**Chemistry Problem: Determining Partial Pressure in a Gas Mixture**A mixture of **carbon dioxide** and **helium** gases, in a **7.15 L** flask at **50°C**, contains **13.4 grams** of **carbon dioxide** and **2.97 grams** of **helium**. The partial pressure of helium in the flask is ______ atm and the total pressure in the flask is **0.327 atm**.**Instructions:**- Use the ideal gas law and relevant values if needed for this question.**Controls:**- **Submit Answer** (Orange Button)- **Try Another Version** (Gray Button)- You have 1 item attempt remaining**Note:**To access important Chemistry values for calculations, refer to the **References** section.(End of transcription)**Explanation for Educational Context:**This problem involves calculating the partial pressure of a specific gas in a gas mixture using the details provided. Students are expected to apply their knowledge of gas laws, specifically the ideal gas law (PV = nRT), to determine the unknown partial pressure of helium. The total pressure and conditions of the gas mixture are given to assist in the completion of this task.

We can use ideal gas equation to calculate the partial pressure of each gas. The ideal gas equation…

A mixture of carbon dioxide and helium gases, in a 7.15 L flask at 50 °C, contains 13.4 grams of carbon dioxide and 0.327 grams of helium. The partial pressure of helium in the flask is atm and the total pressure in the flask is atm.

A mixture of carbon dioxide and helium gases, in a 7.15 L flask at 50 °C, contains 13.4 grams of carbon dioxide and 0.327 grams of helium. The partial pressure of helium in the flask is atm and the total pressure in the flask is atm.

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...

See similar textbooks

Related questions

Q: A mixture of helium, nitrogen and oxygen has a total pressure of 755 mm Hg. The partial pressures of…

Q: A mixture of argon and krypton gases, in a 9.88 L flask at 13 °C, contains 6.20 grams of argon and…

Q: The pressure of this gas sample

A: Given data - T = 6 oC = 279 K V = 22.30 L n = 1.19 mol Thus

Q: An 8 liter container at 30 C is filled with 14.0 g of neon gas and 8.0 g of helim gas. Calculate the…

A: Given : Mass of Ne = 14.0 g Mass of He = 8.0 g Temperature = 30 oC Volume = 8 L To calculate :-…

Q: In a 2.29 L flask, there are two gases (gas 1 and gas 2). There is 2.13 L of gas 1, with 3.7 bars of…

A: In order to find the final pressure of the gas mixture, we need to use the Ideal Gas Law, which…

Q: A sealed canister holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of…

A: According to Dalton's law of partial pressures, the total pressure in a system is estimated by the…

Q: A mixture of argon and helium gases is maintained in a 9.63 L flask at a pressure of 2.57 atm and a…

A: Ideal gas equation: where, P= pressure of the gas V= volume of the gas n=number of moles of the gas…

Q: A mixture of oxygen and neon gases, in a 7.03 L flask at 44 °C, contains 1.91 grams of oxygen and…

A: Given that : Volume of flask (V) = 7.03 L Temperature (T) = 44°C = 317 K Mass of Oxygen = 1.91 g…

Q: A mixture of oxygen and neon gases is maintained in a 8.18 L flask at a pressure of 2.03 atm and a…

A: Assume that the mixture is an Ideal gas and apply the Ideal gas equation.P is the total pressureV is…

Q: Samples of chlorine, methane, and ammonia gas are stored at 25°C and 1 atm. Each sample contains 1…

A: Each gas is stored at 25oC and 1atm No of moles of each gas =1

Q: Follow the rules of significant digits. A sample of carbon dioxide gas, CO2, has a volume 2754 mL, a…

Q: 5. A reaction yields 5.0 L of nitrogen monoxide. The volume is measured at 20°C and at a pressure of…

A: Ideal gases are hypothetical gases which do have real existence. A gas can behave ideally at low…

Q: 1.33 mol sample of neon gas at a temperature of 9.00 °C is found to occupy a volume of 29.3 liters.…

A: The number of moles of the neon gas sample is .The temperature is .The volume is .To calculate the…

Q: A mixture of helium and argon gases is maintained in a 9.15 L flask at a pressure of 3.19 atm and a…

A: Given that Pressure of gas mixture = P = 3.19 atm Volume = 9.15L Temperature of gas = 38°C =…

Q: thireen. A mixture of gases is made up of nitrogen, methane and oxygen. If the partial pressures…

Q: 5. A reaction yields 3.0 L of nitrogen gas. The volume is measured at 119°C and at a pressure of…

