Urea (H2 NCONH2) is used extensively as a nitrogen source in...

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: $$ 2 \mathrm{NH}_{3}(g)+\mathrm{CO}_{2}(g) \underset{\text { Pressure }}{\text { Heat }}{\mathrm{H}}_{2} \mathrm{NCONH}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(g) $$ 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?

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:
$$
2 \mathrm{NH}_{3}(g)+\mathrm{CO}_{2}(g) \underset{\text { Pressure }}{\text { Heat }}{\mathrm{H}}_{2} \mathrm{NCONH}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(g)
$$
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?

Key Concepts

Stoichiometry

Stoichiometry is the study of the quantitative relationships between reactants and products in a chemical reaction. In this context, it involves using the balanced chemical equation for the production of urea to determine the proportional amounts of ammonia and carbon dioxide required, and subsequently, the amount of urea produced, based on the mole ratios dictated by the equation.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first during a chemical reaction, thus limiting the extent of the reaction and determining the maximum amount of product that can be formed. In processes where reactants are supplied in different amounts, identifying the limiting reactant is crucial for calculating the yield of the desired product.

Ideal Gas Law

The Ideal Gas Law (PV = nRT) relates the pressure, volume, temperature, and moles of a gas. In reactions involving gaseous reactants under specified conditions, it is used to convert the given flow rates (volumes per minute) at certain pressures and temperatures into the number of moles, which is necessary for subsequent stoichiometric calculations.

Molar Mass Conversion

Molar mass conversion is the process of translating the amount of a substance in moles to its mass using the molar mass (grams per mole). Once the number of moles of urea produced is determined using stoichiometry and the limiting reactant concept, multiplying by the molar mass of urea yields the mass of urea produced per minute.

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