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allochka39001 [22]
3 years ago
8

TRUE or FALSE. adding a solute like sodium chloride to water will always increase the freezing point

Chemistry
2 answers:
Afina-wow [57]3 years ago
8 0
I think that is false but don't quote me
irga5000 [103]3 years ago
4 0
It lowers the freezing point, so false.
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Are chromosomes in side the nucleus of a plant cell
Keith_Richards [23]

Answer:

Yes, chromosomes are in the nucleus of all cells that have a nucleus.

Explanation:

5 0
3 years ago
A 3.00 L flexible container holds a sample of hydrogen gas at 153 kPa. If the pressure increases to 203 kPa and the temperature
dybincka [34]

To solve this we assume that the gas is an ideal gas. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant temperature and number of moles of the gas the product of PV is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:

 

P1V1 =P2V2

V2 = P1 V1 / P2

V2 = 153 x 3.00 / 203

<span>V2 = 2.26 L</span>

3 0
3 years ago
A student makes a compound of sulfur and oxygen. She uses 5.00 g of sulfur and 4.99 g of oxygen, and all of the elemental substa
victus00 [196]
First, we apply the law of conservation of mass which states that the total mass in a system remains constant.
Therefore, there must be 5.00 g of sulfur and 4.99 g of oxygen in the product. Now, we determine the mass percentage using:

Mass % = (mass of sulfur x 100) / total mass of compound

Mass % = (5 * 100) / (5 + 4.99)

Mass % = 50.05%

The product contains 50.05% sulfur by mass.
7 0
3 years ago
Kinetic energy and gravitational potential energy are both forms of which type
scoundrel [369]

Answer:

<em>C. Potential energy</em>

Explanation:

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8 0
3 years ago
What is the mole fraction of each component if 3.9 g of benzene (C6H6) is dissolved in 4.6 g of toluene (C7H8)
Savatey [412]

Answer:

Step 1 of 6

(a)

The mass of benzene is  , so calculate the moles of benzene as follows:



The mass of toluene is, so calculate the moles of toluene as follows:



Now, calculate the mole fraction as follows:





Therefore, the mole fraction of benzene and toluene is  and  respectively.

Step 2 of 6

(b)

The formula to calculate the partial pressure is as follows:



Here,  is the partial pressure of benzene,  is the vapour pressure of pure benzene and  is the mole fraction of benzene.

Vapour pressure of pure benzene at  is.

Substitute the values in the equation as follows:



Therefore, the partial pressure is  .

Step 3 of 6

(c)

Vapor pressure of the solution at 1 atm is  .

When the total pressure of the vapour pressure of the mixture is  at a temperature, then, the solution boils. It corresponds to the boiling point of the solution.

Calculate the total pressure of the solution at  as follows:



Since, the total pressure is less than the atmospheric pressure, the solution will not boil at  .

Calculate the total pressure of the solution at  as follows:



Since, the total pressure is greater than the atmospheric pressure, the solution will boil at  .

Therefore, the boiling point of the solution is  .

Step 4 of 6

(d)

Mole fraction of benzene at  is calculated as follows:



Mole fraction of toluene at  is calculated as follows:



Therefore, the mole fractions of benzene and toluene are  and  respectively.

Step 5 of 6

(e)

Vapor pressure of benzene at  is  .

Partial pressure of benzene is calculated as follows:



Vapor pressure of toluene at  is  .

Partial pressure of toluene is calculated as follows:



Step 6 of 6

Weight composition of the vapour that is in equilibrium with the solution is calculated as follows:



Weight composition of the vapour that is in equilibrium with the solution is calculated as follows:



Explanation:

mark me as brainliest

4 0
3 years ago
Read 2 more answers
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