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Veseljchak [2.6K]
3 years ago
13

What is an empirical formula for a compound that is 82.2% nitrogen and 17.8% hydrogen

Chemistry
1 answer:
makkiz [27]3 years ago
8 0
Percent to mass
Mass to mole
Divide by small
Multiply 'til whole

Assume 100 g of substance, then 82.2 g N and 17.8 g H.

82.2 g N * (1 mol/14.01 g N) = 5.86 mol N
17.8 g H * (1 mol/1.01 g H) = 17.6 mol H

Divide by the smallest mole
17.6 H / 17.6  = 1 H
5.86 N / 17.6 =  1/3 N

Multiply to make whole number ( x3 in this case)
3 x 1 H = 3H
3 x 1/3 N = 1 N

NH3
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Answer:

The molarity of urea in this solution is 6.39 M.

Explanation:

Molarity (M) is <em>the number of moles of solute in 1 L of solution</em>;  that is

molarity = moles of solute ÷ liters of solution

To calculate the molality, we need to know the number of moles of urea and the volume of solution in liters. We assume 100 grams of solution.

Our first step is to calculate the moles of urea in 100 grams of the solution,

using the molar mass a conversion factor. The total moles of 100g of a 37.2 percent by mass solution is

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Now we need to calculate the volume of 100 grams of solution, and we use density as a conversion factor.

1.032 g/mL ÷ 100 g = 96.9 mL

This solution contains 0.619 moles of urea in 96.9 mL of solution. To express it in molarity, we need to calculate the moles present in 1000 mL (1 L) of the solution.

0.619 mol/96.9 mL × 1000 mL= 6.39 M

Therefore, the molarity of the solution is 6.39 M.

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3 years ago
Find the molecular mass of.
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Answer:

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