In the body, the amino acid glycine (C2 H5 NO2) reacts according to the following equation: (9.3

step 1 Here in this problem given this reaction and we have to find out how many grams of O2 are needed

In the body, the amino acid glycine (C2 H5 NO2) reacts...

In the body, the amino acid glycine $\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2}\right)$ reacts according to the following equation: (9.3) $2 \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2}(a q)+3 \mathrm{O}_{2}(g) \longrightarrow$ Glycine $\quad 3 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CH}_{4} \mathrm{~N}_{2} \mathrm{O}(a q)$ UreaIn the body, the amino acid glycine $\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2}\right)$ reacts according to the following equation: (9.3) $2 \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2}(a q)+3 \mathrm{O}_{2}(g) \longrightarrow$ Glycine $\quad 3 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CH}_{4} \mathrm{~N}_{2} \mathrm{O}(a q)$ Urea a. How many grams of $\mathrm{O}_{2}$ are needed to react with $15.0 \mathrm{~g}$ of glycine? b. How many grams of urea are produced from $15.0 \mathrm{~g}$ of glycine? c. How many grams of $\mathrm{CO}_{2}$ are produced from $15.0 \mathrm{~g}$ of glycine?

In the body, the amino acid glycine $\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2}\right)$ reacts according to the following equation: (9.3)
$2 \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2}(a q)+3 \mathrm{O}_{2}(g) \longrightarrow$
Glycine $\quad 3 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CH}_{4} \mathrm{~N}_{2} \mathrm{O}(a q)$
UreaIn the body, the amino acid glycine $\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2}\right)$ reacts according to the following equation: (9.3)
$2 \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{2}(a q)+3 \mathrm{O}_{2}(g) \longrightarrow$
Glycine $\quad 3 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CH}_{4} \mathrm{~N}_{2} \mathrm{O}(a q)$
Urea
a. How many grams of $\mathrm{O}_{2}$ are needed to react with $15.0 \mathrm{~g}$ of glycine?
b. How many grams of urea are produced from $15.0 \mathrm{~g}$ of glycine?
c. How many grams of $\mathrm{CO}_{2}$ are produced from $15.0 \mathrm{~g}$ of glycine?

Key Concepts

Stoichiometry

Stoichiometry involves using a balanced chemical equation to determine the quantitative relationships between the amounts of reactants and products. It is the backbone of calculations in chemical reactions, enabling one to convert between masses, moles, and particle numbers based on the mole ratios provided by the stoichiometric coefficients in the equation.

Molar Mass

Molar mass is the mass of one mole of a substance, usually expressed in grams per mole, and serves as the conversion factor between the mass of a substance and the number of moles. It is calculated by summing the atomic masses of the elements in a compound, allowing one to convert given masses into moles for use in stoichiometric calculations.

Mole Ratio from a Balanced Equation

The mole ratio is derived from the coefficients in a balanced chemical equation, representing the proportion of moles of one substance that reacts with or is produced relative to another. This ratio is crucial for converting from the amount of one substance to the amount of another in a reaction, ensuring that the law of conservation of mass is followed.

Mass-to-Mole and Mole-to-Mass Conversions

These conversions are fundamental in stoichiometry, where one uses the molar mass of a substance to convert a given mass into moles, and vice versa. This step is essential for applying mole ratios from the balanced equation, linking the measurable quantities in grams to the theoretical molar proportions in the reaction.

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