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Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please answer B.) thank you  

# Core Chemistry Skill: Using the Combined Gas Law ## Understanding the Combined Gas Law All pressure–volume–temperature relationships for gases can be combined into a single equation known as the **combined gas law**. This expression is useful when examining the effects of changes in two of these variables on the third, provided the amount of gas (number of moles) remains constant. To apply the combined gas law correctly, temperatures must always be expressed in kelvin. The formula for the combined gas law is: \[ \frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2} \] ### Example Problem In this exercise, the volume of a gas initially occupying a certain space is calculated after some changes in its conditions. - **Given**: - Initial volume (\(V_1\)): 4.20 L - Initial pressure (\(P_1\)): 365 mmHg - Initial temperature (\(T_1\)): 20.0 °C - **Final Conditions**: - Final volume (\(V_2\)): 2.60 L - Final temperature (\(T_2\)): 31 °C The task is to calculate the new pressure (\(P_2\)) inside the container assuming no change in the amount of gas. #### Calculation Results - **Calculated Volume**: \(V_2\) was determined to be 38.1 L. The difference in rounding or significant figures may account for discrepancies. - **Feedback**: The relationship between pressure, volume, and temperature is depicted accurately as air pressure decreases with altitude, causing volume changes inversely as temperature influences volume reductions. ### Solution to Part B The new pressure (\(P_2\)) is computed as follows: - **Pressure (P<sub>2</sub>)**: 573.94 mmHg This value is derived using the combined gas law, considering all conversions and adjustments for the change in conditions. ### Key Understanding: These exercises showcase how changes in conditions such as volume and temperature affect gas pressure, relying on the combined gas law to predict these changes under constant mole quantities.
Transcribed Image Text:# Core Chemistry Skill: Using the Combined Gas Law ## Understanding the Combined Gas Law All pressure–volume–temperature relationships for gases can be combined into a single equation known as the **combined gas law**. This expression is useful when examining the effects of changes in two of these variables on the third, provided the amount of gas (number of moles) remains constant. To apply the combined gas law correctly, temperatures must always be expressed in kelvin. The formula for the combined gas law is: \[ \frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2} \] ### Example Problem In this exercise, the volume of a gas initially occupying a certain space is calculated after some changes in its conditions. - **Given**: - Initial volume (\(V_1\)): 4.20 L - Initial pressure (\(P_1\)): 365 mmHg - Initial temperature (\(T_1\)): 20.0 °C - **Final Conditions**: - Final volume (\(V_2\)): 2.60 L - Final temperature (\(T_2\)): 31 °C The task is to calculate the new pressure (\(P_2\)) inside the container assuming no change in the amount of gas. #### Calculation Results - **Calculated Volume**: \(V_2\) was determined to be 38.1 L. The difference in rounding or significant figures may account for discrepancies. - **Feedback**: The relationship between pressure, volume, and temperature is depicted accurately as air pressure decreases with altitude, causing volume changes inversely as temperature influences volume reductions. ### Solution to Part B The new pressure (\(P_2\)) is computed as follows: - **Pressure (P<sub>2</sub>)**: 573.94 mmHg This value is derived using the combined gas law, considering all conversions and adjustments for the change in conditions. ### Key Understanding: These exercises showcase how changes in conditions such as volume and temperature affect gas pressure, relying on the combined gas law to predict these changes under constant mole quantities.
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