A balloon vendor at a street fair is using a tank of helium to fill her balloons. The tank has a volume of 126.0 L and a pressure of 127.0 atm at 25.0 °C. After a while she notices that the valve has not been closed properly. The pressure had dropped to 117.0 atm. (The tank is still at 25.0 °C.) 1st attempt l See Periodic Table O See Hint How many moles of gas has she lost? mol

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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**Scenario: Balloon Vendor's Helium Usage**

A balloon vendor at a street fair is using a tank of helium to fill her balloons. The tank has a volume of 126.0 L and a pressure of 127.0 atm at 25.0 °C. After a while, she notices that the valve has not been closed properly, and the pressure has dropped to 117.0 atm. (The tank is still at 25.0 °C.)

**Question:**

How many moles of gas has she lost?

**Response Box:**

[______] mol

**Additional Tools:**

- **See Periodic Table**
- **See Hint**

---

This scenario provides an opportunity for learners to apply the ideal gas law to determine the number of moles of helium lost due to the pressure decrease in the tank. The information given allows for calculations using the formula: 

\[
PV = nRT
\]

where \(P\) is pressure, \(V\) is volume, \(n\) is the number of moles, \(R\) is the ideal gas constant, and \(T\) is temperature in Kelvin.
Transcribed Image Text:**Scenario: Balloon Vendor's Helium Usage** A balloon vendor at a street fair is using a tank of helium to fill her balloons. The tank has a volume of 126.0 L and a pressure of 127.0 atm at 25.0 °C. After a while, she notices that the valve has not been closed properly, and the pressure has dropped to 117.0 atm. (The tank is still at 25.0 °C.) **Question:** How many moles of gas has she lost? **Response Box:** [______] mol **Additional Tools:** - **See Periodic Table** - **See Hint** --- This scenario provides an opportunity for learners to apply the ideal gas law to determine the number of moles of helium lost due to the pressure decrease in the tank. The information given allows for calculations using the formula: \[ PV = nRT \] where \(P\) is pressure, \(V\) is volume, \(n\) is the number of moles, \(R\) is the ideal gas constant, and \(T\) is temperature in Kelvin.
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