Q: 132.0 g of chlorine gas (Cl2) and 24.0 g of helium (He) are mixed in a container with a total…

A: Given, Mass of. Cl2 = 132 g Molar mass of Cl2 = 71 g/mol Moles = mass/MM = 132/71 = 1.86 mol…

Q: The pressure of a sample of argon gas was increased from 3.54 atm to 8.38 atm at constant…

A: Above question is based on Boyle's law i.e at constant temperature and for same number of moles of…

Q: A mixture of methane and oxygen gases, in a 7.82 L flask at 68 °C, contains 3.36 grams of methane…

Q: A sample of helium gas at a pressure of 727 torr and a temperature of 23.8°C, occupies a volume of…

Q: A 7.53 L container of oxygen gas at 12.1 °C is heated to 87.9 °C. Assuming that the volume of the…

Q: A balloon containing 0.75 mol of nitrogen gas has a volume of 16.8 L. If the amount of nitrogen in…

Q: A 2.68 L container of oxygen gas at 27.9 °C is heated to 46.8 °C. Assuming that the volume of the…

Q: 1.19 mol sample of neon gas at a temperature of 12.0 °C is found to occupy a volume of 24.3 liters.…

Q: A mixture of helium and carbon dioxide gases, at a total pressure of 920 mm Hg, contains 1.38 grams…

A: Given: Total Pressure of the mixture(Pt)= 920mmHg Mass of Helium gas = 1.38 g Mass of Carbon dioxide…

Q: A mixture of oxygen and neon gases is maintained in a 5.98 L flask at a pressure of 2.08 atm and a…

Q: A mixture of xenon and hydrogen gases, at a total pressure of 821 mm Hg, contains 16.6 grams of…

Q: A mixture of neon and argon gases, in a 7.40L flask at 48 °C, contains 1.63 grams of neon and 11.1…

A: Given :- mass of Neon = 1.63 g mass of Argon = 11.1 g volume = 7.40 L temperature = 48°C To be…

Q: An inflated balloon has a volume of 151 L at sea level (1.00 atm), and is allowed to ascend until…

A: Given: The initial volume (V1) is 151 L The initial pressure (P1) is 1.00 atm The initial…

Q: 103.0 g of chlorine gas (Cl2) and 23.0 g of helium (He) are mixed in a container with a total…

Q: A mixture of krypton and hydrogen gases is maintained in a 9.48 L flask at a pressure of 2.25 atm…

Q: A mixture of xenon and hydrogen gases at a total pressure of 965 mm Hg contains xenon at a partial…

A: Given-> Total pressure (P) = 965 mmHg Partial pressure of xenon (Xxe) = 313 mmHg Weight of Xe =…

Q: A 2.00 L sample of helium originally at 25 oC and a pressure of 745 torr is allowed to expand to a…

A: In all the gas laws (Boyle's, Charles' and Gay-Lussac's Law), pressure (P) and volume (V) remain in…

Q: An ideal gas is placed into a sealed container with a fixed volume. The initial temperature and…

A: Ideal gas equation: PV = nRT p----> pressure of gas V----> volume of gas n-----> number of…

Q: 1.47 mol sample of helium gas at a temperature of 26.0 °C is found to occupy a volume of 20.6…

A: Given :- Number of moles of gas = n = 1.47 moles temperature of gas = T = 26 0C = 26 +273.15 =…

Q: A mixture of oxygen and krypton gases, in a 8.75 L flask at 59 °C, contains 10.6 grams of oxygen and…

A: Given,The mass of Oxygen gas = 10.6 gThe mass of krypton gas = 14.6 gVolume of the flask = 8.75…

Q: to access important values if needed for this question. A mixture of helium and methane gases, in a…

A: Gases helium and methane is behave as a ideal gas - Ideal gas law equation is PV = nRT Where , P is…

Q: A mixture of hydrogen and carbon dioxide gases, in a 6.09 L flask at 31 °C, contains 0.236 grams of…

A: The formula of partial pressure of any gas pi can be given by---------------- pi = Ptotal × xi where…

Q: A mixture of oxygen and carbon dioxide gases is maintained in a 5.57 L flask at a pressure of 2.73…

A: The objective of the question is to find the mass of carbon dioxide in a mixture of gases, given the…

Q: A mixture of krypton and methane gases is maintained in a 6.32 L flask at a pressure of 3.01 atm and…

A: Total number of moles present in the mixture can be calculated using Ideal gas equation as follows,

