Answer:
84.00g CO2 * 1mol CO2/44.009g CO2 * 25mol O2/16mol CO2 * 31.998g O2/1mol O2 = 95.43g O2
Explanation:
The percentage of Calcium carbonate in chalk = 100%
<h3>Further explanation</h3>
Given
1.51 g piece of chalk produces 0.665 g of carbon dioxide
Required
percentage of calcium carbonate
Solution
Reaction
CaCO3 (s) + 2 HCl (aq) → CaCl2 (aq) + H2O (l) + CO2 (g)
mol CO2 :
= 0.665 g : 44 g/mol
= 0.015
From the equation, mol CaCO3 = mol CO2 = 0.015
mass CaCO3 :
= mol x MW
= 0.015 x 100
= 1.5 g
Answer:
Explanation:
We can start with the <u>reaction of hydrogen and nitrogen to produce ammonia</u>, so:
When we <u>balance</u> the reaction we will obtain:
Now, the <u>production of nitric acid</u> with oxygen would be:
If we <u>balance</u> the reaction we will obtain:
Now, if we put the reactions together we will obtain:
We can <u>multiply</u> the second reaction by "2":
We have "" on <u>both sides</u>. In the first reaction is in the right in the second reaction is on the left. Therefore we can <u>cancel out</u> this compound and we will obtain:
On this reaction, we will have 2 nitrogen atoms on both sides, 6 hydrogen atoms on both sides, and 8 oxygen atoms on both sides. So, this would be the <u>net reaction</u> for the production of nitric acid.
Answer:
the particles with a negative charge are protons