Initial Post Instructions: This Week We Are Studying The Ide ✓ Solved

Initial Post Instructionsthis Week We Are Studying The Ideal Gas Law

This week, we are studying the ideal gas law. In this discussion, you will be trying your hand at applying one of the ideal gas laws to a real world situation. Consider a situation that involves an ideal gas law and discuss how you would apply your chosen ideal gas law to the situation. Write your own ideal gas law problem based on this situation but DO NOT solve this yourself. A peer will solve the problem you wrote.

Sample Paper For Above instruction

Understanding the Ideal Gas Law and Its Application in Real-World Situations

The ideal gas law is a fundamental principle in chemistry that relates the pressure, volume, temperature, and amount of gas through the equation PV = nRT, where P represents pressure, V volume, n the number of moles, R the universal gas constant, and T the temperature in Kelvin. This law assumes the gas particles do not interact and occupy no volume, idealizing real gases only under specific conditions.

In practical applications, the ideal gas law enables scientists and engineers to predict the behavior of gases in various scenarios, such as designing chemical reactors, calculating gas storage capacities, or understanding atmospheric phenomena. To effectively apply the ideal gas law to a real-world situation, it is essential to understand the context, the given quantities, and which variables need to be determined or predicted.

For instance, consider a scenario involving the transportation of natural gas in a pipeline. Suppose a pipeline contains 5000 liters of natural gas at a temperature of 300 Kelvin and a pressure of 2 atmospheres. The engineer needs to determine how much gas (in moles) is present in the pipeline. To address this, the ideal gas law can be rearranged to solve for n:

n = PV / RT

Where:

  • P = 2 atm
  • V = 5000 L
  • R = 0.0821 L·atm/(mol·K)
  • T = 300 K

Substituting these values into the equation:

n = (2 atm × 5000 L) / (0.0821 L·atm/(mol·K) × 300 K)

Calculating the numerator and denominator gives:

n = 10000 / 24.63 ≈ 406 mol

This example illustrates how the ideal gas law can be applied to determine the amount of gas in a real-world context, which is critical for safety, efficiency, and regulatory compliance.

Now, based on this understanding, I will create a problem that applies the ideal gas law to a relevant scenario but will leave it unsolved for a peer to analyze and solve.

Ideal Gas Law Problem: A balloon containing helium at a temperature of 290 Kelvin has a volume of 8 liters and an internal pressure of 1.2 atmospheres. If the balloon is heated to 310 Kelvin while the amount of helium remains constant, what will be the new pressure inside the balloon, assuming it behaves ideally? (Use R = 0.0821 L·atm/(mol·K)).

References

  • Chang, R. (2010). Chemistry (10th ed.). McGraw-Hill Education.
  • Tro, N. J. (2017). Chemistry: A Molecular Approach. Pearson Education.
  • Zumdahl, S. S., & Zumdahl, S. A. (2014). Chemistry: An Atoms First Approach. Cengage Learning.
  • Brown, T. L., LeMay, H. E., Bursten, B. E., Murphy, C., & Woodward, A. (2014). Chemistry: The Central Science. Pearson.
  • Laidler, K. J., Meiser, J. H., & Sanctuary, B. C. (1999). Physical Chemistry. Houghton Mifflin.
  • McQuarrie, D. A., & Simon, J. D. (1997). Physical Chemistry: A Molecular Approach. University Science Books.
  • Atkins, P., & de Paula, J. (2010). Physical Chemistry. Oxford University Press.
  • Petrucci, R. H., Herring, F. G., Madura, J. D., & Bissonnette, C. (2017). General Chemistry: Principles & Modern Applications. Pearson.
  • Steinfeld, J. I., Francisco, J., & Hase, W. L. (2009). Chemical Kinetics and Dynamics. Prentice Hall.
  • Moore, J. W., & Pearson, D. (2006). Kinetics and Mechanism. Wiley.

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