A0.1153-gram sample of a pure hydrocarbon was burned in a c-h combustion train to produce 0.3986 gram of co2and 0.0578 gram of h2o. determine the masses of c and h in the sample and the percentages of these elements in this hydrocarbon.

The mass of carbon and hydrogen in the sample is 0.1087 g and 0.0066 g respectively and the percentage composition of carbon and hydrogen in the sample is 94.27 % and 5.72 % respectively.

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon and hydrogen follows:

where, 'x' and 'y' are the subscripts of carbon and hydrogen respectively.

We are given:

Mass of

Mass of

Mass of sample = 0.1153 g

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 0.3986 g of carbon dioxide, of carbon will be contained.

In 18g of water, 2 g of hydrogen is contained.

So, in 0.0578 g of water, of hydrogen will be contained.

To calculate the percentage composition of a substance in sample, we use the equation:

     ......(1)

Mass of sample = 0.1153 g

Mass of carbon = 0.1087 g

Putting values in equation 1, we get:

Mass of sample = 0.1153 g

Mass of hydrogen = 0.0066 g

Putting values in equation 1, we get:

Hence, the mass of carbon and hydrogen in the sample is 0.1087 g and 0.0066 g respectively and the percentage composition of carbon and hydrogen in the sample is 94.27 % and 5.72 % respectively.

6.4 cm (max) - 25 cm (min)

answer: cellular respiration takes in food and uses it to create atp, a chemical which the cell uses for energy. usually, this process uses oxygen, and is called aerobic respiration. it has four stages known as glycolysis, link reaction, the krebs cycle, and the electron transport chain.