This problem asks for the net ionic equation between barium hypochlorite and perchloric acid. The answer then turns out to be 
.
<h3>Net ionic equations</h3>
In chemistry, when a chemical reaction takes place, one can study three versions of the chemical equation representing it:
1. Complete molecular equation: shows all the substances, their phases of matter and every balanced atom. In this case, one can write:
2. Complete ionic equation: shows all the aqueous salts and strong both acids and bases split into cation and anion; however, weak both acids and bases, such as the hypochlorous acid here, remain unionized as well as solid precipitates, liquids or gases:
3. Net ionic equation: cancels out the spectator ions (those equal on both reactants and products) and shows the relevant ions that undergo a reaction. In this case, both perchlorate and barium ions act as the spectator ones, consequently, we obtain:
That can also be written at equilibrium due to the concept of weak acid for the formation of hypochlorous acid:
Learn more about spectator ions: brainly.com/question/15365313
Based on the equation of the reaction, the moles of chlorine gas initially in the vessel is 0.12 moles
<h3>How many moles of chlorine were initially present?</h3>
The moles of chlorine initially present is determined using the equation of the reaction:
At STP, 1 mole of P4 reacts with 6 moles of chlorine.
Molar mass of P4 = 124.0 g
Molar mass of chlorine = 71.0 g
Mass of P4 in reaction vessel = 250 mg = 0.25g
moles of P4 in 0.25 g = 0.25/124 = 0.02 moles
0.02 moles of P4 will react with 0.02 × 6 moles of chlorine = 0.12 moles of chlorine.
Therefore, the moles of chlorine gas initially in the vessel is 0.12 moles.
Learn more about moles of a gas at: brainly.com/question/25417922
D is true because NO2 is a catalyst, and a catalyst is a compound which makes a reaction occur faster (not necessarily more effectively, creating more product, but it decreases the amount of time it takes).
Answer:
168 g
Reaction:
Explanation:
First we need to figure out what is the formula mass (Mr) of Fe2O3 (Iron(III) oxide).
The atomic mass of Fe=56, O=16
Mr= 56+56+16+16+16=160 g/mol
We can now figure out the moles of the iron:
240/160 = 1.5 mol
Then we need to find the ratio to make Fe.
In the reaction, we know that 1 mole of Fe2O3 can make 2 moles of Fe. So 1.5 moles of Fe2O3 can make 3 moles of Fe.
And then we need to find the mass of the Fe.
3×56=168 g.
Hence 168g of the iron is made after the reaction.
