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University of Maine

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Problem 133

The human body excretes nitrogen in the form of urea, $\mathrm{NH}_{2} \mathrm{CONH}_{2} .$ The key step in its biochemical formation is the reaction of water with arginine to produce urea and ornithine:

(a) What is the mass $\%$ of nitrogen in urea, in arginine, and in

ornithine? (b) How many grams of nitrogen can be excreted as

urea when 135.2 $\mathrm{g}$ of ornithine is produced?

Answer

a) fraction(N,urea) $=46,64$ percent

fraction(N,arginine) $=31,98$ percent

fraction(N,ornithine) $=21,04$ percent

b) $\mathrm{m}(\mathrm{N})=28,44 \mathrm{g}$

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## Discussion

## Video Transcript

to calculate the percent nitrogen in the three different compounds given in this reaction. First, we need to have the molecular formulas from structural formula. It's so given the diagrams we can draw, we can write our structural formulas. When we look at the first compound, you see the elements present or kurban hydrogen, nitrogen and oxygen. There are six carbons, 15 hydrogen for a nitrogen and to oxygen's we already have. The formula for Yuria that's been given to us is and each to C O and H two. And finally, for the last compound, we used the picture again to determine the formula. There are five carbons, two nitrogen ins, 13 hydrogen zones and to Oxygen's. Once we have the formulas for each, we can find the molar mass or each. We do that, using our periodic table and adding up the individual molar masses and multiplying by their coefficients. So the first compound has the molar mass of 175.216 grams. Permal second compound Yuria has a Mueller math of 60 0.56 grams per mole, and finally, our last one has a molar mass of 133 0.173 grams per mole. And again, these numbers come from looking up the individual molar masses and multiplying by their sub scripts. Find the percent nitrogen we simply look at the number of nitrogen is in each compound. So for the 1st 1 there are four multiplied by the molar mass of nitrogen and then divide by the total Mueller Mass and multiplied by 100 in the Sequels, 31.98 percent. This one we also have We have to nitrogen, divided by the molar mass times 100 which gives us 46 0.65%. And finally, in our last compound there are two nitrogen divided by the total Moeller mass times 100 or 21 0.4%.

## Recommended Questions

Your body deals with excess nitrogen by excreting it in the form of urea, $\mathrm{NH}_{2} \mathrm{CONH}_{2}$. The reaction producing it is the combination of arginine $\left(\mathrm{C}_{6} \mathrm{H}_{14} \mathrm{N}_{4} \mathrm{O}_{2}\right)$ with water to give urea and ornithine $\left(\mathrm{C}_{5} \mathrm{H}_{12} \mathrm{N}_{2} \mathrm{O}_{2}\right)$. $$\mathrm{C}_{6} \mathrm{H}_{14} \mathrm{N}_{4} \mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{NH}_{2} \mathrm{CONH}_{2}+\mathrm{C}_{5} \mathrm{H}_{12} \mathrm{N}_{2} \mathrm{O}_{2}$$ If you excrete $95 \mathrm{mg}$ of urea, what mass of arginine must have been used? What mass of ornithine must have been produced?

Your body deals with excess nitrogen by excreting it in the form of urea, $\mathrm{NH}_{2} \mathrm{CONH}_{2}$. The reaction producing it is the combination of arginine $\left(\mathrm{C}_{6} \mathrm{H}_{14} \mathrm{N}_{4} \mathrm{O}_{2}\right)$ with water to give urea and ornithine $\left(\mathrm{C}_{5} \mathrm{H}_{12} \mathrm{N}_{2} \mathrm{O}_{2}\right)$ $\mathrm{C}_{6} \mathrm{H}_{14} \mathrm{N}_{4} \mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{NH}_{2} \mathrm{CONH}_{2}+\mathrm{C}_{5} \mathrm{H}_{12} \mathrm{N}_{2} \mathrm{O}_{2}$

Arginine Urea Ornithine If you excrete 95 mg of urea, what mass of arginine must have been used? What mass of ornithine must have been produced?

Urea is a white crystalline solid used as a fertilizer, in the pharmaceutical industry, and in the manufacture of certain polymer resins. Analysis of urea reveals that, by mass, it is 20.1$\%$ . carbon, 6.7$\%$ hydrogen, 46.5$\%$ nitrogen, and the balance oxygen.

(a) Find the empirical formula of urea.

