Nitrogen dioxide and water react to produce nitric acid, HNO3, and nitrogen oxide. 3 NO2(g)+H2 O

step 1 This question asks you to convert grams of a react into grams of another react into product. To

Nitrogen dioxide and water react to produce nitric acid,...

Nitrogen dioxide and water react to produce nitric acid, $\mathrm{HNO}_{3}$, 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 required to react with $28.0 \mathrm{~g}$ of $\mathrm{NO}_{2}$ ? b. How many grams of $\mathrm{NO}$ are produced from $15.8 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O}$ ? c. How many grams of $\mathrm{HNO}_{3}$ are produced from $8.25 \mathrm{~g}$ of $\mathrm{NO}_{2}$ ?

Nitrogen dioxide and water react to produce nitric acid, $\mathrm{HNO}_{3}$, 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 required to react with $28.0 \mathrm{~g}$ of $\mathrm{NO}_{2}$ ?
b. How many grams of $\mathrm{NO}$ are produced from $15.8 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O}$ ?
c. How many grams of $\mathrm{HNO}_{3}$ are produced from $8.25 \mathrm{~g}$ of $\mathrm{NO}_{2}$ ?

Key Concepts

Mass-to-Mass Conversions

Mass-to-mass conversions involve converting an initial mass of a reactant to the mass of a product using the mole concept. This process typically includes converting the given mass to moles using the substance’s molar mass, applying the stoichiometric ratios from the balanced equation, and then converting the resulting moles of the desired product back to grams using its molar mass.

Mole Concept

The mole concept is a fundamental chemical concept used to connect the atomic scale to the macroscopic scale. It allows chemists to count particles by weighing grams, as one mole of any substance contains Avogadro's number of particles. This concept is crucial for converting between masses of substances and the number of moles, which is required in stoichiometric calculations.

Molar Mass

Molar mass is defined as the mass of one mole of a substance, typically expressed in grams per mole. It serves as a conversion factor between the mass of a substance and the number of moles, enabling calculations that relate the quantity of matter to the molar ratios specified in the balanced chemical equation.

Balanced Chemical Equations

A balanced chemical equation represents the conservation of mass, showing the relative number of moles of each reactant and product involved in a chemical reaction. The coefficients indicate the stoichiometric ratios needed for the reaction to occur, and they are essential for converting between different substances in the reaction.

Stoichiometry

Stoichiometry is the area of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It involves using the balanced chemical equation to calculate the amount of any substance, given the amount of another, by relating their moles through the coefficients in the equation.

Transcript

Please give Ace some feedback