Answer:
13.4 (w/w)% of CaCl₂ in the mixture
Explanation:
All the Cl⁻ that comes from CaCl₂ (Calcium chloride) will be precipitate in presence of AgNO₃ as AgCl.
To solve this problem we must find the moles of AgCl = Moles of Cl⁻. As 2 moles of Cl⁻ are in 1 mole of CaCl₂ we can find the moles of CaCl₂ and its mass in order to find mass percent of calcium chloride in the original mixture.
<em>Moles AgCl - Molar mass: 143.32g/mol -:</em>
0.535g * (1mol / 143.32g) = 3.733x10⁻³ moles AgCl = Moles Cl⁻
<em>Moles CaCl₂:</em>
3.733x10⁻³ moles Cl⁻ * (1mol CaCl₂ / 2mol Cl⁻) = 1.866x10⁻³ moles CaCl₂
<em>Mass CaCl₂ -Molar mass: 110.98g/mol-:</em>
1.866x10⁻³ moles CaCl₂ * (110.98g/mol) = 0.207g of CaCl₂ in the mixture
That means mass percent of CaCl₂ is:
0.207g CaCl₂ / 1.55g * 100 =
<h3>13.4 (w/w)% of CaCl₂ in the mixture</h3>
The answer is 2 hope it helps
Answer:
k' = (2.0345 × 10⁻⁸) M/s.
Explanation:
Beer-Lambert's law explains that Absorbance is directly proportional to the concentration of the substrate under consideration.
A ∝c
A = εlc
where ε = molar absorptivity constant = 87,000 M⁻¹cm⁻¹
l = path length of the solution that the light passes through in cm = 1 cm for most cases.
c = concentration of the substrate.
In terms of rate terms,
A' = εlc'
where A' has units of Absorbance/s
c' = rate of reaction, units of concentration/s
A' = εlc'
From the graph, the slope of the graph = 0.00177 Absorbance/s
0.00177 = 87000 × 1 × c'
c' = (0.00177/87000)
c' = (2.0345 × 10⁻⁸) M/s.
This value is the pseudo rate constant, k'.
Hope this Helps!!!