When hydrocarbons are burned in a limited amount of air, both CO and CO2 form. When 0.450 g of a

When hydrocarbons are burned in a limited amount of air,...

Key Concepts

Incomplete vs Complete Combustion

This key concept distinguishes between the two types of combustion based on the availability of oxygen. In complete combustion, enough oxygen is present to convert all carbon to carbon dioxide, whereas in incomplete combustion, limited oxygen results in the formation of both carbon dioxide and carbon monoxide, thus affecting the mass balance and calculations in the reaction.

Stoichiometry

Stoichiometry focuses on the quantitative relationships between reactants and products in a chemical reaction. It is used to relate the masses of reactants (such as oxygen in combustion) to the masses of products formed, and to determine quantities like the amount of oxygen required for both complete and incomplete combustion.

Empirical Formula Determination

Determining the empirical formula involves converting the masses of individual elements obtained (often via combustion products) into moles, and then expressing their simplest whole-number ratio. This method forms the basis for understanding the fundamental composition of a compound from experimental data.

Combustion Analysis

This concept involves studying the products of the combustion of a substance to determine its composition. By analyzing the masses of the products (such as carbon dioxide, carbon monoxide, and water) produced from the burning of a hydrocarbon, one can deduce the relative amounts of carbon, hydrogen, and oxygen in the original compound.

Transcript

00:02 So in this problem we are given a combustion reaction of a hydrocarbon which is burned in a limited amount of air and which is formed both carbon monoxide and carbon dioxide and we are given the mass of carbon monoxide, carbon dioxide and water which is formed in this reaction.

00:30 So in first part of this reaction we have to find out the empirical formal of the compound.

00:34 So to find out the empirical formula of the compound, first we have to know how many grams of carbon and hydrogen are in the compound.

00:50 And we can find out the mass of carbon and hydrogen in the compound by calculating their mass in the products, which is carbon monoxide, carbon dioxide, and h2o.

01:01 So from carbon monoxide and carbon dioxide, we can find the mass of carbon and from h2o, we can find the mass of hydrogen.

01:15 So what we'll do first, we'll find out the number of moles of carbon monoxide, carbon dioxide, and water which is produced.

01:23 From there, we will find out the number of mole of carbon and hydrogen which is being produced.

01:28 And from those number of moles we'll find the mass of carbon and hydrogen in gram and these masses will be the mass of carbon and hydrogen in the original compound and from their mass in original compound we can find the number of moles of carbon and number of moles of hydrogen then we will divide each number of moles by the smallest number of moles to get a simplest whole number ratio of carbon and hydrogen's mole number from there we can find out the empirical formula of the hydrocarbon so our first step will be to find out the number of mole of each product so the number of mole of carbon monoxide produced will be the mass of carbon monoxide which is 0 .467 gram over the molar mass of carbon monoxide which is 28 .01 gram per mole and it it will give us a value of 0 .0167 mole.

02:45 Now, since we can see that in one molecule of carbon monoxide, we have one carbon atom, that means in one mole of carbon monoxide, we will have one mole of carbon, and in 0 .067 mole of carbon monoxide, we will have the same number of mole of carbon.

03:03 So the number of more of carbon here is also 0 .0167 mole and from here we can find the mass of carbon which is being produced in the form of carbon monoxide which will be just the number of moles times the molar mass of carbon which is 12 .01 gram per mole it will give us a value of 0 .200 gram so this is the mass of carbon which is being produced in the form of carbon monoxide now we'll find the mass of carbon in the form of carbon dioxide and for that we'll find out the number of moles of carbon dioxide first which is again the mass of carbon dioxide produced over the molar mass of carbon dioxide which is 44 .01 gram per mole and this will give us a value of 0 .0166.

04:12 Again in one molecule of carbon dioxide we have one carbon that means in this in a in a certain number of mole of carbon dioxide we will have the same number of mole of carbon dioxide that means this is the number of mole of carbon in this much more of carbon dioxide and from here we can directly find out the mass of carbon here which will be the number of mole of carbon in carbon dioxide which is 0 .0166m times the molar mass of carbon which is 12 .01 gram per mole and from here we'll have again the same amount of carbon in carbon dioxide so this is the amount of carbon which is being produced in the form of carbon dioxide so the total carbon in the original hydrocarbon will be the sum of the carbon produced in the form of carbon monoxide and the mass of carbon which is produced in the form of carbon dioxide so the total mass of carbon will be 0 .22 gram plus 0 .200 gram which will give us 0 .40 gram carbon so this is the mass of carbon now we'll find out the mass of hydrozone so for that we need to find out the number of mole of water first which is being produced so the mass of water which is produced is 0 .450 gram and the molar mass of water is 18 .016 gram per mole so from here we will have a value of 0 .0 to 5 mall now this is the number of mole of h2o which is being produced that means and again we can see that in one molecule of h2 we have two hydrogen that means in a certain number of mol of h2 we will have two times that mole of hydrogen so the number of more of hydrogen will be two times 0 .025 mole which will give us 0 .050 mole of hydrogen now from here you can find the mass of hydrogen which will be just this number of moles time the molar mass of hydrogen which is 1 .008 gram per mole so it will give us a value of again up 0 .0 approximately the same mass of hydrogen so this is the mass of hydrogen which is being produced in the form of h2 and since this is formed from the combustion of the original hydrocarbon that means this is the mass of hydrogen in the original hydrocarbon 2 now we know the mass of carbon and hydrozone in the original hydrocarbon so from here we can find the number of mole of carbon and hydrogen in the original hydrocarbon so we will write the mass of carbon which is 0 .40 and mass of hydrozone is 0 .050 gram so these are the mass of carbon and hydrogen in the original hydrocarbon now we'll find out their number of moles in the original hydrocarbon so the number of mole of carbon will be 0 .40 gram over the molar mass of hydrocarbon is 12 .01 gram per mole and it will give us a value of 0 .033 mole and the number of mole of hydrozone will be the mass of hydrogen over the molar mass of hydrogen which will give us a value of 0 .050 mole...

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