An oxide of nitrogen is 25.9% N by mass, has a molar mass of 108 g/mol, and contains no nitrogen-nitrogen or oxygen-oxygen bonds
. Draw its Lewis structure (including all lone pair electrons) and name it. Include any nonzero formal charges in your structure.
1 answer:
Answer:
The compound is N2O4
Explanation:
We have certain important pieces of information about the compound;
1) it is an oxide (a binary compound of nitrogen and oxygen)
2) there are no N-N bonds present
3) there are no O-O bonds present
Since it contains only nitrogen and oxygen then nitrogen accounts for 25.9% of the molecule by mass then oxygen should account for (100-25.9) = 74.1% oxygen
Relative atomic mass of oxygen = 16
Relative atomic mass of nitrogen = 14
We now deduce the empirical formula
Nitrogen. Oxygen
25.9/14. 74.1/16
1.85/1.85. 4.6/1.85 (divide through by the lowest ratio)
1 2
Empirical formula is NO2
To find the molecular formula
(NO2)n = 108
(14+2(16))n= 108
46n=108
n= 108/46
n= 2
Therefore molecular formula= N2O4
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Answer:
The theoretical yield of carbonic acid is 1.24 grams.
Explanation:
The balanced equation for the formation of carbonic acid by the reaction of carbon dioxide with water is:
CO₂ + H₂O → H₂CO₃
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of reactant and product participate:
- CO₂: 1 mole
- H₂O: 1 mole
- H₂CO₃: 1 mole
An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:
P * V = n * R * T
Moles of carbon dioxide can be calculated using ideal gas law equation. In this case:
- P= 101.3 kPa= 1 atm
- V= 495 mL= 0.495 L (being 1,000 mL=1 L)
- n=?
- R= 0.082
- T= 25 C= 298 K (being 0 C=273 K)
Replacing:
1 atm* 0.495 L= n* 0.082 *298 K
Solving:
n= 0.02 moles
Then, by reaction stoichiometry 0.02 moles of carbon dioxide produces 0.02 moles of carbonic acid.
Since the molar mass of carbonic acid is 62.03 g/mol, then you can apply the following rule of three: if there are 62.03 grams in 1 mole, how much mass is there in 0.02 moles?
mass= 1.24 grams
<em><u>The theoretical yield of carbonic acid is 1.24 grams.</u></em>