Answer:
a. 6 mol of oxygen
b. 10 mol of iron(III)oxide
Explanation:
Use mole concept.
Answer:
5.72 grams of O₂ are present in the sample
Explanation:
Let's calculate the moles of O₂ by the Ideal Gases Law.
P . V = n . R . T
1.66 atm . 2.50L = n . 0.082 . 283K
(1.66 atm . 2.50L) / 0.082 . 283K = n
0.179 mol = n
Molar mass O₂ = 32 g/m
Mol . molar mass = mass → 0.179 m . 32g/m = 5.72 g
Answer:
122.28346 inches, which can be rounded up to 122.29 inches.
Explanation:
Step #1: Convert to grams.
120kg × (1000g ÷ 1kg) = 120000g of copper
Step #2: Convert sample mass of copper to moles by dividing sample mass to its atomic weight. Atomic weights could be found in periodic table.
120000g Cu × (1mol Cu ÷ 63.55g Cu) = 1888.277mol Cu
Step #3: Convert moles to atoms by multiplying moles to Avogadro's number.
1888.277mol Cu × (6.022x10^23 ÷ 1mol Cu) = 1.137x10^27 atoms Cu
*I attached a picture to help out with conversions.
When there is a decrease in the pressure or an increase in volume. As the container gets bigger, it will want to increase the pressure to get back to equilibrium. For that to happen, it will have to increase the number of gas moles, and since co2 is the only has in that equation, it will increase.