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sladkih [1.3K]
3 years ago
5

Calculate the H3O+ concentration and then pH in a 0.100 M HC2H3O2 solution that is

Chemistry
1 answer:
Lana71 [14]3 years ago
5 0

Answer:

Please check with the attachment posted.

Please do confirm the answer.

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Gas Law- please help!!!
jekas [21]

The pressure of the carbon dioxide will be 0.09079 atm.

<h3>What is partial pressure?</h3>

The pressure exerted by the individual gas is known as partial pressure.

The partial pressure is given as

\rm P_{Total} = P_1 + P_2 + ...

In a mixture of carbon dioxide and oxygen, 40.0% of the gas pressure is exerted by oxygen.

If the total pressure is 115 mmHg.

The total pressure in atm will be

P = 115 mmHg

P = 0.15132 atm

We have

\rm P_T \ \  \  = P_{O_2} + P_{CO_2}\\\\0.15132 \ \  = 0.4 \times 0.15132 +P_{CO_2}\\\\ P_{CO_2} = 0.09079\ atm

Then the pressure of the carbon dioxide will be 0.09079 atm.

More about the partial pressure link is given below.

brainly.com/question/13199169

#SPJ1

8 0
2 years ago
What is enthalpy of atomisation
Komok [63]
The enthalpy of atomization (also atomisation in British spelling) is the enthalpy change that accompanies the total separation of all atoms in a chemical substance (either a chemical element or a chemical compound)
5 0
3 years ago
How many grams of sulfur in 4.20 x 1021 atoms of sulfur?
Stolb23 [73]

Answer:

look it up

Explanation:

6 0
2 years ago
Can pure substances made from compounds be physically separated?
Arisa [49]

Answer:

it cannot !!

Explanation:

a chemical reaction MUST occur to separate a compound! :)

4 0
3 years ago
if I have 22.1 grams of CO2 gas at -188 degrees Celsius and 165 ml what is the pressure of the gas in kPa​
Harman [31]

Answer:

P = 2.145kPa

Explanation:

Mass = 22.1g

Molar mass of CO2 = 44g/mol

Vol = 165mL = 0.165L

T = -188°C = (-188 + 273.15)K = 85.15K

R = 8.314J/mol.K

From ideal gas equation,

PV = nRT

P = pressure of the ideal gas

V = volume the gas occupies

n = number of moles if the gas

R = ideal gas constant

T = temperature of the gas

n = number of moles

n = mass / molar mass

n = 22.1 / 44 = 0.50moles

PV = nRT

P = nRT/ V

P = (0.5 × 8.314 × 85.15) / 0.165

P = 2145.26Pa = 2.145kPa

Pressure of the gas is 2.145kPa

6 0
3 years ago
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