b) [H⁺]  = 3 × 10⁻⁶

pH = -log [H⁺]

pH = -log [3 × 10⁻⁶ ]

pH = 5.5

c) [OH⁻] = 8.2 × 10⁻⁶

pOH = -log[OH]

pOH = -log[8.2 × 10⁻⁶]

pOH = 5.1

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pH = 14 - 5.1

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pOH = -log[0.53]

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pH = 14 - pOH

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5 0
3 years ago
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lukranit [14]

Answer:

is an aqueous reactant

is a liquid product

is a gaseous product

Explanation:

H_2CO_3 ⇔ CO_2 + H_2O

Hydrogen carbonate dissocates to form carbon dioxide and water. The acid (hydrogen carbonate) is in aqueous form and it dissociates to water (liquid) and carbon dioxide (a gas). It is also seen that the hydrogen carbonate is on the reactant side and it dissociates to produce water and carbon dioxide.

WH_2CO_3<u> is an aqueous reactant</u> (a reactant undergoes changes in a chemical reaction

<u />H_2O<u> is a liquid product</u> (product refers to the species produced from  chemical reaction)

<u />CO_2<u> is a gaseous product</u>

6 0
3 years ago
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