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Get Full Access to Introductory Chemistry - 5 Edition - Chapter 11 - Problem 121p
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# Consider the reaction:2 SO2(g) + O2(g) ? 2 SO3(g)A reaction flask initially contains

ISBN: 9780321910295 34

## Solution for problem 121P Chapter 11

Introductory Chemistry | 5th Edition

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Problem 121P

PROBLEM 121P

Consider the reaction:

2 SO2(g) + O2(g) → 2 SO3(g)

A reaction flask initially contains 0.10 atm of SO2 and 0.10 atm of O2. What is the total pressure in the flask once the limiting reactant is completely consumed? Assume a constant temperature and volume and a 100% reaction yield.

Step-by-Step Solution:
Step 1 of 3

Solution 121P

Here, we are going to calculate the total pressure in the given reaction flask once the limiting reactant is completely consumed.

Step1:

The given reaction is:

2SO2(g) + O2(g) → 2SO3(g)

From the above equation, it is clear that 2 moles of SO2 requires 1 mole of O2 for complete reaction.

Now, at constant temperature and volume, the pressure(p) of a gas is directly proportional to the number of moles(n).

Thus,

p ∝ n

Now, if p1, n1 are the pressure and number of moles of a gas and p2, n2 are the volume and number of moles of another gas , then,

p1 = kn1

p2 = kn2

Combining the two equations, we get, p1 / n1 = p2 / n2        -----(1)

Step2:

Let, p1, n1 are the pressure and number of moles of SO2 and p2, n2 are the volume and number of moles of O2 , then, pressure of O2 required to react with 0.10 atm pressure of SO2 is given by:

p2 = (p1 x n2) / n1

= (0.10 atm x 1 mol) / 2 mol

= 0.05 atm

But we have oxygen at 0.10 atm pressure, i.e., the pressure of O2 is in excess. Thus, SO2 acts as a limiting reactant.

Step3:

Pressure of O2 after the reaction is complete = initial pressure - pressure required in the reaction

= 0.10 atm - 0.05 atm

= 0.05 atm

Again, since 2 moles of SO2 produces 2 moles of SO3

Therefore, pressure of SO3 after reaction is complete = pressure of SO2 consumed = 0.10 atm.

Thus,

Total pressure in the flask after the limiting reactant is completely consumed = Pressure of SO3 + pressure of remaining O2

= (0.10 + 0.05) atm

= 0.15 atm.

Total pressure in the flask once the limiting reactant is completely consumed is 0.15 atm.

Step 2 of 3

Step 3 of 3

##### ISBN: 9780321910295

This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. This full solution covers the following key subjects: reaction, atm, flask, initially, constant. This expansive textbook survival guide covers 19 chapters, and 2046 solutions. Since the solution to 121P from 11 chapter was answered, more than 1431 students have viewed the full step-by-step answer. The full step-by-step solution to problem: 121P from chapter: 11 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The answer to “Consider the reaction:2 SO2(g) + O2(g) ? 2 SO3(g)A reaction flask initially contains 0.10 atm of SO2 and 0.10 atm of O2. What is the total pressure in the flask once the limiting reactant is completely consumed? Assume a constant temperature and volume and a 100% reaction yield.” is broken down into a number of easy to follow steps, and 48 words.

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Consider the reaction:2 SO2(g) + O2(g) ? 2 SO3(g)A reaction flask initially contains