20. compound with molar mass 180.2 g/mol has the following composition: Determin

Question

20.

compound with molar mass 180.2 g/mol has the following composition:

Determine the molecular formula

(Express your answer as a chemical formula.)

(Input the elements in your formula in the order shown above. If parentheses are needed in the formula, be sure to include them in your answer.)

25.

A 0.4230 g sample of impure sodium nitrate (contains sodium nitrate plus inert ingredients) was heated, converting all the sodium nitrate to 0.1002 g of sodium nitrite and oxygen gas. Determine the percent of sodium nitrate in the original sample.

sodium nitrate in the original sample = %

35.

Hexamethylenediamine (C6H16N2) is one of the starting materials for the production of nylon. It can be prepared from adipic acid (C6H10O4) by the following overall reaction:

C6H10O4(l) + 2 NH3(g) + 4 H2(g) ? C6H16N2(l) + 4 H2O(l)

Click here to see the production of nylon.

What is the percent yield if 364.0 g hexamethylenediamine is made from 863.6 g adipic acid?

33.

The production capacity for acrylonitrile (C3H3N) in the United States is over 2 billion pounds per year. Acrylonitrile, the building block for polyacrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen:

2C3H6(g) + 2NH3(g) + 3O2(g) ? 2C3H3N(g) + 6H2O(g)

Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below:

g = mass of acrylonitrile produced

What mass of water is formed from your mixture?

mass of water formed =  g

Calculate the mass (in grams) of each reactant after the reaction is complete:

g

Explanation / Answer

Ans 20 :

Let the mass of sample be 100 g

So the mass of carbon = 60.0 g

number of moles of carbon = 60.0 / 12 = 5 mol

Mass of hydrogen = 4.48 g

Number of moles of hydrogen = 4.48 / 1.008 = 4.44 mol

mass of oxygen = 35.5 g

number of moles of oxygen = 35.5 / 16 = 2.22 mol

Dividing the number of mol by a common value we get the ratio of number of moles as : 9 : 8 : 4

So the empirical formula of the compound becomes : C9H8O4

The empirical mass = 9(12) + 8(1.008) + 4(16)

= 180 g /mol

This corresponds with the molar mass of the compound , so the molecular formula of the compound will be C9H8O4

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