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Mandarinka [93]
2 years ago
9

When collecting a gas over water, the gas is always a mixture of the gas collected and water vapor. question 5 options:

Chemistry
1 answer:
Lunna [17]2 years ago
6 0

When collecting gas over water, the gas is always a mixture of the gas collected and water vapor. This statement is true.

The gaseous phase of water is known as water vapor or aqueous vapor. Within the hydrosphere, it is one type of water state. Water vapor can be created by the boiling or evaporation of liquid water as well as by the sublimation of ice. Like the majority of other atmospheric elements, water vapor is transparent. The mist that hovers above a saucepan of boiling water is an illustration of water vapor.

Gaseous water, particularly when it is distributed in the atmosphere. Steam. The most frequent greenhouse gas is water vapor. It contributes to around half of the planet's warming. It absorbs heat that is projected upward from the earth while letting practically all sunlight reach the planet's surface like other greenhouse gases do.

To learn more about water vapor please visit -
brainly.com/question/20899075
#SPJ4

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If 12.5 grams of strontium hydroxide is reacted with 150 mL of 3.5 M carbonic acid, identify the limiting reactant.
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Answer:

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We'll begin by calculating the number of mole of carbonic acid in 150mL of 3.5 M carbonic acid solution. This is illustrated below:

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Next, we shall convert 0.525 mole of carbonic acid, H2CO3 to grams.

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Mass of H2CO3 = 0.525 x 62 = 32.55g

Next, we shall write the balanced equation for the reaction. This is given below:

Sr(OH)2 + H2CO3 → SrCO3 + 2H2O

Next, we shall determine the mass of Sr(OH)2 and H2CO3 that reacted from the balanced equation. This is illustrated below:

Molar mass of Sr(OH)2 = 88 + 2(16 + 1) = 88 + 2(17) = 122g/mol

Mass of Sr(OH)2 from the balanced equation = 1 x 122 = 122g

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Mass of H2CO3 from the balanced equation = 1 x 62 = 62g.

From the balanced equation above, 122g of Sr(OH)2 reacted with 62g of H2CO3.

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From the balanced equation above, 122g of Sr(OH)2 reacted with 62g of H2CO3.

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We can see evidently from the calculations made above that it will take 6.35g out 32.55g of H2CO3 to react with 12.5g of Sr(OH)2. Therefore, Sr(OH)2 is the limiting reactant and H2CO3 is the excess reactant

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