We have 8.22 1 C atoms
We have 4.11 1 ethanol molecules
<u>Explanation</u>:
Step 1: Data given
Molecular formula of ethanol =
Mass of C = 164 grams
Molar mass C = 12.01 g/mol
Step 2: Calculate moles C
Moles C = mass C / molar mass C
Moles C = 164 grams / 12.01 g/mol
Moles C = 13.66 moles
Step 3: Calculate molecules of C
Atoms C = moles C number of Avogadro
Atoms C = 13.66 moles 6.02 1 molecules/ mol
Atoms C = 8.22 1 C atoms
Step 4: Calculate molecules in the sample
For 1 mol we have 2 moles C
For 13.66 moles C we have 13.66/ 2 = 6.83 moles
Molecules = 6.83 moles 6.02 1 = 4.11 1 molecules.
Answer : The final volume of the sample of gas is, 120 mL
Explanation :
According to the Boyle's law, the pressure of the gas is inversely proportional to the volume of gas at constant temperature and moles of gas.
or,
where,
= initial pressure = 1.5 atm
= final pressure = 5 atm
= initial volume = 400 mL
= final volume = ?
Now put all the given values in the above formula, we get:
Therefore, the final volume of the sample of gas is, 120 mL
I believe a heterogenous mixture cannot be considered as a single phase.
Answer:
The correct answer is option C.
Explanation:
The given rate law of reaction :
Rate of the reaction after doubling the concentration of Y : R'
The rate of the reaction will increase by the factor of 4.
Answer:
P(N₂) = 2.5 atm
Explanation:
Given data:
Total pressure of gasses = 6.7 atm
Partial pressure of O₂ = 3.0 atm
Partial pressure of CO₂ = 1.2 atm
Partial pressure of N₂ = ?
Solution;
According to Dalton law of partial pressure,
The total pressure inside container is equal to the sum of partial pressures of individual gases present in container.
Mathematical expression:
P(total) = P₁ + P₂ + P₃+ ............+Pₙ
Now we will solve this problem by using this law.
P(total) = P(O₂) + P(CO₂) + P(N₂)
6.7 atm = 3.0 atm + 1.2 atm + P(N₂)
6.7 atm = 4.2 atm + P(N₂)
P(N₂) = 6.7 atm - 4.2 atm
P(N₂) = 2.5 atm