Oxygen can be separated by heating certain oxygen compounds by electrolysis or by liquefying air.
Answer: The number of moles in 250.0 L of He at STP is 11.0 mole.
Explanation:
- It is known that 1.0 mole of a gas at STP conditions will occupy 22.7 L.
- To show this information: STP means that T = 0.0 °C = 273.15 K and P = 1.0 kPa = (100/101.325) = 0.9869 atm.
- From the ideal gas law: PV = nRT.
- Where, P is the pressure in atm <em>(P = 1.0 atm at STP).</em>
- n is the number of moles (n = 1.0 mole).
- R is the general gas constant (R = 0.0821 L.atm/mol.K).
- T is the temperature in K (T = 273.15 K at STP).
- and now we can get the volume of 1.0 mole at STP: V = nRT/P
- V = (1.0 mole x 0.0821 L.atm/mol.K x 273.15 K) / (0.9869 atm) = 22.7 L.
- Now, we can get the number of moles of 250.0 L of He at STP:
<em>Using cross multiplication:</em>
1.0 mole → 22.7 L
??? mole → 250.0 L
- The number of moles in 250.0 L of He at STP = (250.0 L x 1.0 mole) / (22.7 L) = 11.01 mole ≅ 11.0 mole.
Answer:
In full volume it contain 0.12 moles.
Explanation:
Given data:
Total volume= Vt = 2.9 L
Decreased volume= Vd = 1.2 L
Number of moles of air present in decreased volume= n = 0.049 mol
Number of moles of air in total volume= n = ?
solution:
Formula:
Vt/ Vd = n (in total volume) /n ( decreased volume)
2.9 L / 1.2 L = X / 0.049 mol
2.42 = X / 0.049 mol
X = 2.42 × 0.049
X = 0.12 mol
Answer:
1 mole of Xe
Ne squared times of 6.02 is the greatest mass
The mole, abbreviated mol, is an SI unit which measures the number of particles in a specific substance. One mole is equal to 6.02214179×1023 atoms, or other elementary units such as molecules