Given a gas sample with a Temperature of 298 K, a Pressure of 1.2 atm, and a molar quantity of 0.12 moles. Solve for Volume (in L) PV = nRT P in atm, V in Liters, n in moles, T in Kelvin R = 0.08206 (L*atm)/(mol*K)

Given a gas sample with a Temperature of 298 K, a Pressure of 1.2 atm, and a molar quantity of 0.12 moles. Solve for Volume (in L) PV = nRT P in atm, V in Liters, n in moles, T in Kelvin R = 0.08206 (Latm)/(molK)

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: 2. The form of the Ideal Gas Law that we used in class is pVmRT, where p is absolute pressure, V is…

A: We have pV= mRT, where p is absolute pressure, V is volume, R is the specific gas constant and T is…

Q: (a) Are you more likely to see the density of a gas reported ing/mL, g/L, or kg/cm3? (b) Which units…

A: a) The units which are more likely for density are g/ml and Kg/lit. b) Since the unit of Pressure =…

Q: The ideal gas equation is PV=nRTPV=nRT where PP is pressure, VV is volume, nn is the number of…

A: The ideal gas equation is PV=nRT Where, P is pressure, V is volume, n is the number of moles, R is…

Q: A certain gas is present in a 10.0 L cylinder at 2.0 bar pressure. If the pressure is increased to…

A: Explanation Gas law The gas law are a set of laws that describe the relation between thermodynamic…

Q: Solid ammonium chloride, NH4Cl, is formed by the reaction of gaseous ammonia, NH3, and hydrogen…

A: Given,Mass of NH3 = 5.28 gMass of HCl = 5.28 gMoles of NH3 and HCl can be calculated as:

Q: The ideal gas law (PV=nRT) describes the relationship among pressure P. volume V, temperature T, and…

A: Temperature and pressure are linearly related, and if the temperature is on the kelvin scale, then P…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

A: Please find your solution below : In van der waals equation, the parameters a and b are the…

Q: What is the volume of H2 in (L) that forms at 409 K and a constant 1.7 atm if 2.04 grams of K reacts…

A: the given balanced reaction 2K+2H2O →2KOH+H2

Q: + |/ 00 %24 D. Two bulbs are connected by a stopcock. The 7.50 L bulb contains nitric oxide (NO) at…

A: After the stopcock is opened, the following reaction occurs:

Q: A 1.00 L sample of cooking gas taken from a cylinder was collected. Its mass, measured at 27.0° C…

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

A: Since you have posted questions with multiple subparts, we are entitled to answer the first 3 only.…

Q: At what temperature does sulfur tetrafluoride have a density of 0.225 g/L at 0.0721 atm? Tap here or…

Q: 2 S The ideal gas law describes the relationship among the pressure P, volume V, number of moles n.,…

Q: Pressure of gas = 101.3 KPa = 0.9998 atm Temperature = 293 K Calculating number of moles of Cl2…

Q: The pressure, P, the temperature, T, and the volume V of an ideal gas are related by PV= nRT, wheren…

A: Given: temperature increased by ΔT = 0.04 And nR = 1

Q: p+a |(V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles…

A: Given :

Q: A balloon contains 10 g of H₂ (2.01588 amu) gas. How many moles of argon gas (39.9480 amu) must be…

A: Since the surface of the balloon is flexible, the pressure inside the balloon will be the same as…

Q: Determine the mole fraction and partial pressure for each gas in the mixtures below. a) 1.62 g CO2…

Q: 6. Krypton, first discovered in samples of liquefied air, takes its name from the Greek word for…

A: Since you have posted a question with multiple questions, we will solve first question for you. To…

Q: The average kinetic energy of the molecules in a gas sample depends only on the temperature, T.…

A: The root mean square velocity (rms) of a gas is given by the formula rms speed = 3RTM R = gas…

Q: The pressure of a gas is 380 mm Hg. Express this pressure in units of a. atmospheres. Pressure = b.…

A: Given:The pressure of a gas is 380 mmHg.We have to convert the pressure at different units.

