The _HIGHER__ vapor pressure at high altitudes causes a liquid to boil at a _LOWER___ temperature.
Explanation:
Vapor pressure is the pressure applied by the molecule of a liquid at the surface of the liquid as it transitions into a gaseous phase. When the vapor pressure exceeds the atmospheric pressure, this is when the liquid begins to boil. Therefore when the atmospheric pressure is low, then the liquid will boil at lower temperatures, because the vapor pressure of the liquid will overcome the atmospheric pressure at lower temperatures.
Answer:
Ok so, I think I have it, but it might not be right, but 16 grams of oxygen
Explanation:
2H+O=H2O
36gH2O x 1mol/18g(molar mass of water)= 2 moles of water
20 grams of H2 x 1/2= 10 moles of H2
2 moles of H2 react with 1 mole of O2 to produce 2 moles of water, so...
1 mole O2 x 16g/mole = 16 g O2
The answer should be C. I dont know know if you have misspellings or not
I think it's A but it might be different from your school and mine
Answer: Option (b) is the correct answer.
Explanation:
Buffere is defined as the solution to whom when an acid or base is added then it resists any in change in pH of the solution.
This is because a buffer has the ability to not get affected by the addition of small amounts of an acid or a base. So, basically it keeps the concentration of both hydrogen ions and hydroxides equal. As a result, it helps in maintaining the pH of the solution.
And, the capacity of a buffer solution to resist the change is known as buffer capacity.
Thus, we can conclude that buffering capacity refers to the extent to which a buffer solution can counteract the effect of added acid or base.