Answer:
74.1%
Explanation:
Based on the reaction:
S₈ + 16F₂ → 8SF₄
1 mole of sulfur reacts with 16 moles of Fâ‚‚ to produce 8 moles of SFâ‚„
To solve this question we must find the moles of each reactant in order to find the moles of SFâ‚„. Thus, we can find the theoretical mass produced. Percent yield is:
Percent yield = Actual yield (25.0g) / Theoretical yield * 100
Moles S₈: 256.52g/mol
10.0g * (1mol / 256.52g) = 0.0390 moles
Moles Fâ‚‚:
PV = nRT
PV/RT = n
Where P is pressure in atm, V is volume in liters, R is gas constant and T is absolute temperature (0°C = 273.15K)
2.69atm*5.00L / 0.082atmL/molK*273.15K = n
0.600 moles = n
For a complete reaction of 0.600 moles Fâ‚‚ are required:
0.600mol F₂ * (1mol S₈ / 8 mol F₂) = 0.075 moles S₈
As there are just 0.0390 moles, S₈ is limiting reactant.
The theoretical moles and mass of SFâ‚„ -Molar mass: 108.07g/mol- is:
0.0390 moles S₈ * (8mol SF₄ / 1mol S₈) = 0.312 moles SF₄ * (108.07g) =
33.7g
Percent yield = 25.0g / 33.7g * 100
= 74.1%
