The answer is 1.6 atm. Let's first calculate the mole fraction of gas Y.
The mole fraction (x) is: x = n1/n, where n1 is a number of moles of an
individual gas in a mixture and n is total moles of the gas mixture. We
know that n1 of gas Y is 6.0 mol (n1 = 6.0 mol) and that there are in
total 8. mol of the gas mixture (n = 2.0 + 6.0 = 8.0 mol). Now calculate
the mole fraction of gas Y. x = 6.0/8.0 = 0.75. Now, let's use the mole
fraction of gas Y (x) and the total pressure (P) to calculate the
partial pressure of gas Y (P1): x = P1/P. P1 = x * P. If x = 0.75 and P =
2.1 atm, then the partial pressure of gas Y is: P1 = 0.75 * 2.1 atm =
1.6 atm.
Answer: The pressure of the He is 2.97 atm
Explanation:
According to Dalton's law, the total pressure is the sum of individual pressures.
Given : 
=total pressure of gases = 6.50 atm
= partial pressure of Nitrogen = 1.23 atm
= partial pressure of oxygen = 2.3 atm
= partial pressure of Helium = ?
putting in the values we get:
The pressure of the He is 2.97 atm
Answer:
Explanation:
Metal is a material in the periodic table s much as iron or gold. A non metal is carbon in diamonds and graphite for pencil lead.
Answer:
10.80
Explanation:
As per the equation, let us calculate the mole ratio. N2+3H2→2NH3. As per the equation one mole of nitrogen reacts with 1 mol of hydrogen.
In terms of mass. 28.01 g of nitrogen needs 3 mol of hydrogen or 6.048 g of hydrogen.
We can set up the ratio;
28.01 g of
l
N
2
needs
6.048 g of
l
H
2
1 g of
l
N
2
needs
6.048
28.01
g of
l
H
2
50.0 g of
l
N
2
needs
6.048
×
50.0
28.01
l
g of
l
H
2
=
10.80 g of
l
H
2