Q: A sample of helium gas at a pressure of 673 torr and a temperature of 24.8 celcius , occupies a…

Q: A student collects 122. mL of hydrogen gas at 23.8 °C. The pressure of the hydrogen gas was…

Q: At 58 C, the volume of a gas is 53.2 mL. At the same pressure, its volume is 154 mL at what…

A: Charles law: At constant pressure, the volume of a fixed mass of a gas is directly proportional to…

Q: The atmosphere in a sealed diving bell contained oxygen and helium. If the gas mixture has 0.170 atm…

A: Given: The total pressure of the gas mixture = 2.90 atm The pressure of oxygen in the mixture =…

Q: A mixture of oxygen and krypton gases, in a 7.91 L flask at 41 °C, contains 8.74 grams of oxygen and…

Concept explainers

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 be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

**Chemistry Problem: Determining Partial Pressure in a Gas Mixture**

A mixture of **carbon dioxide** and **helium** gases, in a **7.15 L** flask at **50°C**, contains **13.4 grams** of **carbon dioxide** and **2.97 grams** of **helium**. The partial pressure of helium in the flask is ______ atm and the total pressure in the flask is **0.327 atm**.

**Instructions:**
- Use the ideal gas law and relevant values if needed for this question.

**Controls:**
- **Submit Answer** (Orange Button)
- **Try Another Version** (Gray Button)
- You have 1 item attempt remaining

**Note:**
To access important Chemistry values for calculations, refer to the **References** section.

(End of transcription)

**Explanation for Educational Context:**
This problem involves calculating the partial pressure of a specific gas in a gas mixture using the details provided. Students are expected to apply their knowledge of gas laws, specifically the ideal gas law (PV = nRT), to determine the unknown partial pressure of helium. The total pressure and conditions of the gas mixture are given to assist in the completion of this task.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A balloon has 0.158 mol of gas and has a volume of 2.46 L. If an additioal 0.113 mol of gas is added to the balloon (at the same temperature and pressure), what is its final volume?
A mixture of nitrogen and carbon dioxide gases, in a 6.15 L flask at 59 °C, contains 2.64 grams of nitrogen and 11.7 grams of carbon dioxide. The partial pressure of carbon dioxide in the flask is atm and the total pressure in the flask is atm.
An engine cylinder contains 250 mL of gas at a pressure of 1.0 atm. As the engine runs, it compresses the cylinder, reducing the volume of the gas to 25 mL. What is the new pressure of the gas at this volume?
A mixture of oxygen and hydrogen gases is maintained in a 7.48 L flask at a pressure of 1.05 atm and a temperature of 60 °C. If the gas mixture contains 4.63 grams of oxygen, the number of grams of hydrogen in the mixture is
A mixture of argon and krypton gases, in a 9.30 L flask at 46 °C, contains 6.46 grams of argon and 45.4 grams of krypton. The partial pressure of krypton in the flask is atm and the total pressure in the flask is atm.
A container holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of the three gases are 2.00 atm, 3.00 atm, and 4.00 atm, respectively. What is the total pressure inside the container?
A mixture of neon and hydrogen gases at a total pressure of 973 mm Hg contains neon at a partial pressure of 331 mm Hg. If the gas mixture contains 2.39 grams of neon, how many grams of hydrogen are present?
Two students perfomed an experiment on the decomposition of hydrogen peroxide. One student was in Wisconsin where the atmospheric pressure was 0.996 atm. The other was in Colorado, where the atmospheric pressure was 0.832 atm. Both reactions were performed at the same temperature and produced the same number of moles of oxygen gas. How do the volumes of gases collected compare? Are they the same or not? Explain.
A mixture of hydrogen and xenon gases, in a 6.78 L flask at 18 °C, contains 0.426 grams of hydrogen and 21.5 grams of xenon. The partial pressure of xenon in the flask is__ atm and the total pressure in the flask is__ atm.
The atmospehere in a sealed diving bel contained oxygen and helium. If the gas mixture has 0.200 atm of oxygen and a total pressure of 3.00 atm, calcuate the mass of helium in 1.00 L of the gas mixture at 25.0 C.
A mixture of nitrogen and xenon gases, in a 5.99 L flask at 50 °C, contains 2.90 grams of nitrogen and 43.1 grams of xenon. The partial pressure of xenon in the flask is atm and the total pressure in the flask is atm.
Container A holds 752 mL of ideal gas at 2.30 atm. Container B holds 124mL of ideal gas at 4.70 atm. If the gases are allowed to mix together, what is the partial pressure of each gas in the total volume?