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