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Grace [21]
3 years ago
7

Determine the boiling point of a solution made by dissolving 0.60 mol K2SO4 in 1.0 kg water. Water has a boiling point elevation

constant of 0.51°C•kg/mol. What is the boiling point of this solution?

Chemistry
2 answers:
Semmy [17]3 years ago
8 0

<em>Answer: </em>

1) -65.9

2) 100.31

<em> Explanation: edg 2020</em>

<em></em>

MissTica3 years ago
5 0
To determine the boiling point (bp), you need this formula---> bp solution= bp solvent + Δbp solution

bp solvent is known since we are dealing with water; it is 100C

all we have to do is to solve for Δbp solution and add it to the 100C. 

Δbp solution= Kb x i x m, where Kb is the constant, i is the number of particles and m is molality. 

Kb= 0.51 
i= 3, K2SO4 ----> 2K+ + SO4-2 (the solute breaks into three ions)
m= ? = moles/kg of solvent

molality (m)= 0.60 mol/ 1.0 Kg= 0.60 m

Δbp solution= 0.51 x 3 x 0.60= 0.918 C

bp solution= 100C + 0.918 C= 100.918 C
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katovenus [111]

Answer:

No

Explanation:

No, his mass remains the same no matter where he is in the universe.

But then again the moon has less gravitational pull, therefore your weight and mass will be smaller in space and on the moon than on earth

I hope this was helpful! ;)

3 0
3 years ago
At 35.0°c and 3.00 atm pressure, a gas has a volume of 1.40 l. what pressure does the gas have at 0.00°c and a volume of 0.950 l
Leona [35]

Answer : The pressure of gas will be, 3.918 atm and the combined gas law is used for this problem.

Solution :

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}

where,

P_1 = initial pressure of gas = 3 atm

P_2 = final pressure of gas = ?

V_1 = initial volume of gas = 1.40 L

V_2 = final volume of gas = 0.950 L

T_1 = initial temperature of gas = 35^oC=273+35=308K

T_2 = final temperature of gas = 0^oC=273+0=273K

Now put all the given values in the above equation, we get the final pressure of gas.

\frac{3atm\times 1.40L}{308K}=\frac{P_2\times 0.950L}{273K}

P_2=3.918atm

Therefore, the pressure of gas will be, 3.918 atm and the combined gas law is used for this problem.

4 0
3 years ago
Read 2 more answers
Consider this equilibrium reaction between carbon monoxide and hydrogen gas, occurring in a sealed flexible container. CO(g) + 3
wariber [46]

Answer:

More H2(g) is added to the container : <u>Towards products.</u>

CO is removed from the container : <u>Towards reactants.</u>

More CH4(g) is added to the container : <u>Towards reactants</u>

H2O(g) is removed from the container <u>: Towards products.</u>

The contents of the container are heated up. :<u> Towards the reactants.</u>

The contents of the container are cooled down : <u>Towards the products.</u>

The pressure inside the container is increased. :<u>Towards the products</u>

The container is stretched to increase the volume: <u>Towards the reactants.</u>

Explanation: :

CO(g) + 3 H2g) → CH4(g) + H2O(g)+ heat

There is released heat, so this reaction is exothermic

If the H2 concentration is increased, the system will try to change the concentration change by shifting the balance to the right, and thus the concentration of products will increase.<u> Towards products.</u>

If the CO is removed, the system will try to change this situation by shifting the balance to the left, and thus the concentration of reactants will increase, the concentration of products will decrease. <u>Towards reactants.</u>

If the CH4 concentration is increased, the system will try to change the concentration change by shifting the balance to the left, and thus the concentration of reactants will increase. <u>Towards reactants</u>

If the H2O is removed, the system will try to change this situation by shifting the balance to the right, and thus the concentration of products will increase, the concentration of products will decrease. <u>Towards products.</u>

If the temperature is increased, the system will reduce the amount of heat released. So the balance will shift to the left. <u>Towards the reactants.</u>

This because the extra heat / energy must be used.

If the temperature is decreased, the system will produce more heat  So the balance will shift to the right. <u>Towards the products.</u>

This because more heat /energy needs to be produced to make up for the loss of heat (energy).

If the pressure is increased, the system will shift to the side with fewer moles of gas. In this case, there are 4 moles on the left and 2 moles on the right.  So the balance will shift to the right. <u>Towards the products.</u> An increase of pressure has the same effect on the equilibrium as a decrease of the volume.

If the volume is increased, this means the pressure is decreased, the system will shift to the side with most moles of gas. In this case, there are 4 moles on the left and 2 moles on the right.  So the balance will shift to the left. <u>Towards the reactants.</u> An increase of volume has the same effect on the equilibrium as a decrease of the pressure.

6 0
3 years ago
Which two minerals make up the complex hydroxyapatite?
matrenka [14]
Ca₁₀(PO₄)₆(OH)₂ - hydroxyapatite

b. phosphorus (P) and calcium (Ca)
6 0
2 years ago
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During which stage of life is a human most dependent on others?
AfilCa [17]

Erm, I think when they are little. When they are just born.

7 0
2 years ago
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