**Problem Statement:**An unknown gas at 49.1 °C and 1.05 atm has a molar mass of 30.07 g/mol. Assuming ideal behavior, what is the density of the gas?**Density Calculation:**Density: [ _______ ] g/L**Explanation:**To find the density of the gas, use the ideal gas law and the relationship between molar mass, pressure, temperature, and volume. The ideal gas equation is:\[ PV = nRT \]Where:- \( P \) = pressure in atm- \( V \) = volume in liters- \( n \) = number of moles- \( R \) = ideal gas constant (0.0821 L·atm/mol·K)- \( T \) = temperature in Kelvin**Steps to calculate density:**1. Convert the temperature from Celsius to Kelvin: \[ T(K) = 49.1 + 273.15 \]2. Use the density formula derived from the ideal gas law: \[ \text{Density} = \frac{PM}{RT} \] Where \( M \) is the molar mass in g/mol.3. Substitute the known values into the formula to calculate the density in g/L.

The formula required to determine the density of gas with ideal behavior is as follows,Calculation is as follows,

Answered: An unknown gas at 49.1 C and 1.05 atm…

An unknown gas at 49.1 C and 1.05 atm has a molar mass of 30.07 g/mol. Assuming ideal behavior, what is the density of the gas?

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: If 45.5 g of O2 and 2.1 g of CO2 are placed in a 11.1 L container at 34 oC , what is the pressure…

Q: A 1.35 g sample of an unknown gas at 43 ∘C and 1.10 atm is stored in a 1.45 L flask. What is the…

A: The density is calculated by using given mass and volume.

Q: The molar volume of a sample of a gas at 353 Kand 100. atm is 0.204 L mol. At these conditions,…

A: Given that : The molar volume of the gas (Vmolar) = 0.204 L/mol The temperature of the gas (T) = 353…

Q: A newly discovered gas has a density of 2.16 g/L at 26.0 °C and 731 mm Hg. What is the molar mass of…

A: Given: The density of new element,(d)=2.16 g/L The temperature, (T)=26.0 °C=(273.15+26)=299.15 K The…

Q: A sample of 2.85 mol of gas in a 8.00 L container is at 45.0 °C. What is the pressure (in bar) of…

Q: molar mass

Q: A 2.55 g sample of an unknown gas at 31 ∘C and 1.05 atm is stored in a 2.85 L flask. What is the…

A: First the density is determined by using density formula as shown below,

Q: The percent composition of air by volume is 78.08% N2, 20.95% O2, 0.93% Ar, and 0.036% CO2. What are…

A: According to Dalton's law, the partial pressure of a particular gas in a mixture can be used to…

Q: An unknown gas at 25.1 ∘C25.1 ∘C and 1.10 atm1.10 atm has a molar mass of 44.10 g/mol.44.10 g/mol.…

Q: A mixture of methane and neon gases, in a 5.79 L flask at 55 °C, contains 4.14 grams of methane and…

A: Given Volume ( V ) = 5.79 Liter Temperature ( T ) = 55 ℃ = ( 55 +…

Q: vessel contained N2, Ar, He, and Ne. The total pressure in the vessel was 987 torr. The partial…

A: According to the Dalton’s law For a non-reacting gaseous mixture sum of partial pressure of…

Q: You have produced 170 g of NHin a 5.0L tank at 400.0 C. What is the total pressure of the gasses?

A: The relationship between temperature, pressure, volume and number of mole is given by ideal gas…

Q: A mixture of gases containing 0.362 moles of oxygen, 1.23 moles of nitrogen, and 0.0234 moles of…

A: Given: moles of O2 = 0.362 mol moles of N2 = 1.23 mol moles of Ar = 0.0234 mol Total pressure = 2.60…

Q: A mixture of argon and helium gases contains argon at a partial pressure of 464 mm Hg and helium at…

A: Dalton’s Law of Partial Pressures states that the total pressure exerted by the mixture of…

Q: A sample of O3 gas is observed to effuse through a pourous barrier in 7.68 minutes. Under the same…

A: Graham’s law states that rate of effusion is inversely proportional to the square root of molar mass…

Q: A mixture of xenon and oxygen gases contains xenon at a partial pressure of 195 mm Hg and oxygen at…

A: Given: Partial Pressure of Xenon =195mm Hg The partial pressure of Oxygen= 656 mm Hg To calculate:…

Q: Under identical conditions, separate samples of O2 and an unknown gas were allowed to effuse through…

Q: A mixture of gas contain 4.00 g of element A and 4.00 g of element B. Element A has a molar mass of…

A: To solve this problem we have to calculate the mole fraction of A and B .

Q: What is the volume occupied by a mixture of 0.386 mol of N2 and 0.386 mol of O2 gases at 1.04 atm…

A: The total number of moles of the gas in a mixture is expressed as the sum of the moles of the…

Q: A 10.00 gram gas mixture contains Nz and CO2. If 2.00 grams of the mixture is Nz and the total…

A: Given :- Amount of mixture of N2 and CO2 = 10.00 g Mass of N2 in mixture = 2.00 g Total pressure…

Q: What is the partial pressure of neon that's 18% by volume in a gas mixture with a total pressure of…

A: Answer: According to Dalton's law of partial pressure, partial pressure of any gas in the gaseous…

Q: 0.0380g of Mg Strip reacted completely with 6 M HCl in the gas buret and 35.8 mL of hydrogen gas is…

A: Number of Mole-ratio of given mass of substance to the molar mass of substance is called number of…

Q: 3.55 g sample of an unknown gas at 33 degrees Celcius and 1.10 atm is stored in a 2.55 L flask. What…

A: The density of the gas present in the flask can be calculated by diving its mass by volume.

