What is the molecular mass of the complete combustion of 858g?

The complete combustion of .858 g of compound X gives 2.63 g of CO2 and 1.28 g of H2O. What is the lowest molecular mass X can have? – Quora The complete combustion of .858 g of compound X gives 2.63 g of CO2 and 1.28 g of H2O.

How many grams of CO2 are produced from combustion of X?

No Problem Ask this as a question. Complete combustion of 0.858 g of compound X gives 2.63g of CO 2 and 1.28g of H 2 O. The lowest molecular mass X can have

What is the molecular weight of CO2 in H2O?

Complete combustion of 0.858 g of compound X gives 2.63 g of CO2 and 1.28 g of H2O . The lowest molecular weight which X can have, is: O. The lowest molecular weight which X can have, is: =2.630g or since the molar mass of C O2 is 44g/mol since there is 1 mole. so C in C O2

What is the lowest molecular mass X can have?

Complete combustion of 0.858 gram of compound X gives 2.63 gram of CO2 and 1.28 gram of H2O the lowest molecular mass X can have? The compound X can only be a hydrocarbon as the total percentages of both carbon and hydrogen is almost equal to 100. C : H = 83.6/12 : 16.6/1 = 6.97 : 16.6 = 1 : 16.6/6.97 = 1 : 2.38.

What are the products of combustion of hydrocarbons?

The key here is to realize that you’re dealing with a hydrocarbon, that is, a compound that contains only carbon and hydrogen. Notice that the products of this combustion reaction are carbon dioxide, CO2, and water, H2O. This tells you that all the carbon that was initially a part of the hydrocarbon will now be part of the carbon dioxide.

What is the molecular mass of the compound X?

Originally Answered: complete combustion of .858g of compound X gives 2.63g of CO2 and 1.28g of H2O.The lowest molecular mass X can have is? The compound X can only be a hydrocarbon as the total percentages of both carbon and hydrogen is almost equal to 100.

What is the empirical formula of the hydrocarbon?

The empirical formula of the hydrocarbon will thus be C1H2 ⇒ CH2