How does the potential energy of a double bond (like oxygen-oxygen) compare to a weak interaction or single bond (like argon-oxy
1 answer:
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Answer:
C₃H₅O₂
4C₃H₅O₂ + 13O₂ → 12CO₂ + 10H₂O
Explanation:
The reaction can be expressed as:
CₓHₓOₓ + nO₂ → CO₂ + H₂O
Under the assumption that there was a total combustion, all of the carbon in the reactant was combusted into CO₂, so <u>the mass of C contained in the C.H.O. compound is the same mass of C contained in 1.039 g of CO₂</u>:
All of the hydrogens atoms in the compound ended up becoming H₂O, so <u>the mass of H contained in the C.H.O. compound is the same mass of H contained in 0.6369 g of H₂O</u>:
Because the compound is composed only by C, H and O, <u>the mass of O in the compound can be calculated by substraction</u>:
0.5438 g Compound - 0.2834 g C - 0.0354 g H = 0.2250 g O
In order to determine the empirical formula, we calculate the moles of each component:
- mol C = 0.2834 g C ÷ 12 g/mol = 0.0236 mol C
- mol H = 0.0354 g H ÷ 1 g/mol = 0.0354 mol H
- mol O = 0.2250 g O ÷ 16 g/mol = 0.0141 mol O
Then we divide those values by the lowest one:
0.0236 mol C ÷ 0.0141 = 1.67
0.0354 mol H ÷ 0.0141 = 2.51
0.0141 mol O ÷ 0.0141 = 1
If we multiply those values by 2, we're left with the empirical formula C₃H₅O₂.
- The reaction is:
4C₃H₅O₂ + 13O₂ → 12CO₂ + 10H₂O
A gas is contained in a tick-walled balloon. When the pressure changes from 2. 95atm to <u>2.57</u> atm. p.
<h3>What is pressure?</h3>Pressure is a force perpendicular to the unit area on which it is applied.
Given that, P1, the initial pressure is 2.95 atm
The initial volume, V1 = 7.456 L
The final volume, V2 = 4.782 L
The initial temperature, T1 = 379k
The final temperature, T2 = 212k
The equation will be
Putting the values in the equation
Thus, the pressure changes from 2. 95atm to <u>2.57</u> atm p.
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Answer: The partial pressure of oxygen in the mixture is 321 mm Hg
Explanation:
According to Dalton's law, the total pressure is the sum of individual pressures.
Given : = total pressure of gases = 752 mm Hg
= partial pressure of Helium = 234 mm Hg
= partial pressure of nitrogen = 197 mm Hg
= partial pressure of oxygen = ?
Putting in the values we get:
The partial pressure of oxygen in the mixture is 321 mm Hg