This problem can be solved by Dalton's law of partial pressures which states that <em>in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases</em>.
Ptotal = P₁ + P₂ + P₃ + ..... + Pn
Herein, Ptotal = P(Ne) + P(Ar) + P(He)
Ptotal = 1.25 atm, P(Ne) = 0.68 atm and P(Ar) = 0.35
So, P(He) = Ptotal - P(Ne) - P(Ar) = 1.25 - 0.68 - 0.35 = 0.22 atm
Answer is: 2065.15 kJ.
Balanced chemical reaction: 4NH₃ + 5O₂ → 4NO + 6H₂O<span>, ΔHrxn=−906 kJ.
m(</span>NH₃) = 155 g.
n(NH₃) = m(NH₃) ÷ M(NH₃).
n(NH₃) = 155 g ÷ 17 g/mol.
n(NH₃) = 9.118 mol.
Make proportion: 4 mol(NH₃) : 906 kJ = 9.118 mol : Q.
Q = 906 kJ · 9.118 mol / 4 mol.
Q = 2065.15 kJ.
Factor that can be controlled changed or measured in an experiment.
Closest to Mg: Neon Must lose 2 electrons?
Closest to S: Argon Must gain 2 electrons?
I know the noble gases are right, but I'm not 100% sure if you just need to add/subtract electrons.
Alex earns $400 per week.
He gets $150 per car (x).
"x" is the number of cars Alex has sold.
400 + 150x
If he earned $1450 last week, then
400 + 150x = 1450
First, you subtract 400 from both sides.
150x = 1050
Then divide both sides by 150.
x = 7
Therefore, Alex sold 7 cars last week.
hope this helps!