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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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Read 2 more answers
Be sure to answer all parts. Calculate the pH of the following two buffer solutions: (a) 1.4 M CH3COONa/1.6 M CH3COOH. (b) 0.1 M
aalyn [17]

Answer:

a) pH = 4.68 (more effective)

b) pH =4.44.

Explanation:

The pH of buffer solution is obtained by Henderson Hassalbalch's equation.

The equation is:

pH =pKa +log\frac{[salt]}{[acid]}

a) pKa of acetic acid = 4.74

[salt] = [CH₃COONa] = 1.4 M

[acid] = [CH₃COOH] = 1.6 M

pH = 4.74 + log \frac{1.4}{1.6}= 4.68

This is more effective as there is very less difference in the concentration of salt and acid.

b) pKa of acetic acid = 4.74

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[acid] = [CH₃COOH] = 0.2 M

pH = 4.74 + log \frac{0.1}{0.2}= 4.44

3 0
4 years ago
PLEASE HELP CHEMISTRY
eduard

When sodium carbonate is dissolved in water, the equation is Na_2CO_3 (s) --- > 2Na^+ (aq) + CO_3^{2-} (aq).

When carbon dioxide is placed in water, aqueous carbon dioxide is formed:  CO_2 (g) --- > CO_2(aq)

<h3>Dissolution of compounds in water</h3>

Some compounds are water-soluble, some are just partially soluble, while others are insoluble in water. Some soluble or partially soluble substances dissociate in water into their component ions. These substances are said to be ionic.

Sodium carbonate, like every other sodium salt, is soluble in water. It dissolves in water to form an aqueous solution of sodium carbonate.

While in solution, sodium carbonate dissociates into its component ions according to the following equation:

Na_2CO_3 (s) --- > 2Na^+ (aq) + CO_3^{2-} (aq)

Carbon dioxide, on the other hand, does not dissociate in water. Instead, it dissolves in water where most of it remains as aqueous carbon dioxide in equilibrium with a small amount of hydronium ion and hydrogen carbonate ion.

Since the hydronium and hydrogen carbonate ions formed are so minute, the equation of the reaction can be written as: CO_2 (g) --- > CO_2(aq)

More on the dissolution of substances can be found here: brainly.com/question/28580758

#SPJ1

7 0
1 year ago
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