If you collect 1.75 L of hydrogen gas during a lab experiment when the room temperature is 23oC and the barometric pressure is 1
1 answer:
Answer:
Explanation:
Hello,
In this case, since we can consider hydrogen gas as an ideal gas, we check the volume-pressure-temperature-mole relationship by using the ideal gas equation:
Whereas we are asked to compute the moles given the temperature in Kelvins, thr pressure in atm and volume in L as shown below:
Best regards.
You might be interested in
Answer:
Explanation:
Hello!
In this case, since the by-mass percent of a solution is a measure of the mass of the solute over the mass of the solution:
As we know the mass of the solution and the by-mass percent, we can compute the mass of glucose in the 480 g of solution:
Thus, by plugging in the data, we obtain:
Finally, since the solution is made up of glucose and water, we compute the mass of water as follows:
Best regards!
Answer:
Approximately .
Explanation:
Lookup Avogadro's Number: (three significant figures.)
Lookup the relative atomic mass of ,
, and
on a modern periodic table:
:
.
:
.
:
.
(For example, the relative atomic mass of is
means that the mass of one mole of
atoms would be approximately
grams on average.)
The question counted the number of molecules without using any unit. Avogadro's Number
helps convert the unit of that count to moles.
Each mole of molecules includes exactly
of these
molecules.
molecules would correspond to
of such molecules.
(Keep more significant figures than required during intermediary steps.)
The formula mass of gives the mass of each mole of
molecules. The value of the formula mass could be calculated using the relative atomic mass of each element:
.
Calculate the mass of approximately of
:
.
(Rounded to three significant figures.)