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lozanna [386]
3 years ago
11

If 1.240 g of carbon dioxide dissolves in 1.01 l of water at 755 mm hg, what quantity of carbon dioxide (in grams) will dissolve

at 790 mm hg?
Chemistry
2 answers:
Lelu [443]3 years ago
7 0

Answer : 1.297 g carbon dioxide will dissolve at 790 mm Hg

Explanation :

According to Henry's law, the amount of gas dissolved in water at a given temperature is directly proportional to its vapor pressure .

In equation format the law can be written as

C_{gas}= K\times P_{gas}

Here C is the concentration of the gas

P is the partial pressure of the gas

K is known as Henry's constant which is temperature dependent.

At 2 different partial pressure values, the equation can be modified as follows

\frac{C_{1}}{C_{2}}= \frac{P_{1}}{P_{2}}

Let us calculate C₁

C₁ = amount of gas in grams / L

C₁ = 1.240 g / 1.01 L

C₁ = 1.228 g/L

P₁ = 755 mm Hg

P₂ = 790 mm Hg

C₂ = ?

Let us plug in the values in Henry's equation

1.228 g L⁻¹ / C₂ = 755 mm Hg / 790 mm Hg

1.228 g L⁻¹ / C₂ = 0.956

C₂ = 1.228 g L⁻¹ / 0.956

C₂ = 1.285 g L⁻¹

The concentration of carbon dioxide at 790 mm Hg is 1.285 g/L

We have 1.01 L water.

Therefore the amount of gas dissolved = 1.01 L x 1.285 g/L = 1.297 g

1.297 g carbon dioxide will dissolve at 790 mm Hg in 1.01 L water

maria [59]3 years ago
7 0
Your answer is gonna be 1.297.
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Answer:

the volume occupied by 3.0 g of the gas is 16.8 L.

Explanation:

Given;

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pressure of the gas, P = 1 .0 atm

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atomic mass of helium gas, M = 4.0 g/mol

initial number of moles of the gas is calculated as follows;

n_1 = \frac{m_1}{M} \\\\n_1 = \frac{4}{4} = 1

The number of moles of the gas when the reacting mass is 3.0 g;

m₂ = 3.0 g

n_2 = \frac{m_2}{M} \\\\n_2 = \frac{3}{4} \\\\n_2 = 0.75 \ mol

The volume of the gas at 0.75 mol is determined using ideal gas law;

PV = nRT

PV = nRT\\\\\frac{V}{n} = \frac{RT}{P} \\\\since, \ \frac{RT}{P} \ is \ constant,\  then;\\\frac{V_1}{n_1} = \frac{V_2}{n_2} \\\\V_2 = \frac{V_1n_2}{n_1} \\\\V_2 = \frac{22.4 \times 0.75}{1} \\\\V_2 = 16.8 \ L

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4 0
3 years ago
A 10.5 mL sample of vinegar, containing acetic acid, was titrated using 0.460 M NaOH solution. The titration required 19.13 mL o
laila [671]

Explanation:

Step 1:

A good first step for a problem like this is to write down the chemical formula and balance it.

It appears here that we have 10.5 mL of vinegar, which IS acetic acid, and 19.13 mL of 0.460 M NaOH. That will give us the following balanced chemical equation:

CH3COOH + NaOH ------> NaCH3COO + H2O

All of the constituents come out to a value of 1, conveniently.

Step 2:

Since all of our stoichiometric coefficients are one, we can use a shortcut to answer this equation. I don't know if it has a name, but I just call it the titration formula. It goes something like this:

M1 * V1 = M2 * V2

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So, our M1 for this is going to be what the question says was used for this titration. That's 0.460M NaOH.

Our V1 is going to be the initial volume of the sample, which was 10.5 mL

Our V2 is going to be 19.13, which is the volume when we're finished.

It's clear that we don't know M2, so let's find it.

Keep in mind that it's easier to convert to liters pretty much always, so I've done that by dividing the mL values each by 1000.

Using some algebra, we can see that we now have:

0.460 M * 0.0105 L = x M * 0.01913 L

Which goes to:

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<h3>So our M2, the molar concentration of acetic acid in this vinegar, is equal to 0.252 M. </h3>
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Assuming 100% dissociation, calculate the freezing point and boiling point (in °C) of a solution with 83.6 g of AgNO 3 in 1.00 k
Thepotemich [5.8K]

Answer:

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Explanation:

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The freezing point will decrease and the boiling point will increase. These are two colligative properties.

<u></u>

<u>Find attached the file with the whole answer, as the site is not uploading the answer in here.</u>

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8 0
3 years ago
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