Answer:
P=9
Explanation:
Formula: P = M/V
First, we need to find the volume. This can be done by: 5 x 3 x 2 which will give us 30
Now we can plug it in
P= 270/30
P=9!
<span>Collisions between gas particles are inelastic. - A
The collisions in a gas are assumed to be perfectly elastic
</span>
Answer:
1.86% NH₃
Explanation:
The reaction that takes place is:
- HCl(aq) + NH₃(aq) → NH₄Cl(aq)
We <u>calculate the moles of HCl that reacted</u>, using the volume used and the concentration:
- 32.27 mL ⇒ 32.27/1000 = 0.03227 L
- 0.1080 M * 0.03227 L = 3.4852x10⁻³ mol HCl
The moles of HCl are equal to the moles of NH₃, so now we <u>calculate the mass of NH₃ that was titrated</u>, using its molecular weight:
- 3.4852x10⁻³ mol NH₃ * 17 g/mol = 0.0592 g NH₃
The weight percent NH₃ in the aliquot (and thus in the diluted sample) is:
- 0.0592 / 12.949 * 100% = 0.4575%
Now we <u>calculate the total mass of NH₃ in the diluted sample</u>:
Diluted sample total mass = Aqueous waste Mass + Water mass = 23.495 + 72.311 = 95.806 g
- 0.4575% * 95.806 g = 0.4383 g NH₃
Finally we calculate the weight percent NH₃ in the original sample of aqueous waste:
- 0.4383 g NH₃ / 23.495 g * 100% = 1.86% NH₃
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%
