A sample of CO2 is collected over water at 23oC. If the total pressure of the sample is 734 torr, and the vapor pressure of wate
2 answers:
<u>Answer:</u> The partial pressure of carbon dioxide is 712.8
<u>Explanation:</u>
Dalton's law of partial pressure states that the total pressure of the system is equal to the sum of partial pressure of each component present in it.
To calculate the partial pressure of carbon dioxide gas, we use the law given by Dalton, which is:
We are given:
Total pressure, = 734 torr
Vapor pressure of water, = 21.2 torr
Putting values in above equation, we get:
Hence, the partial pressure of carbon dioxide is 712.8
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Answer:
44 g
Explanation:
The formula for the number of moles (n) is equal to .
Since we need to find the mass, we derive it from the formula of the number of moles and we get that mass = n x molecular weight .
The molecular weight of = 12 g/mol (from the carbon) + 19x4 g/mol (from the 4 fluorine atoms)= 88 g/mol
We plug in the numbers in the derived formula for the mass and we get :
mass = n x molecular weight = 0.5 mol x 88 g/mol = 44 g
Answer:
30.17 grams of Cr can be produced by the reaction of 44.1 g of Cr₂O₃ with 35.0 g of Al.
19.33 grams of the excess react will remain once the reaction goes to completion.
Explanation:
You know:
2 Al + Cr₂O₃ → Al₂O₃ + 2 Cr
By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of the compounds participating in the reaction react and are produced:
- Al: 2 moles
- Cr₂O₃: 1 mole
- Al₂O₃: 1 mole
- Cr: 2 moles
Being:
- Al: 27 g/mole
- Cr: 52 g/mole
- O: 16 g/mole
the molar mass of the compounds participating in the reaction is:
- Al: 27 g/mole
- Cr₂O₃: 2*52 g/mole + 3 *16 g/mole= 152 g/mole
- Al₂O₃: 2*27 g/mole + 3 *16 g/mole= 102 g/mole
- Cr: 52 g/mole
Then, by stoichiometry of the reaction, the amounts of reagents and products that participate in the reaction are:
- Al: 2 moles* 27 g/mole= 54 g
- Cr₂O₃: 1 mole* 152 g/mole= 152 g
- Al₂O₃: 1 mole* 102 g/mole= 102 g
- Cr: 2moles*52 g/mole= 104 g
First, you must determine the limiting reagent. The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.
Then, for this you must apply the following rule of three: if 54 grams of Al react with 152 grams of Cr₂O₃ by stoichiometry of the reaction, 35 grams of Al with how much mass of Cr₂O₃ will react?
mass of Cr₂O₃= 98.52 grams
But 98.52 grams of Cr₂O₃ are not available, 44.1 grams are available. Since you have less moles than you need to react with 35 grams of Al, the compound Cr₂O₃ will be the limiting reagent.
To determine the amount of Cr that can be produced, you use the amount of limiting reagent available and apply the following rule of three: if by stoichiometry 152 grams of Cr₂O₃ produce 104 grams of Cr, 44.1 grams of Cr₂O₃ how much mass of Cr does it produce?
mass of Cr= 30.17 grams
<u><em>30.17 grams of Cr can be produced by the reaction of 44.1 g of Cr₂O₃ with 35.0 g of Al.</em></u>
As Al is the excess reagent, you must first calculate the amount of mass that reacts with 44.1 grams of Cr₂O₃ using the following rule of three: if 152 grams of Cr₂O₃ react with 54 grams of Al, 44.1 grams of Cr₂O₃ with how much mass of Al reaction to?
mass of Al=15.67 grams
With 35 grams being the amount of Al available, the amount of Al that will remain in the reaction after all the limiting reagent reacts and the reaction is complete is calculated by:
mass of excess= 35 grams - 15.67 grams= 19.33 grams
<em><u>19.33 grams of the excess react will remain once the reaction goes to completion.</u></em>