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Lemur [1.5K]
2 years ago
12

A gas occupying 50.0 ml volume in a confined space at 20.0 dc at 50.0 kpa is heated to 40.0 dc. What is the pressure exerted by

the gas in the container?
Chemistry
1 answer:
aliina [53]2 years ago
7 0

Answer:

The pressure exerted by the gas is 100kPa

Explanation:

Let's apply the Charles Gay Lussac law, to solve the question.

At constant volume the pressure varies proportionally with the temperature.

P initial / T° initial = P final / T° final

50kPa / 20°C = P final / 40°C

Temperature has increased the double, so the pressure will be increased, the double too.

100 kPa

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Kruka [31]

Answer:

Well I know that when the liquid changes from clear to dark blue and small bubbles form and rise to the surface that is a reaction

Explanation:

7 0
3 years ago
What was the result of the atomic theory?
Cerrena [4.2K]

Answer:

The result of the atomic theory was atomic theory proposed that all matter was composed of atoms, also postulated that chemical reactions resulted in the rearrangement of the reacting atoms.

4 0
3 years ago
Hydrogen produced from a hydrolysis reaction was collected over water and the following data was compiled.
Shkiper50 [21]

Answer:

  • 0.00358 mol

Explanation:

<u>1) Data:</u>

a) V = 93.90 ml

b) T = 28°C

c) P₁ = 744 mmHg

d) P₂ = 28.25 mmHg

d) n = ?

<u>2) Conversion of units</u>

a) V = 93.90 ml × 1.000 liter / 1,000 ml = 0.09390 liter

b) T = 28°C = 28 + 273.15 K = 301.15 K

c) P₁ = 744 mmHg × 1 atm / 760 mmHg = 0.9789 atm

d) P₂ = 28.5 mmHg × 1 atm / 760 mmHg = 0.0375 atm

<u>3) Chemical principles and formulae</u>

a) The total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas. Hence, the partical pressure of the hydrogen gas collected is equal to the total pressure less the vapor pressure of water.

b) Ideal gas equation: pV = nRT

<u>4) Solution:</u>

a) Partial pressure of hydrogen gas: 0.9789 atm - 0.0375 atm = 0.9414 atm

b) Moles of hygrogen gas:

pV = nRT ⇒ n = pV / (RT) =

n =  (0.9414 atm × 0.09390 liter) / (0.0821 atm-liter /K-mol × 301.15K) =

n = 0.00358 mol (which is rounded to 3 significant figures) ← answer

7 0
3 years ago
Read 2 more answers
Calculate each of the following quantities:<br> (a) Total number of ions in 38.1 g of SrF₂
adelina 88 [10]

The total number of ions in 38.1 g of SrF₂ is 5.479 x 10²³.

<h3>What are ions?</h3>

Ions are the elements with a charge on them. It happens when they share electrons with other atoms to form a compound.

We have to calculate the total number of ions in 38.1 g of .

The molar mass of SrF₂ = 125.62 g/mol

The number of moles = 38.1 g of  1.0 mol / 125.62  = 0.30329 moles

Given that, total moles of SrF₂ ions in  = 1.0 mol of + 2.0 moles of  = 3.0 moles

Total moles of ions in 0.30329 moles of

= (0.30329 moles of SrF₂) x 3.0 / 1.0  = 0.90988 mol ions

We know that,

1.0 mole of ions = 6.023 x 10²³ ions

Thus, the number of total ions = ( 0.90988 mol ions) x  6.023 x 10²³ / 1.0 mol = 5.479 x 10²³ ions

Thus, the number of ions is in 38.1 g of 5.479 x 10²³ ions

To learn more about ions, refer to the link:

brainly.com/question/14295820

#SPJ4

8 0
1 year ago
4HCI + O2 =2H20 + Cl2
Sergio039 [100]

The rate of the backward reaction increases

Explanation:

It is evident that if the reaction is left to proceed spontaneously, the forward reaction is favored because it results in a decrease in pressure in the system (The total reactants have 5 moles and the products have 3 in total).

Increasing H₂O concentration is then reaction, therefore, stymies the forward reaction and favors the reserves reaction. This is because the reverse reaction will lead to reduced pressure.

6 0
3 years ago
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