Answer:
101
Explanation:
Provided that
And,
Now we expect the same
{S} (0.1mM)
This determines that generates a higher rate of product formation as compared to the
So we can easily calculate the for either of
or
as we know that Tube 1 is
and tube 2 is
As we know that
As the rates do not include any kind of units so we do not consider the units for
Now the calculation is
= 100.5
≈ 101
Answer:
n = 0.207 mole
Explanation:
We have,
P = 1 atm
V = 5 liter
R = 0.0821 L.atm/mol.K
T = 293 K
We need to find the value of n. The relation is as follows :
PV = nRT
Solving for n,
So, the value of n is 0.207 mol.
Answer:
The mass of oxygen that reacted is approximately 1.6 grams of oxygen
Explanation:
The given information are;
The mass of magnesium in the reaction = 2.43 grams
The final mass of the magnesium oxide = 4.12 grams
The chemical equation for the reaction is given as follows;
2Mg + O₂ → 2MgO
From which we see that two moles of magnesium, Mg, reacts with one mole of oxygen gas molecule, O₂, to produce two moles of magnesium oxide, MgO
The number of moles of magnesium present, , is given as follows;
By the given chemical equation, 2 moles of magnesium reacts with one mole of O₂, therefore;
1 mole of magnesium will react with 1/2 moles of oxygen which is 0.5 moles of oxygen also;
0.1 mole of magnesium will react with 0.05 moles of oxygen
The mass of one mole of oxygen = The molar mass of oxygen = 32 g/mol
The mass of oxygen in the reaction = The number of moles of oxygen × The molar mass of oxygen
The mass of oxygen in the reaction = 0.05 × 32 = 1.6 grams
Also from the molar mass of MgO which is 40.3044 g/mol, we have;
The mass fraction of oxygen = 16/40.3044 = 0.39698 ≈ 0.4
The mass of oxygen = 0.39698 × 4.12 = 1.636 g
Therefore, the mass of oxygen in the reaction is approximately 1.6 grams.