The correct option is:
The latent heat of vaporization of water is given by option D. 22,590J
Latent heat of vaporization:
Latent heat of vaporization is energy required to change 1 kg of liquid to gas at atmospheric pressure at its boiling point.
Also, Latent heat is the energy released or absorbed during a phase change.
Energy released during phase change is Exothermic process.
Whereas energy absorbed during phase change is Endothermic process.
Q=mL
Q= Latent heat
m= mass= 10 g
L= Latent heat of vaporization= 2,259 J/g
Putting the values in the above equation:
Q=10*2259
Q=22590 L
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Answer:
5 moles of Argon is present in the mixture.
Explanation:
Total pressure of the gaseous mixture = 4 atm
Total number of moles = 16
Partial pressure of Ne = 2.75 atm
By Dalton's law of partial pressure, the total pressure of gaseous mixture is the sum of partial pressures of individual gases which are non-reactive.
Hence:
Also :
Partial pressure = mole fraction*total pressure
∴Number of moles of Argon = 5
Answer:
No because it changes velocity, instead of accelerating
Explanation:
and yes, I am in K12 ツ
Answer:
2.06 atm
Explanation:
The computation of the pressure inside the flask is shown below;
As per the ideal gas law
we know that
P V = nRT
where
V = 1.50L
T = 325 K
R = 0.0821
Now moles of N_2 is
= 3.25 ÷ 28
= 0.116 mol
Now
P = NRT ÷ V
= 0.116 × 0.0821 × 325 ÷ 1.50
= 2.06 atm
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