Answer:
0.5667 M ≅ 0.57 M.
Explanation:
- It is known that the no. of millimoles of a solution before dilution is equal to the no. of millimoles of the solution after the dilution.
<em>(MV) before dilution = (MV) after dilution.</em>
M before dilution = 1.5 M, V before dilution = 340 mL.
M after dilution = ??? M, V after dilution = 340 mL + 560 mL = 900 mL.
∴<em> M after dilution = (MV) before dilution/(V) after dilution</em> = (1.5 M)(340 mL)/(900 mL) = <em>0.5667 M ≅ 0.57 M.</em>
Answer: The partial pressure of is 0.35 atm.
Explanation:
Given: Total pressure = 0.98 atm
Partial pressure of = 0.48 atm
Partial pressure of Ar = 0.15 atm
Partial pressure of = ?
Total pressure is the sum of partial pressure of each component present in a mixture of gases.
Hence, partial pressure of is calculated as follows.
Total pressure =
Substitute the values into above formula as follows.
Thus, we can conclude that the partial pressure of is 0.35 atm.
I think the answer would be A because O is oxygen and it has 7. Although it’s in parentheses and has a 2 on the outside of those parentheses, so you would multiply and 7 x 2 = 14. 14 is larger than the other ones.
Hopefully I’m right and hopefully that helps.
Answer:
Explanation:
The atomic mass of <em>nickel</em> is 58.963g/mol. Thus, one mole of nickel weighs "exactly" 58.693g.
How much nickel does every coin contain?
How many times 58.693g contains 1.25g?
That means that you need to have 47 coins of nickel to have one mole of nickel.