This is the chemical formula for methyl acetate: CH32CO2. Calculate the mass percent of hydrogen in methyl acetate. Round your a
1 answer:
<u>Answer:</u> The mass percent of hydrogen in methyl acetate is 8 %
<u>Explanation:</u>
The given chemical formula of methyl acetate is
To calculate the mass percentage of hydrogen in methyl acetate, we use the equation:
Mass of hydrogen = (6 × 1) = 6 g
Mass of methyl acetate = [(3 × 12) + (6 × 1) + (2 × 16)] = 74 g
Putting values in above equation, we get:
Hence, the mass percent of hydrogen in methyl acetate is 8 %
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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>
Answer:
The correct answer is - option D. (check image)
Explanation:
Alkynes and alkenes both decolorized bromine in carbon tetrachloride. The absorption of the IR at about 3300 cm-1 for the X here that are found in the terminal alkynes absorption range only. In presence of excess hydrogen and a nickel catalyst, x gives the 2-methyl pentane.
The most likely structure for X is: CH3-CH3-ch-CH2-C≡CH
