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DanielleElmas [232]
2 years ago
9

which process describe water changing from a liquid state to a gas? condensation evaporation infiltration precipitation

Chemistry
2 answers:
Bogdan [553]2 years ago
8 0
<span>evaporation  is the process that describe changing of water from liquid to gas</span>
ValentinkaMS [17]2 years ago
8 0

Answer: Option (b) is the correct answer.

Explanation:

When we heat a liquid substance then its molecules gain kinetic energy due to which more number of collisions occur between the particles. As a result, liquid state of substance will change into gaseous state.

This process of conversion of liquid into gaseous phase is known as evaporation.

Whereas when gaseous phase changes into liquid state then there occurs decrease in kinetic energy of molecules of a substance. Due to which they change into liquid state. This process is known as condensation.

When two aqueous solution react chemically with each other then an insoluble solid formation into the solution is known as precipitate. This type of reaction is known as precipitation.

When water present on the surface of earth enters into the soil then it is known as infiltration.

Therefore, we can conclude that evaporation process describe water changing from a liquid state to a gas.

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More than one atom

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Which of the following systems has the highest entropy?. . . A cup of ice at 0 degrees C. . A cup of water at 50 degrees C. . A
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Entropy is a measure of chaos or disorder in a system. For the first one, the system with the highest entropy is a cup of water at 0 degress centigrade.  For the second question, the system with the lowest entropy is  sugar crystals in 95 degrees centigrade cup of coffee. 
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Calculate the ph of a buffer that is 0.225 m hc2h3o2 and 0.162 m kc2h3o2. the ka for hc2h3o2 is 1.8 Ã 10-5. 4.60 9.26 4.74 4.89
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Answer:

The pH of the buffer solution is 4.60.

Explanation:

Concentration of acid = [HC_2H_3O_2]=0.225 M

Concentration of salt = [KC_2H_3O_2]=0.162 M

Dissociation constant = K_a=1.8 \times 10^{-5}

The pH of the buffer can be determined by Henderson-Hasselbalch equation:

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

pH=-\log[1.8 \times 10^{-5}]+\log\frac{0.162 M}{0.225 M}

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The pH of the buffer solution is 4.60.

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Instrument for measuring the basic units​
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4 0
3 years ago
A helium balloon with a volume of 550mL is cooled from 305 to 265K. The pressure on the gas is reduced from 0.45 atm to 0.25 atm
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860 mL.

<h3>Explanation</h3>

Separate this process into two steps:

  1. Cool the balloon from 305 K to 265 K.
  2. Reduce the pressure on the balloon from 0.45 atm to 0.25 atm.

What would be the volume of the balloon after each step?

After Cooling the balloon at constant pressure:

By Charles's Law, the volume of a gas is directly related to its temperature in degrees Kelvins.

In other words,

\dfrac{V_2}{V_1} = \dfrac{T_2}{T_1},

where

  • V_1 and V_2 are volumes of the same gas.
  • T_1 and T_2 are the temperatures (in degrees Kelvins) of that gas.

Rearranging,

V_2 = V_1 \cdot \dfrac{T_2}{T_1}\\\phantom{V_2} = 550 \times \dfrac{265}{305}\\\phantom{V_2} = 478 \; \text{mL}.

The balloon ended up with a lower temperature. As a result, its volume drops: V_2 < V_1.

After reducing the pressure on the balloon at constant temperature:

By Boyle's Law, the volume of a gas is inversely proportional to the pressure on this gas.

In other words,

\dfrac{V_2}{V_1} = \dfrac{P_1}{P_2},

where

  • V_1 and V_2 are volumes of the same gas.
  • P_1 and P_2 are the pressures on this gas.

Rearranging,

V_2 = V_1 \cdot \dfrac{P_1}{P_2}\\\phantom{V_2} = 478 \times \dfrac{0.45}{0.25}\\\phantom{V_2} = 860 \;\text{mL}.

There's now less pressure on the balloon. As a result, the balloon will gain in volume: V_2 > V_1.

The final volume of the balloon will be 860 \; \text{mL}.

7 0
3 years ago
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