941539.2 g of mass of oxygen is produced when 2000 kg of aluminium oxide is completely electrolysed.
<h3>What is electrolysis?</h3>
Electrolysis is the process by which electric current is passed through a substance to effect a chemical change.
The mass of aluminium oxide Al₂O₃ = 2000 kg = 2000 000 g
Molar mass of Al₂O₃ = 101.96 g/mol
no of moles = 
no of moles of Al₂O₃ = 
no of moles of Al₂O₃ = 19615.4 mol
From the reaction:
4Al + 3O₂ ⇒ Al₂O₃
To determine the moles of O₂ in Al₂O₃:
Then;
19615.4 mol X 
mol of O₂ = 29423.1
The mass of oxygen now = 29423.1 × 32 g
= 941539.2 g
Hence, 941539.2 g of mass of oxygen is produced when 2000 kg of aluminium oxide is completely electrolysed.
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Answer:
1.3 M
Explanation:
The question asks to calculate the molarity of a solution.
We have to use the following equitation:
Molarity = # moles / 1 lt of solution
In this case we have a solution composed of 0.65 mol of NaF diluted in a total volume of 0.5 lt. We will have to do the following cross multiplication solving for x:
0.65 mol NaF / 0.5 lt = x mol NaF/ 1 lt
x = 1.3 mol NaF / 1 lt = 1.3 M
Answer:
4s2
Explanation:
The electronic configuration of zinc in the ground state of the atom is 1s22s22p6 3s23p63d104s2. It can be written in a condensed form by showing the inert gas core as follows; [Ar] 3d¹⁰ 4s².
Zinc has a pseudo inert gas configuration when the 4s electrons are removed during oxidation. Hence this sublevel is usually affected when zinc atoms are oxidized according to the scheme;
Zn---->Zn^2+ + 2e-
Answer:
a. 10.54
Explanation:
reaction is
NH₃ + NaOH -----------------NH₄Cl + H₂O
0.10 mol NaOH will consume 0.10 mol NH₃ thereby decreasing the initial amount of moles NH₃ and increasing that of NH₄Cl
mol NH₃ = 0.80 - 010 = .70
mol NH₄Cl = 0.80 + .10 = 0.90
pH = pKₐ + log (( NH₃/NH₄Cl))
pH = 9.26 + log (( 0.90 + 0.70)) = 9.26 + 0.11 = 10.54
