A hydrocarbon with the general formula CxHy is 92.26% carbon. Experiment shows that 0.311 g hydrocarbon...

A hydrocarbon with the general formula C_xH_y is 92.26% carbon. Experiment shows that 0.311 g hydrocarbon fills a 185 mL flask at 88.7 °C with a pressure of 486 mm Hg.

Calculate the molecular formula for this compound.

Expert Solution

queen_honey_blossom answered 2 months ago

A hydrocarbon with general formula CxHy was burned completely in air, yielding .18g of water and...

A hydrocarbon with general formula CxHy was burned completely in air, yielding .18g of water and .44 g of carbon dioxide. Which formula could give such data? Please explain step by step process. The answer is C2H4 and molar mass for water is 18. g/mol-1 and CO2 is 44.0 g / mol -1

an unkown hydrocarbon contain carbon hydrogen and oxygen combustion of 1.6 g of the hydrocarbon produces...

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As with any combustion reaction, the products of combusting a hydrocarbon fuel (CxHy) with oxygen (O2)...

As with any combustion reaction, the products of combusting a hydrocarbon fuel (CxHy) with oxygen (O2) are carbon dioxide (CO2) and water (H2O). A mass of 16.89 g for an unknown fuel was combusted in a reaction vessel containing an unknown amount of oxygen. At the end of the reaction, there still remained 16.85 g of the fuel as well as 0.0654 g of water and 0.1198 g of carbon dioxide. The oxygen was completely consumed during the reaction. How...

Cumene, a hydrocarbon, is 89.94% carbon, and its molar mass is 120.2 g/mol. What are the...

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A high grade fuel oil which consists of only hydrocarbon, CxHy is burnt in a combustion chamber at 25 °C. The standard heat of combustion is -43,515 J/g with CO2 (g) and H2O (l) as products. The temperature of the fuel and air entering the combustion chamber is 25 °C. The air is assumed dry. The flue gases leave at 300 °C and their average composition is 11.2 % CO2, 0.4 % CO, 6.2 % O2 and 82.2 % N2...

When 1.661 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 5.211grams of...

When 1.661 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 5.211grams of CO2 and 2.134 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 42.08 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. Enter the elements in the order presented in the question.

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Complete combustion of a 0.0150 mol sample of a hydrocarbon, CxHy, gives 3.024 L of CO2 at STP and 1.891 g of H2O. (a) What is the molecular formula of the hydrocarbon? (b) What is the empirical formula of the hydrocarbon? A 0.500-L bulb containing Ne at 685 torr is connected by a valve to a 2.50-L bulb containing CO2 at 375 torr. The valve between the two bulbs is opened and the two gases mix. The initial gas pressures...

An unknown gaseous hydrocarbon contains 85.63 % carbon. If its density is 0.488 g/L at 0.355...

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When 5.895 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 18.50 grams...

When 5.895 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 18.50 grams of CO2and 7.574 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 42.08 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. Empirical formula? Molecular formula?

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