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Fudgin [204]
3 years ago
5

5. You have two sealed jars of water at the same temperature. In the first jar there is a large amount of water. In the second j

ar there is a small amount of water. Using 3 -4 sentences explain how the vapor pressure of water in the first jar compares with the vapor pressure of water in the second jar.
Chemistry
1 answer:
Aneli [31]3 years ago
5 0
The vapor pressure of the two jars are the same.

The volume of water inside the container does not change the vapor pressure.

As long as the liquid remains being water and the temperature does not change the vapor pressure will be the same. The vapor pressure depends only in the nature of the substance and the temperature of the system.
If you want to know more about this, i.e. why, here you have additional explanation:

The vapor pressure is the pressure of the vapor of a substance in equilibrium with the substance in liquid (or solid state) and it is due to the fact that some molecules in the liquid (or solid), those that are close to the surface of liquid in contact with the gas phase and that have enough kinetic energy, evaporate.

At equilibrium the number of molecules passing from the liquid state to the gas state is equal to the number of molecules that pass from the gas state to the liquid state.  If the volume of liquid is increased or decreased, as long as the temperaature of the system remains constant the equilibrium is reached again with the same vapor pressure.


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A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 667 torr. Use Boyle's law to calculate the pres
zaharov [31]

Answer:

The pressure, when the volume is reduced to 7.88L, is 846 torr (option A)

Explanation:

Step 1: Data given

The temperature of a gas = 25.0°C

AT 25 °C the gas occupies a volume of 10.0L and a pressure of 667 torr.

The volume reduces to 7.88 L but the temperature stays constant.

Step 2: Boyle's law

(P1*V1)/T1 = (P2*V2)/T2

 ⇒ Since the temperature stays constant, we can simplify to:

P1*V1 = P2*V2

⇒ with P1 = the initial pressure 667 torr

⇒ with V1 = the initial volume = 10.0 L

⇒ with P2 = the final pressure = TO BE DETERMINED

⇒ with V2 = the final volume = 7.88L

P2 = (P1*V1)/V2

P2 = (667*10.0)/7.88

P2 = 846 torr

The pressure, when the volume is reduced to 7.88L, is 846 torr (option A)

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3 years ago
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Hope this helps you
6 0
2 years ago
A barium hydroxide solution is prepared by dissolving 2.06 g of Ba(OH)2 in water to make 32.9 mL of solution. What is the concen
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Answer:  1.36 M

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.

Molarity=\frac{n\times 1000}{V_s}

where,

n = moles of solute

To calculate the moles, we use the equation:

moles of solute= \frac{\text {given mass}}{\text {molar mass}}=\frac{2.06g}{171g/mol}=0.0120moles

Molarity=\frac{0.0120\times 1000}{32.9}=0.364M

The balanced reaction between barium hydroxide and perchloric acid:

2HCIO_4+Ba(OH_)2\rightarrow BaCIO_4+2H_2O

To calculate the concentration of acid, we use the equation given by neutralization reaction:

n_1M_1V_1=n_2M_2V_2

where,

n_1,M_1\text{ and }V_1 are the n-factor, molarity and volume of acid which is HClO_4

n_2,M_2\text{ and }V_2 are the n-factor, molarity and volume of base which is Ba(OH)_2

We are given:

n_1=1\\M_1=?\\V_1=8.50mL\\n_2=2\\M_2=0.364M\\V_2=15.9mL

Putting values in above equation, we get:

1\times M_1\times 8.50=2\times 0.364\times 15.9\\\\M_1=1.36M

Thus the concentration of the acid is 1.36 M

4 0
3 years ago
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