You have 0.50 mol of NH3 and 0.20 mol of NH4+ to start (NH4Cl dissolves completely), given the molarity and 1.0 L solution.
30.0 mL of 1.0 M HCl is 0.0300 mol of HCl. This will react with the NH3 to produced 0.030 mol of NH4+.
You now have 0.47 mol NH3 and 0.23 mol NH4+. Now use the Henderson-Hasselbach equation to calculate your pH. The equation says to use concentration of acid and base, but you can just use the moles of them because it doesn’t make a difference.
pH = pKa + log(base/acid)
pKa = 14 - pKb = 14 - 4.75 = 9.25
pH = 9.25 + log(0.47/0.23) = 9.56
Answer:
a
Explanation:
because I said so and I think it's right
Answer:
E = 19.89 × 10⁻¹³ J
Explanation:
Given data:
Wavelength of gamma ray= 1.0× 10⁻¹³ m
Energy of gamma ray = ?
Solution:
Formula:
E = h c/λ
h = plancks constant = 6.63× 10⁻³⁴ js
c = speed of light = 3 ×10⁸ m/s
by putting values,
E = 6.63× 10⁻³⁴ js × 3 ×10⁸ m/s /1.0× 10⁻¹³ m
E = 19.89 × 10⁻²⁶ J.m/ 1.0× 10⁻¹³ m
E = 19.89 × 10⁻¹³ J
Answer:
71.8%
Explanation:
The percent yield of a process or a chemical reaction is calculated as:
percent yield = actual yield/theoretical yield x 100%
From the problem we have:
theoretical yield = 3.9 kg
actual yield = 2.8 kg
Thus, we calculate the yield of H₂SO₄ production as follows:
percent yield = (2.8 kg/3.9 kg) x 100 = 71.79 % ≅ 71.8%
Answer:
<u><em>100N</em></u>
Explanation:
<u>Given</u> <u>Required</u>
Effort force = 50N Force applied to a resistance = ??
Ideal Mechanical Advantage (IMA) = 2
<u>Solution</u>
Force applied to a resistance = Effort force x Ideal Mechanical Advantage (IMA)
= 50N x 2
= 100N
