Answer:
n₁ = 1.0× 10⁻⁴ mol
Explanation:
Given data:
Initial volume of balloon = 230 mL
Initial number of moles of He =?
Final number of moles of He = 3.8 × 10⁻⁴ mol
Final volume of balloon = 860 mL
Solution:
The given problem will be solve through Avogadro law,
"Number of moles of gas and volume are directly proportional to each other at constant temperature and constant pressure"
Mathematical relationship:
V₁/n₁ = V₂/n₂
No we will put the values.
230 mL /n₁ = 860 mL/ 3.8 × 10⁻⁴ mol
n₁ = 230 mL× 3.8 × 10⁻⁴ mol/ 860 mL
n₁ = 874 × 10⁻⁴ mol. mL / 860 mL
n₁ = 1.0× 10⁻⁴ mol
Answer:
3520 g of CO₂
Explanation:
2C₂H₆ + 70₂ → 4CO₂ + 6H₂O
molar ratio of the above reaction is;
2 : 7 → 4 : 6
2 moles of C₂H₆ will form 6 moles of H₂O
Thus, 1 mole of C₂H₆ will form 3 moles of H₂O
mass of H₂O = 360 g
molecular weight of H₂O = 18 g/mol
molar mass = mass ÷ molecular weight = 360÷18 = 20 moles
Total number of moles of H₂O formed = 6 * 20 moles = 120 moles
Number of moles of C₂H₆ reacted = 120 moles ÷ 3 = 40 moles
molar ratio of C₂H₆ to CO₂ = 1 : 2
Thus, number of moles of CO₂ formed = 2 * 40 moles = 80 moles
molecular weight of CO₂ = 44 g/mol
mass of CO₂ formed = number of moles x molecular weight = 80 * 44 = 3520 g
Both atoms must be non-metals,
Both atoms must have an incomplete outer energy level / shell of electrons
