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djverab [1.8K]
3 years ago
11

As the organsims develops, its cells become -------

Chemistry
1 answer:
exis [7]3 years ago
3 0
It's cells become larger in numbers.
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When humans burn fossil fuels, most of the the carbon quickly enters the atmosphere as carbon dioxide in the atmosphere in the p
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Transpiration i think
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3 years ago
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If the container is closed and the ethanol is allowed to reach equilibrium with its vapor, how many grams of liquid ethanol rema
SVETLANKA909090 [29]

Explanation:

Let us assume that the given data is as follows.

        V = 3.10 L,        T = 19^{o}C = (19 + 273)K = 292 K

       P = 40 torr    (1 atm = 760 torr)

So,     P = \frac{40 torr}{760 torr} \times 1 atm

             = 0.053 atm

          n = ?

According to the ideal gas equation, PV = nRT.

Putting the given values into the above equation to calculate the value of n as follows.

                 PV = nRT

   0.053 atm \times 3.10 L = n \times 0.0821 L atm/mol K \times 292 K

                 0.1643 = n \times 23.97

                    n = 6.85 \times 10^{-3}

It is known that molar mass of ethanol is 46 g/mol. Hence, calculate its mass as follows.

               No. of moles = \frac{mass}{\text{molar mass}}

                 6.85 \times 10^{-3} = \frac{mass}{46 g/mol}  

                    mass = 315.1 \times 10^{-3} g

                              = 0.315 g

Thus, we can conclude that the mass of liquid ethanol is 0.315 g.

4 0
3 years ago
PLEASE HELP When I combine Sprite with a sour candy, it starts to bubble a lot. Is this a physical or chemical change?
maksim [4K]

Answer:

B. chemical

Explanation:

Chemical change cannot go back to its original form

4 0
2 years ago
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12. The vapor pressure of water at 90°C is 0.692 atm. What is the vapor pressure (in atm) of a solution made by dissolving 3.68
luda_lava [24]

Answer : The vapor pressure (in atm) of a solution is, 0.679 atm

Explanation : Given,

Mass of H_2O = 1.00 kg = 1000 g

Moles of CsF = 3.68 mole

Molar mass of H_2O = 18 g/mole

Vapor pressure of water = 0.692 atm

First we have to calculate the moles of H_2O.

\text{Moles of }H_2O=\frac{\text{Mass of }H_2O}{\text{Molar mass of }H_2O}=\frac{1000g}{18g/mole}=55.55mole

Now we have to calculate the mole fraction of H_2O

\text{Mole fraction of }H_2O=\frac{\text{Moles of }H_2O}{\text{Moles of }H_2O+\text{Moles of }CsF}=\frac{55.55}{55.55+3.68}=0.938

Now we have to partial pressure of solution.

According to the Raoult's law,

P_{Solution}=X_{H_2O}\times P^o_{H_2O}

where,

P_{Solution} = vapor pressure of solution

P^o_{H_2O} = vapor pressure of water = 0.692 atm

X_{H_2O} = mole fraction of water = 0.938

P_{Solution}=X_{H_2O}\times P^o_{H_2O}

P_{Solution}=0.938\times 0.692atm

P_{Solution}=0.649atm

Therefore, the vapor pressure (in atm) of a solution is, 0.679 atm

5 0
2 years ago
PLEASE HELP
HACTEHA [7]
Not sure gets hotter prolly
5 0
2 years ago
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