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taurus [48]
2 years ago
14

if 8.15 ml of water is placed in a graduated cylinder the mass of the cylinder = 56.98g and the combined mass of both the cylind

er of both the cylinder + water is 65.11g What is the mass of the water? what is the density of the water?
Chemistry
1 answer:
Allushta [10]2 years ago
4 0

1. The mass of the water is 8.13 g.

2. The density of the water is 1 g/mL

Density is related to mass and volume by the following equation:

<h3>Density = mass / volume </h3>

<h3>1. Determination of the mass of water. </h3>

Mass of cylinder = 56.98 g

Mass of cylinder + water = 65.11 g

<h3>Mass of water =? </h3>

<h3>Mass of water = (Mass of cylinder + water) – (Mass of cylinder) </h3>

Mass of water = 65.11 – 56.98

<h3>Mass of water = 8.13 g</h3>

Thus, the mass of the water is 8.13 g

<h3>2. Determination of the density of water. </h3>

Mass of water = 8.13 g

Volume of water = 8.15 mL

<h3>Density of water =? </h3>

Density = mass / volume

Density = 8.13 / 8.15

Density of water = 0.998 g/mL

<h3>Density of water ≈ 1 g/mL </h3>

Therefore, the density of the water is 1 g/mL

Learn more: brainly.com/question/24679715

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Read 2 more answers
Equal moles of H2, N2, O2, and He are placed into separate containers at the same temperature. Assuming each gas behaves ideally
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They would all exhibit the same pressure.

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Now, the gases were observed at the same temperature. This means they will all have the same pressure as their volume is the same.

Now we can further understand this by doing a simple calculation as follow:

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P = 1 atm

Therefore, H2 has a pressure of 1 atm.

For N2:

Number of mole (n) = 1 mole

Volume (V) = 22.4L

Temperature (T) = 298K

Gas constant (R) = 0.0821 atm.L/Kmol

Pressure =..?

PV = nRT

Divide both side V

P = nRT /V

P = 1 x 0.0821 x 298 / 22.4

P = 1 atm

Therefore, N2 has a pressure of 1 atm

For O2:

Number of mole (n) = 1 mole

Volume (V) = 22.4L

Temperature (T) = 298K

Gas constant (R) = 0.0821 atm.L/Kmol

Pressure =..?

PV = nRT

Divide both side V

P = nRT /V

P = 1 x 0.0821 x 298 / 22.4

P = 1 atm

Therefore, O2 has a pressure of 1 atm

For He:

Number of mole (n) = 1 mole

Volume (V) = 22.4L

Temperature (T) = 298K

Gas constant (R) = 0.0821 atm.L/Kmol

Pressure =..?

PV = nRT

Divide both side V

P = nRT /V

P = 1 x 0.0821 x 298 / 22.4

P = 1 atm

Therefore, He has a pressure of 1 atm.

From the above illustrations we can see that the gases have the same pressure since they have the same number of mole, volume and were observed at the same temperature.

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