Answer:
3.0 mol H₂O
Explanation:
Step 1: Write the balanced combustion equation
C₂H₆ + 3.5 O₂ ⇒ 2 CO₂ + 3 H₂O
Step 2: Establish the appropriate molar ratio
The molar ratio of C₂H₆ to H₂O is 1:3.
Step 3: Calculate the moles of H₂O formed from 1.0 mole of C₂H₆
1.0 mol C₂H₆ × 3 mol H₂O/1 mol C₂H₆ = 3.0 mol H₂O
This is key: remember it's only an ion when it transfers electrons! If it isn't going through the process of the transfer of electrons it's a neutral atom.
When The rate of effusion is inversely proportional to the √molar mass of the substance.
and we have R(He) = 1L / 4.5 min so,
R(He)/R(Cl2) = (molar mass of Cl2/ molar mass of He)^0.5
and when we have the molar mass of Cl2 = 70.9 & the molar mass of He = 4
so by substitution:
(1L/4.5 min)/ R(Cl2) = (70.9 / 4)^0.5
(1L/4.5 min) / R(Cl2) = 4.21
∴R(Cl2) = (1L/4.5 min) / 4.21 = 1L/ (4.5*4.21)min = 1 L / 18.945 min
∴Cl2 will take 18.945 min for 1 L to effuse under identical conditions
