There is one missing point in the question.
The formula to find an increase in boiling Temperature is :
ΔT = kb x M
ΔT = is the increase in boiling Temperature
Kb = Boiling point constant of the Solvent
M = Molarity
You did not provide the Kb. If you have it, you just have to insert it to the formula to find the ΔT.
And assuming that the other solution is water, you just have to add it up with 100 Celcius
Answer:
The correct answer is option A.
Explanation:
Equilibrium is a state when rate of forward reaction is equal to the rate of backward reaction. The concentration of reactants and products becomes constant at this state.
The ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric coefficients is termed as Equilibrium constant. It is denoted by 
.
aA + bB 
cC
![K_{eq}=\frac{[C]^c}{[A]^a[B]^b}](https://tex.z-dn.net/?f=K_%7Beq%7D%3D%5Cfrac%7B%5BC%5D%5Ec%7D%7B%5BA%5D%5Ea%5BB%5D%5Eb%7D)
The number of moles of argon that must be released in order to drop.
Solution:
Initial Temperature = 25°c = 298 K
Final Temperature =125 °c = 398 K
Initial Moles (n1) = 0.40 mole
Now, Using the ideal gas law,
n1T1 = n2T2
0.400×298 = n2 × 398
n2 = 0.299 mol
Moles of Argon released
= 0.400-0.299
= 0.100 mol.
Pressure and force are related. That is using the physical equations if you know the other, you can calculate one using pressure = force/area. This pressure can be reported in pounds per square inch, psi, or Newtons per square meter N/m2. Kinetic energy causes air molecules to move faster. They hit the walls of the container more often and with greater force. The increased pressure inside the can may exceed the strength of the can and cause an explosion.
Learn more about The temperature here:-brainly.com/question/24746268
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Answer:The boiling point of the solution is 108° C.
Explanation:
Boiling point of pure water=T=
Boiling point of water after addition of 500 g of ethylene glycol=
Mass of water = 500g = 0.5 kg (1000 g = 1 kg)
The boiling point of the solution is 108° C.
