Consider the following gas phase reaction: 4 NH3(g)+ 5 O2(g) →4 NO(g)+6 H2 O(g) . If 6.98 liters

step 1 Hi there. This is a gas stoichiometry problem. So for any stoichiometry problem, we of course ne

Consider the following gas phase reaction: 4 NH3(g)+ 5 O2(g)...

Consider the following gas phase reaction: $4 \mathrm{NH}_{3}(g)+$ $5 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) .$ If 6.98 liters of $\mathrm{O}_{2}(\mathrm{g})$ gas at $129^{\circ} \mathrm{C}$ and 0.836 atm are reacted, what volume of $\mathrm{H}_{2} \mathrm{O}(\mathrm{g})$ will be produced if it is collected at $74^{\circ} \mathrm{C}$ and 0.630 atm?

Consider the following gas phase reaction: $4 \mathrm{NH}_{3}(g)+$ $5 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) .$ If 6.98 liters of $\mathrm{O}_{2}(\mathrm{g})$ gas at
$129^{\circ} \mathrm{C}$ and 0.836 atm are reacted, what volume of $\mathrm{H}_{2} \mathrm{O}(\mathrm{g})$ will be produced if it is collected at $74^{\circ} \mathrm{C}$ and 0.630 atm?

Key Concepts

Reaction Stoichiometry

This concept involves using a balanced chemical equation to relate the moles of reactants to the moles of products. It is essential in determining how much product forms from a given quantity of a reactant by applying the mole ratios indicated by the coefficients in the balanced equation.

Ideal Gas Law

The ideal gas law (PV = nRT) relates the pressure, volume, temperature, and number of moles of a gas. It is fundamental in solving problems involving gases under different conditions, allowing one to convert between volume and moles as well as to adjust for changes in pressure and temperature.

Temperature Conversion

Temperature conversion, specifically converting temperatures from Celsius to Kelvin, is crucial in gas law calculations. Since the ideal gas law requires absolute temperature, converting Celsius into Kelvin by adding 273.15 ensures that calculations are accurate.

Transcript

00:01 Hi there.

00:02 This is a gas stoichiometry problem.

00:04 So for any stoichiometry problem, we of course need a balanced equation.

00:08 So the first thing i'm going to do is copy that balanced equation from the book.

00:15 So we had 4nh3 plus 502 produces 4n0 plus 6h2.

00:34 And all of these reactants and products are gases.

00:42 We are given 6 .98 liters of oxygen to begin with.

00:49 This oxygen is at 129 degrees celsius and a pressure of 0 .836 atmospheres.

01:04 I'm going to go ahead and change this temperature into kelvin since this is a gas problem, i know temperatures have to be in kelvin to do calculations.

01:15 I'm going to get 402 kelvin.

01:19 What we want to find out in this problem is how many liters we're going to collect of the water.

01:25 However, the water is not collected under the same conditions.

01:29 The water is going to be collected when it is now 74 degrees celsius and a pressure of 0 .630 atmospheres.

01:42 Again, changing my temperature to kelvin, i get 347.

01:52 That is all of the information from the problem.

01:55 Let's think about how to solve this.

01:58 I would like to use the volume ratio and the balanced equation to convert from oxygen to water.

02:04 However, before i can do that, i need to make sure that the volumes of both of these gases are at the same temperature and pressure.

02:13 The first thing i'm going to do, therefore, is to convert the volume of oxygen that i'm starting with to the volume that i would have under the conditions that the water's being collected at.

02:26 In other words, it's a combined gas law problem where i want to take my initial conditions for the oxygen and convert it to the conditions of pressure and temperature that the water's collected at.

02:45 I'm going to go ahead and plug all my values into this...

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