Question

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.

Homework Answers

Answer #1

Solution :-

Lets first calculate the mass of the each element using the given mass of the CO2 , H2O and sample mass

mass of the C = 2.20 g CO2 * 27.29% C / 100 % = 0.60 g C

mass of H = 0.440 g H2O * 11.2 % H / 100 % = 0.0493 g H

now lets find the mass of oxygen

mass of O = mass of sample - (mass of C + mass of H)

                   = 1.00 g - (0.60 g +0.0493 g)

                  = 0.351 g

now lets calculate moles of the each element

moles = mass / molar mass

moles of C = 0.600 g / 12.01 g per mol = 0.05 mol

moles of H = 0.0493 g / 1.0079 g per mol = 0.05 mol

moles of O = 0.351g / 16 g per mol = 0.022 mol

now lets find the ratio of the elements by dividing the moles by the smallest mole value

C= 0.05 / 0.022 = 2

H= 0.05 / 0.022 = 2

O = 0.022 / 0.022 = 1

Therefore Empirical formula is C2H2O

now lets find the empirical fiormula mass

C2H2O = (2*12.01)+(2*1.0079)+(1*16) = 42.04 g

now lets find the ratio of the molar mass to empirical formula mass

N= molar mass / empirical formula mass

   = 170 / 42.04

   = 4

Therefore moilecular formula = 4 * empirical formula

                                                     = 4*C2H2O

                                                     = C8H8O4

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 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?
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...
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 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!
A, an unknown compound, is composed of only carbon and hydrogen. When 95.2g of A was...
A, an unknown compound, is composed of only carbon and hydrogen. When 95.2g of A was completely burned, 85.6g of water was produced. If the mass of A has a value between 115 g/mol and 125 g/mol, obtain A's experimental and molecular formula. Also, calculate the mass of carbon dioxide produced by this reaction.
9.00g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen,...
9.00g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 70./gmol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 28.29g water 11.58g Use this information to find the molecular formula of X .
8.00g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen,...
8.00g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 46./gmol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 15.31g water 9.40g Use this information to find the molecular formula of X .
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?
cyclopentane, a hydrocarbon with carbon and hydrogen , has a molar mass of 70.13 g/mol. If...
cyclopentane, a hydrocarbon with carbon and hydrogen , has a molar mass of 70.13 g/mol. If the combustion of .5600 g of cyclopentane produces .7195 grams h20 and 1.757 grams CO2 what is the molecular formula?