Answer:
Percent yield = 61.5%
Explanation:
Given data:
Moles of hydrogen = 2.00 mol
Actual yield of ammonia= 0.80 mol
Percent yield = ?
Solution:
Chemical equation:
3H₂ + N₂ → 2NH₃
Now we will compare the moles of ammonia with hydrogen from balance chemical equation:
H₂ : NH₃
3 : 2
2 : 2/3×2 = 1.3 mol
Percent yield:
Percent yield = Actual yield / theoretical yield × 100
Percent yield = 0.80 mol /1.3 mol × 100
Percent yield = 0.615 × 100
Percent yield = 61.5%
<span>moles glucose = 19 g / 180 g/mol= 0.105
M = 0.105 / 0.100 L = 1.05
moles in 20.0 mL = 1.05 M x 0.0200 L = 0.0216
New concentration = 0.0216 /0.500 L = 0.0432 M
moles in 100 mL = 0.100 L x 0.0432 = 0.00432
mass = 0.00432 x 180 g/mol= 0.778 g</span>
Answer:
d. Pressure
Explanation:
Pressure is not a factor which affect rates of reaction.
However, surface area, temperature, and concentration are factors that affect rates of reaction.
The answer is K3PO4(s) → 3K+(aq) + PO43–(aq) since water-soluble ionic tripotassium phosphate dissociates completely into K+ and PO43– ions when dissolved, that is, no K3PO4 remains in the solution. Carbonic acid H2CO3 and acetic acid CH3COOH are weak electrolytes since they are weak acids that do not completely ionize, while nonelectrolyte CH3OH do not dissociate into ions.
