When nitrogen dioxide ( NO2 ) from car exhaust combines with water in the air, it forms nitric a

When nitrogen dioxide ( NO2 ) from car exhaust combines with...

When nitrogen dioxide ( $\mathrm{NO}_{2}$ ) from car exhaust combines with water in the air, it forms nitric acid (HNO $_{3}$ ), which causes acid rain, and nitrogen oxide. (7.3,7.6,7.7) a. Write the balanced chemical equation. b. How many moles of each product are produced from 0.250 mole of $\mathrm{H}_{2} \mathrm{O} ?$ c. How many grams of HNO $_{3}$ are produced when $60.0 \mathrm{g}$ of NO, completely reacts? d. How many grams of $\mathrm{NO}_{2}$ are needed to form $75.0 \mathrm{g}$ of $\mathrm{HNO}_{3} ?$

When nitrogen dioxide ( $\mathrm{NO}_{2}$ ) from car exhaust combines with water in the air, it forms nitric acid (HNO $_{3}$ ), which causes acid rain, and nitrogen oxide. (7.3,7.6,7.7)
a. Write the balanced chemical equation.
b. How many moles of each product are produced from 0.250 mole of $\mathrm{H}_{2} \mathrm{O} ?$
c. How many grams of HNO $_{3}$ are produced when $60.0 \mathrm{g}$ of NO, completely reacts?
d. How many grams of $\mathrm{NO}_{2}$ are needed to form $75.0 \mathrm{g}$ of $\mathrm{HNO}_{3} ?$

Key Concepts

Mole-to-Mass Conversion

Mole-to-mass conversion involves using the molar mass of a substance, which is the mass of one mole of its particles, to convert between the number of moles and the mass of a substance. This conversion is essential in stoichiometry to determine how much of a substance is needed or produced in a given reaction.

Stoichiometric Coefficients

Stoichiometric coefficients, appearing in a balanced chemical equation, indicate the relative proportion of moles of reactants and products involved in the reaction. These coefficients are used to establish the mole ratio, which is critical for calculating the amounts of reactants needed or products formed in a chemical reaction.

Balanced Chemical Equation

A balanced chemical equation represents the conservation of mass by ensuring that the number of atoms for each element is the same on both sides of the reaction. It serves as the foundation for stoichiometry calculations since it provides the mole ratios needed to predict how much of each reactant is required and how much product will be formed.

Mole Concept

The mole concept is a fundamental principle in chemistry that allows chemists to count atoms, molecules, or ions by weighing amounts of substance. It is the bridge between the microscopic world of atoms and the macroscopic amounts of substances used in laboratory measurements, forming the basis for stoichiometric conversions between mass and number of particles.

Transcript

00:01 For this problem, it states that we have nitrogen dioxide and the nitrogen dioxide is going to react with water, producing nitric acid and it says nitrogen oxide.

00:16 So it wasn't specific, but i assume they meant nitrogen monoxide.

00:22 So we'll put nitrogen monoxide right here.

00:25 Then we see that we have two hydrogens and only one hydrogen, so we need to put that two right there.

00:30 Then we have two nitrogen plus another nitrogen there, so three nitrogen, so we need to put a three right there.

00:39 Now the chemical equation is balanced.

00:43 It then asks how many moles of each product can be produced from 0 .250 moles of water.

00:50 So we're going to start with 0 .250 moles of water and assume that we have sufficient nitrogen dioxide, although not explicit in the problem, and figure out how much, how many moles, of nitric acid we can make from 0 .25 moles of water and then in a subsequent calculation how many moles of no we can make with 0 .25 moles of water.

01:14 We see that the relationship between moles of water and moles nitric acid is 2 to 1.

01:23 So for every mole water we'll make 2 moles nitric acid so we'll make twice the amount .5 .00 moles nitric acid.

01:31 Then the multiple relation for water to nitrogen monoxide is one to one.

01:38 So we will end up with the same number of moles of nitrogen monoxide as reacted of water.

01:47 Then for the next question, it asks how many grams of nitric acid can be produced from a particular mass of nitrogen dioxide.

01:57 That mass is 60 .0 grams nitrogen dioxide.

02:01 So this is going to require us to go from grams of nitrogen dioxide...

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