A chemical reaction takes place in a closed system. The mass of the reactants before the reaction was grams. What must the mass
1 answer:
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Answer: The empirical formula of one that contains 30.45% nitrogen is .
Explanation:
Given: Mass of nitrogen = 30.45 g
Let us assume that the mass of given oxide is 100 grams.
As the atomic mass of nitrogen is 14.0067 g. So, moles of nitrogen will be calculated as follows.
Also, mass of oxygen = (100 - 30.45) g = 69.55 g
Atomic mass of oxygen is 15.9994 g/mol. So, moles of oxygen will be as follows.
The ratio of both the atoms is as follows.
This means that gas has 2 moles of oxygen to 1 mole of nitrogen. Hence, the formula of oxide is .
Thus, we can conclude that the empirical formula of one that contains 30.45% nitrogen is .
Answer:
630.95 grams of Na₂CO₃ would be needed to produce 1000g of NaHCO₃
Explanation:
The balanced reaction is:
Na₂CO₃ + CO₂+ H₂O → 2 NaHCO₃
By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of each compound participate in the reaction:
- Na₂CO₃: 1 moles
- CO₂: 1 mole
- H₂O: 1 mole
- NaHCO₃: 2 moles
Being the molar mass:
- Na₂CO₃: 106 g/mole
- CO₂: 44 g/mole
- H₂O: 18 g/mole
- NaHCO₃: 84 g/mole
Then by stoichiometry the following quantities of mass participate in the reaction:
- Na₂CO₃: 1 mole* 106 g/mole= 106 g
- CO₂: 1 mole* 44 g/mole= 44 g
- H₂O: 1 mole* 18 g/mole= 18 g
- NaHCO₃: 2 moles* 84 g/mole= 168 g
You can apply the following rule of three: if 106 grams of Na₂CO₃ are needed to produce 168 grams of NaHCO₃, how much mass of Na₂CO₃ is necessary to produce 1000 grams of NaHCO₃?
mass of Na₂CO₃= 630.95 grams
<u><em>630.95 grams of Na₂CO₃ would be needed to produce 1000g of NaHCO₃</em></u>