Question

Combustion analysis of 0.600 g of an unknown compound containing carbon, hydrogen, and oxygen produced 1.043...

Combustion analysis of 0.600 g of an unknown compound containing carbon, hydrogen, and oxygen produced 1.043 g of CO2 and 0.5670 g of H2O. The molar mass is 532.7 g/mol. What is the molecular formula of the compound?

Homework Answers

Answer #1

The MM for CO2 reported is 44 g/mol and for H2O is 18 g/mol.

If we have 1.043 g of CO2 means that we have:

44 g CO2 --------> 12 g C

1.043 g ------------> X

X = 1.043 * 12/44 = 0.2845 g of C

For H:

18 g H2O ----------> 2 g H

0.5670 g -----------> Y

Y = 0.5670 * 2/18 = 0.063 g

For O:

0.600 - 0.063 - 0.2845 = 0.2525 g of O

C = 0.2845 / 12 = 0.0237 / 0.0158 = 1.5

H = 0.063 / 1 = 0.063 / 0.0158 = 3.987

O = 0.2525 / 16 = 0.0158 / 0.0158 = 1

Empirical Formula = C2H4O

MM = 2*12 + 4*1 + 16 = 44 g/mol

n = 532.7 / 44 = 12.11

Molecular Formula = 12 * C2H4O

MF = C24H48O12

Hope this helps

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
Combustion analysis of 0.600 g of an unknown compound containing carbon, hydrogen, and oxygen produced 1.043...
Combustion analysis of 0.600 g of an unknown compound containing carbon, hydrogen, and oxygen produced 1.043 g of CO2 and 0.5670 g of H2O. The molar mass is 532.7 g/mol. What is the molecular formula of the compound?
Combustion analysis of an unknown compound containing only carbon and hydrogen produced 2.845 g of CO2...
Combustion analysis of an unknown compound containing only carbon and hydrogen produced 2.845 g of CO2 and 1.744 g of H2O. What is the empirical formula of the compound? C4H10 CH3 C5H2 CH2
Combustion of a 1.031 g sample of a compound containing only carbon, hydrogen, and oxygen produced...
Combustion of a 1.031 g sample of a compound containing only carbon, hydrogen, and oxygen produced 2.265 g of CO2, and 1.236 g of H2O. What is the empirical formula of the compound? Please explain step by step how you solve this!
Upon combustion, a 0.9004-g sample of a compound containing only carbon, hydrogen, and oxygen produced 0.8802...
Upon combustion, a 0.9004-g sample of a compound containing only carbon, hydrogen, and oxygen produced 0.8802 g CO2 and 0.1802 g H2O. Find the empirical formula of the compound.
combustion of 1.00 g of a common analgesic which is composed of carbon, hydrogen, oxygen produced...
combustion of 1.00 g of a common analgesic which is composed of carbon, hydrogen, oxygen produced 2.20g of carbon dioxide, CO2 and 0.440 grams of water. The molar mass of this compound is known to be between 170 and 190 g. Determine the molecular formula of the compound.
41) Combustion analysis of a 0.675 g sample of an unknown compound that contains only carbon,...
41) Combustion analysis of a 0.675 g sample of an unknown compound that contains only carbon, hydrogen, and oxygen gives 0.627 g of CO2 and 1.534 g of H2O. The molecular mass of the unknown is Select one: A. C6H12O2. B. C3H6O. C. C9H18O3. D. unable to be determined from this data. 42) How many milliliters of 0.550 M hydriodic acid are needed to react with 25.00 mL of 0.217 M CsOH? HI(aq) + CsOH(aq) → CsI(aq) + H2O(l) Select...
In an experiment, 4.624 grams of a compound containing carbon, hydrogen and oxygen yieled 6.557 g...
In an experiment, 4.624 grams of a compound containing carbon, hydrogen and oxygen yieled 6.557 g of CO2 and 4.026 g of H2O in a combustion analysis. Determine the empirical formula of the compound. What are the respective molar concentrations (molarity, M) of Fe3+ and I- ions obtained by dissolving 0.200 mol FeI3 in water and diluting 725 mL? What volume of 3.25 M (NH4)2SO4 is needed in order to give 8.60 g of (NH4)2SO4 (132.14 g/mol).
A compound contains only carbon, hydrogen, and oxygen. Combustion of 65.76 g of the compound yields...
A compound contains only carbon, hydrogen, and oxygen. Combustion of 65.76 g of the compound yields 96.38 g of CO2 and 39.46 g of H2O. The molar mass of the compound is 90.078 g/mol. 1. Calculate the grams of carbon (C) in 65.76 g of the compound: 2. Calculate the grams of hydrogen (H) in 65.76 g of the compound. 3. Calculate the grams of oxygen (O) in 65.76 g of the compound. Based on your previous answers, calculate 1....
A compound contains only carbon, hydrogen, and oxygen. Combustion of 91.88 g of the compound yields...
A compound contains only carbon, hydrogen, and oxygen. Combustion of 91.88 g of the compound yields 134.7 g of CO2 and 55.13 g of H2O. The molar mass of the compound is 180.156 g/mol. 1. Calculate the grams of carbon (C) in 91.88 g of the compound: grams 2. Calculate the grams of hydrogen (H) in 91.88 g of the compound. grams 3. Calculate the grams of oxygen (O) in 91.88 g of the compound. grams 1. the moles of...
An unknown compound contains only carbon, hydrogen, and oxygen (CxHyOz ). Combustion of 4.50 g of...
An unknown compound contains only carbon, hydrogen, and oxygen (CxHyOz ). Combustion of 4.50 g of this compound produced 6.60 g of carbon dioxide and 2.70 g of water. If 4.50 g of the unknown compound contained 0.150 mol of C and 0.300 mol of H, how many moles of oxygen, O, were in the sample?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT