Answer:
I think this is it. and 38 points??
Answer:
Gaseous at standard conditions.
Explanation:
Hello,
In this case, for the given normal boiling point of oxygen, we can notice those are conditions far away from the standard conditions which are 25 °C. In such a way, since the standard temperature is by far higher than the normal boiling point, the most likely state of a sample of pure oxygen would be gaseous since the molecules will move based on the kinetic theory of gases due to the relatively high temperature which make them be separated and moving all around.
Best regards.
The Charles law explains that "volume of an ideal gas at constant pressure is directly proportional to the absolute temperature."
Answer:
28.58 g of NaOH
Explanation:
The question is incomplete. The missing part is:
<em>"Calculate the mass of sodium hydroxide that the chemist must weigh out in the second step"</em>
To do this, we need to know how much of the base we have to weight to prepare this solution.
First we know that is a sodium hydroxide aqueous solution so, this will dissociate in the ions:
NaOH -------> Na⁺ + OH⁻
As NaOH is a strong base, it will dissociate completely in solution, so, starting with the pH we need to calculate the concentration of OH⁻.
This can be done with the following expression:
14 = pH + pOH
and pOH = -log[OH⁻]
So all we have to do is solve for pOH and then, [OH⁻]. To get the pOH:
pOH = 14 - 13.9 = 0.10
[OH⁻] = 10⁽⁻⁰°¹⁰⁾
[OH⁻] = 0.794 M
Now that we have the concentration, let's calculate the moles that needs to be in the 900 mL:
n = M * V
n = 0.794 * 0.9
n = 0.7146 moles
Finally, to get the mass that need to be weighted, we need to molecular mass of NaOH which is 39.997 g/mol so the mass:
m = 39.997 * 0.7146
<h2>
m = 28.58 g</h2>
Rift/Mid-Ocean Ridge.
Magma eventually comes up and creates new ocean floor
