The partial pressure of CO is 0.536 atom.
<h3>Further Explanation</h3>
Dalton's Law of Partial Pressure states that the total pressure of a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases. Mathematically, it can be represented as follows:
If the total pressure is known as well as the number of moles of the gases in the mixture, the partial pressure of a component as can be calculated using the equation below:
where:
Pₓ is the partial pressure of gas X
P(total) = total pressure of the mixture
nₓ = number of moles of gas X
n(total) = total number of moles of gas
To solve the problem, first sort the given:
- n(total) = 0.220 mol CO + 0.350 mol F₂ + 0.640 mol He = <u>1.21 moles</u>
- n(CO) = 0.220 mol
- P(total) = 2.95 atm
Then we plug in the given values into the equation above:
<h3>Learn More</h3>
- Ideal Gas Law brainly.com/question/12936013
- Root Mean Square brainly.com/question/5980325
Keywords: Dalton's Law of Partial Pressure, mole ratio
First, let's assign variables for the moles of CuSO₄·5H₂O as x and moles of MgSO₄·7H₂O as y. The molar mass of the substances are the following
CuSO₄·5H₂O: <span>249.685 g/mol
</span>CuSO₄: <span>159.609 g/mol
</span>MgSO₄·7H₂O: <span>246.49 g/mol
</span>MgSO₄: <span>120.366 g/mol
</span>H₂O: 18 g/mol
The solution is as follows:
2.988 = 249.685x + 246.49y --> eqn 1
5.02 - 2.988 = 18(5x + 7y) --> eqn 2
Solving both equations simultaneously, the values of x and y are:
x = 0.0134 mol CuSO₄·5H₂O
y = 0.0257 mol MgSO₄·7H₂O
Thus, the percent CuSO₄·5H₂O is equal to
Mass Percentage = [(0.0134 mol CuSO₄·5H₂O)*(249.685 g/mol )]/{[(0.0134 mol CuSO₄·5H₂O)*(249.685 g/mol )] + [(0.0257 mol MgSO₄·7H₂O)*(246.49 g/mol)]} * 100
Mass percentage = 34.56%
Answer:
We have the final answer as
<h2>0.8 g/cm³</h2>
Explanation:
The density of a substance can be found by using the formula
From the question
mass of pumpkin = 8 g
volume = 10 cm³
It's density is
We have the final answer as
<h3>0.8 g/cm³</h3>
Hope this helps you