Q: . g of CO2 gas (molecular weight 44 g/mole) occupies 10.0 L at 350 K, what is the pressure of this…

A: Ideal gas is also called a perfect gas. Ideal gas is a gas in which pressure P, volume V and…

Q: What is the pressure of a 50.0 L tank that contains 4.04 kg of oxygen, O2, at 24 degrees C? Assume…

A: According to ideal gas equation,

Q: A sample of xenon gas occupies a volume of 6.95 L at 493K. If the pressure remains constant , at…

A: The xenon gas sample is given at - Volume, V1 = 6.95 L Temperature, T1 = 493 K Volume, V2 = 3.77 L…

Q: Styrene oxide is a fairly simple aromatic organic compound that has a pleasant odor and is often…

A: Mole of a substance or a mole of a particles is defined as exactly 6×10^23 particles which may be…

Q: 5. After blowing up a balloon, a student was curious what the partial pressure of each gas was in…

A: Daltons Law of partial pressure says that total pressure is the sum of the individual pressures of…

Q: 2.2 L of He gas at 7.6 atm pressure and 25oC and 3.8L of Ne gas at 4.2 atm pressure and 25oC are…

A: Given, Volume of He gas = 2.2 L Pressure = 7.6 atm Temperature = 25◦c Volume of Ne gas = 3.8 L…

Q: A gas mixture has partial pressures of 90. mm Hg O2, 150 mmHg Ar, and 325 mmHg CO2. What is the mole…

Q: The density of a gas is 1.74 g/L at 31oC and 592 torr. Calculate the molar mass of this gas. R =…

Q: A compound which is 39.9 % C, 13.5 % H, and 46.6 % N by mass was studied. A 0.378 g sample of the…

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

**Problem Statement:**

An unknown gas at 49.1 °C and 1.05 atm has a molar mass of 30.07 g/mol. Assuming ideal behavior, what is the density of the gas?

**Density Calculation:**

Density: [ _______ ] g/L

**Explanation:**

To find the density of the gas, use the ideal gas law and the relationship between molar mass, pressure, temperature, and volume. The ideal gas equation is:

\[ PV = nRT \]

Where:
- \( P \) = pressure in atm
- \( V \) = volume in liters
- \( n \) = number of moles
- \( R \) = ideal gas constant (0.0821 L·atm/mol·K)
- \( T \) = temperature in Kelvin

**Steps to calculate density:**
1. Convert the temperature from Celsius to Kelvin:
\[ T(K) = 49.1 + 273.15 \]

2. Use the density formula derived from the ideal gas law:
\[ \text{Density} = \frac{PM}{RT} \]

Where \( M \) is the molar mass in g/mol.

3. Substitute the known values into the formula to calculate the density in g/L.

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 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 gas sample with a mass of 11.2 g exerts a pressure of 1.05 atm at 22.0ºC and a volume of 2.79 L. What is the molar mass of the gas? *
A 30.0 L vessel contains a mixture of carbon dioxide, sulfur trioxide, oxygen, and neon gases at 25.0°C and 2.75 atm. The mole fraction of each gas is 0.25. What mass of each gas is present?
A chamber contains a mixture of gases: 0.25 mol O2, 0.85 mol N2, 0.032 mol CO2 and 0.25 mol CO. The total pressure in the chamber is 9.55 atm. Calculate the partial pressures for each gas.
2.0 g of H2 gas and 4.0 g of He gas are contained in a 50.0-L gas-tight vessel 25.0o C. Calculate the partial pressure of each gas.
150. g of an unknown monatomic gas phase element has just been released into a container of volume 90.95 L at a pressure of 1.0114 atm. If the temperature of the room is 25.4°C, what are the molar mass and the identity of the gas? molar mass identity of the gas
A 1.25 g sample of an unknown gas at 47 ∘C and 1.00 atm is stored in a 2.55 L flask. What is the density of the gas? density: g/L What is the molar mass of the gas? molar mass: g/mol
A 18.0 mg sample of an unknown gas is placed in a 750.0 mL flask at 85 0C and 1.20 atm. What is the molar mass (gm/mole) of this substance? (b) What the average speed (units) of helium at 25.00C?
A gas has a density of 1.53 g L-1 at 53 °C and P = 0.938 atm. What will be its density at 161 °C? Calculate the molar mass of the gas, assuming it obeys the ideal gas law.Density at 161 °C = g L-1Molar mass = g mol-1
12. Suppose 435 mL of Ne gas at 21 °C and 1.09 atm, and 456 mL of SF6 at 25 °C and 0.89 atm are put into a 325 mL flask at 30.2 °C. (a) What will be the total pressure in the flask? (b) What is the mole fraction of for each of the gases in the flask? (c) How many grams of each gas are in the flask?
An unknown gas at 79.1 ∘C and 1.10 atm has a molar mass of 16.04 g/mol. Assuming ideal behavior, what is the density of the gas? density: g/L