Sorry, Cant really tell how to differentiate the students and trial times
<span>The instructor should be questioned to see if the filtrate is able to be recycled. This precipitate can contaminate the filtrate, rendering it useless for repeated experiments. If it is able to be recycled, a second pass through the filter might be required to remove the precipitate.</span>
Answer : The partial pressure of nitrogen gas is, 2.94 atm
Explanation:
According top the Henry's Law, the concentration of a gas in a liquid is directly proportional to the partial pressure of the gas.
is Henry's constant.
or,
where,
= initial concentration of gas = 
= final concentration of gas = 
= initial partial pressure of gas = 0.78 atm
= final partial pressure of gas = ?
Now put all the given values in the above formula, we get the final partial pressure of the gas.
Therefore, the partial pressure of nitrogen gas is, 2.94 atm
When the concentration is expressed in molality, it is expressed in moles of solute per kilogram of solvent. Since we are given the mass of the solvent, which is water, we can compute for the moles of solute NaNO3.
0.5 m = x mol NaNO3/0.5 kg water
x = 0.25 mol NaNO3
Since the molar mass of NaNO3 is 85 g/mol, the mass is
0.25 mol * 85 g/mol = 21.25 grams NaNO3 needed
Hello!
To find the amount of atoms that are in 80.45 grams of magnesium, we will need to know Avogadro's number and the mass of one mole of magnesium.
Avogadro's number is 6.02 x 10^23 atoms, and one mole of magnesium is equal to 24.31 grams.
1. Divide by one mole of magnesium
80.45 / 24.31 = 3.309 moles (rounded to the number of sigfigs)
2. Multiply moles by Avogadro's number
3.309 x (6.02 x 10^23) = 1.99 x 10^24 (rounded to the number of sigfigs)
Therefore, there are 1.99 x 10^24 atoms in 80.45 grams of magnesium.