(b) $\mathrm{A} 5.0 \mathrm{g} / \mathrm{L}$ solution of urea in water has an osmotic pressure of

2.04 $\mathrm{atm}$ , measured at $25^{\circ} \mathrm{C}$ . What is the molar mass and molecular

formula of urea?

Given the mass in grams of a substance in a reaction, calculate the mass in grams of another substance in the reaction.

Nitrogen dioxide and water react to produce nitric acid, HNO $_{3}$ and nitrogen oxide.

$$

3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g)

$$

a. How many grams of $\mathrm{H}_{2} \mathrm{O}$ are needed to react with $28.0 \mathrm{g}$ of $\mathrm{NO}_{2} ?$

b. How many grams of NO are produced from $15.8 \mathrm{g}$ of $\mathrm{NO}_{2} ?$

c. How many grams of HNO $_{3}$ are produced from $8.25 \mathrm{g}$ of $\mathrm{NO}_{2} ?$

Given the mass in grams of a substance in a reaction, calculate the mass in grams of another substance in the reaction.

Ammonia and oxygen react to form nitrogen and water.

$$

4 \mathrm{NH}_{3}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{N}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)

$$

a. How many grams of $\mathrm{O}_{2}$ are needed to react with $13.6 \mathrm{g}$ of $\mathrm{NH}_{3} ?$

b. How many grams of $\mathrm{N}_{2}$ can be produced when $6.50 \mathrm{g}$ of $\mathrm{O}_{2}$ reacts?

c. How many grams of $\mathrm{H}_{2} \mathrm{O}$ are formed from the reaction of $34.0 \mathrm{g}$ of $\mathrm{NH}_{3} ?$

Calculate the amount of water (in grams) that must be added to (a) $5.00 \mathrm{g}$ of urea $\left(\mathrm{NH}_{2}\right)_{2} \mathrm{CO}$ in the preparation of a 16.2 percent by mass solution, and (b) $26.2 \mathrm{g}$ of $\mathrm{Mg} \mathrm{Cl}_{2}$ in the preparation of a 1.5 percent by mass solution.

Urea $\left(\mathrm{H}_{2} \mathrm{NCONH}_{2}\right)$ is used extensively as a nitrogen source in fertilizers. It is produced commercially from the reaction of ammonia and carbon dioxide:

$$2 \mathrm{NH}_{3}(g)+\mathrm{CO}_{2}(g) \frac{\mathrm{Heat}}{\mathrm{Presure}} \mathrm{H}_{2} \mathrm{NCONH}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(g)$$

Ammonia gas at $223^{\circ} \mathrm{C}$ and $90 .$ atm flows into a reactor at a rate of $500 . \mathrm{L} / \mathrm{min}$ . Carbon dioxide at $223^{\circ} \mathrm{C}$ and 45 atm flows into the reactor at a rate of $600 . \mathrm{L} / \mathrm{min}$ . What mass of urea is produced per minute by this reaction assuming 100$\%$ yield?

Given the mass in grams of a substance in a reaction, calculate the mass in grams of another substance in the reaction.

Nitrogen gas reacts with hydrogen gas to produce ammonia.

$$

\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)

$$

If you have $3.64 \mathrm{g}$ of $\mathrm{H}_{2},$ how many grams of $\mathrm{NH}_{3}$ can be produced?

b. How many grams of $\mathrm{H}_{2}$ are needed to react with $2.80 \mathrm{g}$ of $\mathrm{N}_{2} ?$

c. How many grams of $\mathrm{NH}_{3}$ can be produced from $12.0 \mathrm{g}$ of $\mathrm{H}_{2} ?$

Ammonia is a principal nitrogen fertilizer. It is prepared by the reaction between hydrogen and nitrogen:

$$3 \mathrm{H}_{2}(g)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)$$

In a particular reaction, 6.0 moles of $\mathrm{NH}_{3}$ were produced. How many moles of $\mathrm{H}_{2}$ and how many moles of $\mathrm{N}_{2}$ were consumed to produce this amount of $\mathrm{NH}_{3} ?$

Ammonia is a principal nitrogen fertilizer. It is prepared by the reaction between hydrogen and nitrogen.

$$

3 \mathrm{H}_{2}(g)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)

$$

In a particular reaction, 6.0 moles of $\mathrm{NH}_{3}$ were produced. How many moles of $\mathrm{H}_{2}$ and how many moles of $\mathrm{N}_{2}$ were reacted to produce this amount of $\mathrm{NH}_{3} ?$