A cylinder with a movable piston contains 2.00 g of helium, He, at room temperature. More helium wa to the cylinder and the volume was adjusted so that the gas pressure remained the same. How many helium were added to the cylinder if the volume was changed from 2.00 L to 2.50 L ? (The temperatu held constant.) Express your answer with the appropriate units. • View Available Hint(s)
A cylinder with a movable piston contains 2.00 g of helium, He, at room temperature. More helium wa to the cylinder and the volume was adjusted so that the gas pressure remained the same. How many helium were added to the cylinder if the volume was changed from 2.00 L to 2.50 L ? (The temperatu held constant.) Express your answer with the appropriate units. • View Available Hint(s)
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 question 2 Part A, B, and C
![**Part C**
A cylinder with a movable piston contains 2.00 g of helium, He, at room temperature. More helium was added to the cylinder and the volume was adjusted so that the gas pressure remained the same. How many grams of helium were added to the cylinder if the volume was changed from 2.00 L to 2.50 L? (The temperature was held constant.)
**Express your answer with the appropriate units.**
\[
\begin{array}{|c|}
\hline
\textbf{mass of helium added} = \quad \boxed{\text{Value}} \quad \text{Units} \\
\hline
\end{array}
\]
**View Available Hint(s)**
---
*Note: This is a calculation question involving gas laws, specifically considering the conditions of constant pressure and temperature.*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fded90a0e-1aa2-42d3-8902-387fb21746ad%2F612d50ae-511f-4098-a470-51faefb5ff07%2Fnvc8hfh_processed.png&w=3840&q=75)
Transcribed Image Text:**Part C**
A cylinder with a movable piston contains 2.00 g of helium, He, at room temperature. More helium was added to the cylinder and the volume was adjusted so that the gas pressure remained the same. How many grams of helium were added to the cylinder if the volume was changed from 2.00 L to 2.50 L? (The temperature was held constant.)
**Express your answer with the appropriate units.**
\[
\begin{array}{|c|}
\hline
\textbf{mass of helium added} = \quad \boxed{\text{Value}} \quad \text{Units} \\
\hline
\end{array}
\]
**View Available Hint(s)**
---
*Note: This is a calculation question involving gas laws, specifically considering the conditions of constant pressure and temperature.*
![The Ideal Gas Law \((PV = nRT)\) describes the relationship among pressure \(P\), volume \(V\), temperature \(T\), and molar amount \(n\). When some of these variables are constant, the ideal gas law can be rearranged in different ways to take the following forms where \(k\) is a constant:
| Name | Expression | Constant |
|---------------|-------------|-----------|
| Boyle’s Law | \(PV = nRT = k\) | \(n\) and \(T\) |
| Charles's Law | \(\frac{V}{T} = \frac{nR}{P} = k\) | \(n\) and \(P\) |
| Avogadro's Law| \(\frac{V}{n} = \frac{RT}{P} = k\) | \(T\) and \(P\) |
**Figure:**
Illustration 1 of 1 shows a visual representation of a gas cylinder with a movable piston. Initially, the cylinder contains a volume of 3.00 L of chlorine gas. The piston is then pushed down, reducing the volume to 1.00 L.
**Part A**
A certain amount of chlorine gas was placed inside a cylinder with a movable piston at one end. The initial volume was 3.00 L, and the initial pressure of chlorine was 1.25 atm. The piston was pushed down to change the volume to 1.00 L. Calculate the final pressure of the gas if the temperature and number of moles of chlorine remain constant.
**Express your answer with the appropriate units.**
\[ P_{\text{final}} = \text{Value} \quad \text{Units} \]
**Part B**
In an air-conditioned room at 19.0 °C, a spherical balloon had a diameter of 50.0 cm. When taken outside on a hot summer day, the balloon expanded to 51.0 cm in diameter. What was the temperature outside in degrees Celsius? Assume that the balloon is a perfect sphere and that the pressure and number of moles of air molecules remains the same.
**Express your answer with the appropriate units.**
\[ \text{outside temperature} = \text{Value} \quad \text{Units} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fded90a0e-1aa2-42d3-8902-387fb21746ad%2F612d50ae-511f-4098-a470-51faefb5ff07%2Fx5wekrb_processed.png&w=3840&q=75)
Transcribed Image Text:The Ideal Gas Law \((PV = nRT)\) describes the relationship among pressure \(P\), volume \(V\), temperature \(T\), and molar amount \(n\). When some of these variables are constant, the ideal gas law can be rearranged in different ways to take the following forms where \(k\) is a constant:
| Name | Expression | Constant |
|---------------|-------------|-----------|
| Boyle’s Law | \(PV = nRT = k\) | \(n\) and \(T\) |
| Charles's Law | \(\frac{V}{T} = \frac{nR}{P} = k\) | \(n\) and \(P\) |
| Avogadro's Law| \(\frac{V}{n} = \frac{RT}{P} = k\) | \(T\) and \(P\) |
**Figure:**
Illustration 1 of 1 shows a visual representation of a gas cylinder with a movable piston. Initially, the cylinder contains a volume of 3.00 L of chlorine gas. The piston is then pushed down, reducing the volume to 1.00 L.
**Part A**
A certain amount of chlorine gas was placed inside a cylinder with a movable piston at one end. The initial volume was 3.00 L, and the initial pressure of chlorine was 1.25 atm. The piston was pushed down to change the volume to 1.00 L. Calculate the final pressure of the gas if the temperature and number of moles of chlorine remain constant.
**Express your answer with the appropriate units.**
\[ P_{\text{final}} = \text{Value} \quad \text{Units} \]
**Part B**
In an air-conditioned room at 19.0 °C, a spherical balloon had a diameter of 50.0 cm. When taken outside on a hot summer day, the balloon expanded to 51.0 cm in diameter. What was the temperature outside in degrees Celsius? Assume that the balloon is a perfect sphere and that the pressure and number of moles of air molecules remains the same.
**Express your answer with the appropriate units.**
\[ \text{outside temperature} = \text{Value} \quad \text{Units} \]
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