The molarity of the solution will be 3.45 M
<h3>Further explanation
</h3>
Dilution is the process of adding a solvent to get a more dilute solution.
The moles(n) before and after dilution are the same.
Can be formulated :
M₁V₁=M₂V₂
M₁ = Molarity of the solution before dilution
V₁ = volume of the solution before dilution
M₂ = Molarity of the solution after dilution
V₂ = Molarity volume of the solution after dilution
The initial solution
345 mL of a 2.5 M NaCl solution.
M₁=2.5 M
V₁=345 ml
The solution after boiled :
V₂=250 ml
Answer:
<h2>volume = 3.63 mL</h2>
Explanation:
The density of a substance can be found by using the formula
<h3>
</h3>
Since we are finding the volume
Making volume the subject we have
<h3>
</h3>
From the question
mass = 63.6 g
Density = 17.5 g/mL
Substitute the values into the above formula and solve for the volume
That's
<h3>
</h3>
We have the final answer as
<h3>volume = 3.63 mL</h3>
Hope this helps you
Answer:
* Beryllium is the lightest of all the alkaline earth metals.
* It has higher melting and boiling points compared to other elements in group 2.
Explanation:
<em>I</em><em> </em><em>hope</em><em> </em><em>it</em><em> </em><em>helps</em><em> </em><em>></em><em>~</em><em><</em>
Kinetic energy = 1/2mv²
where m = 54kg
and v =3m/s
k.e = 1/2×54×3×3
= 1/2×54×9
= 1/2×426
= 486÷2
= 243J
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Answer:
20 moles
Explanation:
The important thing to realize here is that you're working under STP conditions, which implies that you can use the molar volume of a gas at STP to find how many moles of helium will occupy that volume.
Now, the molar volume of a gas represents the volume occupied by one mole of a gas under some specific conditions for pressure and temperature.
Starting from the ideal gas law equation
PV=nRT
you can say that the molar volume of gas at a pressure P and a temperature T will be equal to
Vn=RTP
Now, Standard Temperature and Pressureconditions are defined as a pressure of 100 kPaand a temperature of 0∘C. Under these specific conditions, the molar volume of a gas will be equal to
Vn=0.0821⋅atm⋅Lmol⋅K⋅(273.15+0)K100101.325atm
Vn=22.7 L/mol
This of course implies that one mole of any ideal gas will occupy 22.7 L.
In your case, the volume of the gas is said to be equal to 500 L. This means that you will have
500L⋅1 mole He22.7L=22.026 moles He
Rounded to one sig fig, the number of sig figs you have for the volume of the gas, the answer will be
nHe=20 moles
SIDE NOTE Many textbooks and online sources still list STP conditions as a pressure of 1 atmand a temperature of 0∘C.
Under these conditions for pressure and temperature, one mole of any ideal gas occupies 22.4 L. If these are the values for STP given to you by your instructor, make sure to redo the calculations using 22.4 L instead of 22.7 L
