Question

1.A 0.5538 g sample of a pure soluble bromide compound is dissolved in water, and all...

1.A 0.5538 g sample of a pure soluble bromide compound is dissolved in water, and all of the bromide ion is precipitated as AgBr by the addition of an excess of silver nitrate. The mass of the resulting AgBr is found to be 1.1298 g. What is the mass percentage of bromine in the original compound? %

2. A student determines the manganese(II) content of a solution by first precipitating it as manganese(II) hydroxide, and then decomposing the hydroxide to manganese(II) oxide by heating. How many grams of manganese(II) oxide should the student obtain if his solution contains 37.0 mL of 0.419 M manganese(II) nitrate? g

3. A 13.36 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 19.58 grams of CO2 and 8.017 grams of H2O are produced. In a separate experiment, the molar mass is found to be 60.05 g/mol. Determine the empirical formula and the molecular formula of the organic compound.

4. A 3.605 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 5.374 grams of CO2 and 1.650 grams of H2O are produced. In a separate experiment, the molar mass is found to be 118.1 g/mol. Determine the empirical formula and the molecular formula of the organic compound.

Homework Answers

Answer #1

1)

1st find the mass of Br in AgBr

Molar mass of AgBr,

MM = 1*MM(Ag) + 1*MM(Br)

= 1*107.9 + 1*79.9

= 187.8 g/mol

mass(AgBr)= 1.1298 g

use:

number of mol of AgBr,

n = mass of AgBr/molar mass of AgBr

=(1.13 g)/(1.878*10^2 g/mol)

= 6.016*10^-3 mol

This is number of moles of AgBr

one mole of AgBr contains 1 moles of Br

use:

number of moles of Br = 1 * number of moles of AgBr

= 1 * 6.016*10^-3

= 6.016*10^-3

Molar mass of Br = 79.9 g/mol

use:

mass of Br,

m = number of mol * molar mass

= 6.016*10^-3 mol * 79.9 g/mol

= 0.4807 g

same will be the mass of Br in sample

mass % of Br = mass of Br * 100 / mass of sample

= 0.4807 * 100 / 0.5538

= 86.8 %

Answer: 86.8 %

Only 1 question at a time please

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A 5.797 gram sample of an organic compound containing C, H and O is analyzed by...
A 5.797 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 9.656 grams of CO2 and 3.163 grams of H2O are produced. In a separate experiment, the molar mass is found to be 132.1 g/mol. Determine the empirical formula and the molecular formula of the organic compound. **** Do the problem in Conversion factor style!
a 7.284 gram sample of an organic compound containing Containing C,H,O is analyzed by combustion analysis...
a 7.284 gram sample of an organic compound containing Containing C,H,O is analyzed by combustion analysis and 9.242 grams CO2 and 2.523 grams H2O are produced. I need the molecular and empirical formula
A 0.4958 g sample of a pure soluble chloride compound is dissolved in water, and all...
A 0.4958 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 1.0569 g. What is the mass percentage of chlorine in the original compound? % A student determines the copper(II) content of a solution by first precipitating it as copper(II) hydroxide, and then decomposing the hydroxide to copper(II)...
In a combustion analysis, 0.7308 g of an organic compound yielded 2.0840 g CO2 and 0.4874...
In a combustion analysis, 0.7308 g of an organic compound yielded 2.0840 g CO2 and 0.4874 g H2O. From mass spectrometry, it was found that the molecular weight for the compound is 108 amu. Determine the mass composition of this compound, its empirical formula, and its molecular formula.
7. A compound has the empirical formula CH and a molar mass of 78.11 g/mol. What...
7. A compound has the empirical formula CH and a molar mass of 78.11 g/mol. What is its molecular formula? 8. Upon combustion, a compound containing only carbon and hydrogen produces 1.83 g CO2 and 0.901 g H2O. Find the empirical formula of the compound. 9. Write a balanced equation for the reaction between solid cobalt(III) oxide and solid carbon to produce solid cobalt and carbon dioxide gas.
Combustion analysis of a compound yielded 269.01 g CO2, 55.09 g H2O, 70.30 g NO2, and...
Combustion analysis of a compound yielded 269.01 g CO2, 55.09 g H2O, 70.30 g NO2, and 97.90 g SO2. (a) What is the empirical formula of the compound? (Assume it contains no oxygen.) (b) If the molar mass of the compound is 196.30 g/mol, what is the molecular formula of the compound?
When 4.748 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 16.05 grams...
When 4.748 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 16.05 grams of CO2 and 3.286grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 26.04 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. empirical formula = ? molecular formula = ?
When 2.050 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 6.280 grams...
When 2.050 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 6.280 grams of CO2 and 3.000grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 86.18 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. empirical formula =? molecular formula =?
A 3.000 g sample of an organic compound was heated in oxygen and produced 7.568 g...
A 3.000 g sample of an organic compound was heated in oxygen and produced 7.568 g of CO2 and 1.328 g of water. a. Determine the empirical formula of the substance. b. In a separate experiment, the molar mass of the compound was determined to be 122.1. What is the molecular formula of the compound?
1. Combustion of 6.38g of an organic compound containing C, H and O gives 9.06g of...
1. Combustion of 6.38g of an organic compound containing C, H and O gives 9.06g of CO2 and 5.58g of H2O. What is the empirical formula of the compound?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT