Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Mole Concept
Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can b…
Question
**Problem Statement: Ideal Gas Law Application** Calculate the number of moles of \( \text{N}_2 \) that would take up a volume of 5.25 L with a pressure of 4.80 atm at 298 K. **Answer:** [Provide your answer here] **Discussion:** This question requires using the Ideal Gas Law, which is represented by the formula: \[ PV = nRT \] Where: - \( P \) is the pressure (in atm), - \( V \) is the volume (in L), - \( n \) is the number of moles, - \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), - \( T \) is the temperature (in K). To find the number of moles, rearrange the formula to solve for \( n \): \[ n = \frac{PV}{RT} \] By substituting the given values: \[ P = 4.80 \text{ atm} \] \[ V = 5.25 \text{ L} \] \[ R = 0.0821 \text{ L}·\text{atm/mol}·\text{K} \] \[ T = 298 \text{ K} \] This equation will yield the number of moles of nitrogen gas \( \text{N}_2 \).
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Transcribed Image Text:**Problem Statement: Ideal Gas Law Application** Calculate the number of moles of \( \text{N}_2 \) that would take up a volume of 5.25 L with a pressure of 4.80 atm at 298 K. **Answer:** [Provide your answer here] **Discussion:** This question requires using the Ideal Gas Law, which is represented by the formula: \[ PV = nRT \] Where: - \( P \) is the pressure (in atm), - \( V \) is the volume (in L), - \( n \) is the number of moles, - \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), - \( T \) is the temperature (in K). To find the number of moles, rearrange the formula to solve for \( n \): \[ n = \frac{PV}{RT} \] By substituting the given values: \[ P = 4.80 \text{ atm} \] \[ V = 5.25 \text{ L} \] \[ R = 0.0821 \text{ L}·\text{atm/mol}·\text{K} \] \[ T = 298 \text{ K} \] This equation will yield the number of moles of nitrogen gas \( \text{N}_2 \).
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