Q: When a car airbag is deployed, it expands because of nitrogen gas generated by the rapid…

A: Answer:-This question is answered by using the simple concept of stoichiometry which involves the…

Q: dX = (3nR) dT +( an- -)dv where R (= 0.08206 atm-L/mol-K or 8.314 J/mol-K) is the gas constant; van…

Q: partial pressure of each constituent knowing their respective amounts: nA = 2.25 mol ; na = 0.60 mol…

A: 3. Given : Total Pressure = 1.20atm T = 300 K…

Q: A tank contains 2 m³ of a gas which is 70% methane, 25% ethane, and 5% nitrogen by volume. The…

Q: 10.0L tank at 1.21°C is filled with 9.54g of dinitrogen difluoride gas and 13.5g of chlorine…

Q: If I have a gas with a volume of 35.0 liters at 100. C and 3.00 atm, what is the volume of the gas…

A: At Initial Conditions : Volume, V1 = 35 L Temperature, T1 = 100 °C = (100 + 273.15) K…

Q: Payalben

A: Step 1:Vander waals parameter 'a' depends on the attraction forces between gaseous molecules. As we…

Q: An 11-L flask contains 20 g of Ne (20.17970 amu) and an unknown weight of H₂ (2.01588 amu). The gas…

Q: A gas that obeys the equation of state: P = RT V-b a T²V² For this gas, determine the Boyle…

A: We are given the equation of state. We need to find Boyle temperature expression and a/b ratio.

Q: To apply the ideal gas law to problems involving temperature, pressure, volume, and moles of a gas

A: Ideal gas equation is PV=nRT where P= pressure of the gas in atm V = volume of the gas…

Q: Please show complete solution and given 1. For each of the following pairs of variables, which…

A: In first question we used the ideal gas equation- PV = nRT in the second question used the Boyle…

Q: p+a- |(V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles…

A: For the consistency of units, the units of an2V2 must be same as the units of P

Q: Given that the molar volume of an ideal gas is 22,4186 liters/gmol at 273,15 K and 1.000 atm,…

A: Using ideal gas equation: PV = nRT Where, P is pressure of gas V is volume of gas n is number of…

Q: 4. Consider a sample of gas at 393 K and 22 atm. (a) Calculate the molar volume V (L/mol) of the…

Q: 10 mol of NH3 (g) were placed in a previously evacuated 20-L container. After a sudden temperature…

A: Given information: No. of moles of NH3 = 10 mol volume of container =20 L

Q: The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to…

Q: The ideal gas law describes the relationship among the volume of an ideal gas (V), its pressure (P),…

A: Answer:Ideal gas law : Van Der waal equation :

Q: Starting with Charles's law (stated as an equation), obtain an equation for the final volume of a…

A: Complete the given relation by using gaseous law ---

Q: oles If I have 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 56 °C, what is the…

Q: Sodium bicarbonate is reacted with concentrated hydrochloric acid at 37.0°C and 1.00 atm How much…

A: We use here balanced equation which tells about the moles of product corresponding to moles of…

Q: Using Kay's method, what is the number of moles of this mixture in the tank?

A: As per Kay's method ; the no. of moles of a mixture in tank is 2.27 Kmoles ( option A is correct )

Q: Determine the pressure of 2.581 moles of an ideal gas to THE WHOLE NUMBER in atm that has a volume…

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

Given a gas sample with a Temperature
of 298 K, a Pressure of 1.2 atm, and a
molar quantity of 0.12 moles.
Solve for Volume (in L)
PV = nRT
P in atm, V in Liters, n in moles, T in
Kelvin
R = 0.08206 (L*atm)/(mol*K)

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 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

At what temperature does sulfur tetrafluoride have a density of 0.290 g/L at 0.0721 atm? Tap here or pull up for additional resources Question 6 of 33 C > 4-A b 1 4 7 +/- 2 5 8 27.5 K 3 6 9 O ||| 0 Submit C x 100 <
Give Detailed Solution (don't give Handwritten answer)
A mixture of Oxygen and Chlorine gases contain twice as much Oxygen (by mass - in grams) as Chlorine (2xO2g= Cl2g) If the total pressure of the mixture is 565mmHg, then what is the partial pressure of chlorine ? Using (from Ideal Gas law - Dalton) Partial Pressure Partial Pressure (?) Moles of Chlorine (?) / (divided) by Total Moles O2+Cl2 or written nA / nT (Total Pressure) I've tried to determine what multiple of Oxygen, in grams - by atomic mass, will give me 1/2 the weight of Chlorine - in order to determine Mole (mol) Count for each DIATOMIC. I'm not frustrated, but i'm a little tired of going through this, for 2 hours, I have looked at - similar formula - variations, but this is the challenge. thanks
Determination of the Universal Gas Constant Postlab 1. An evaluation of Rwas performed using the procedures outlined in this exercise, The barometric pressure was 735 torr and the temperature was 21.5 "C. The volume of H2(9) collected was 32.7 mL. The calculated value of Rwas 0.0817 L'atm/mol-K. a. How many grams of Mg metal were used in this determination? 0.0316 70.361 b. If the correction for the vapor pressure of water had not been performed, what would be the calculated value of R? Incorrect c. If the syringe volume had been incorrectly read, resulting in a calculated H, volume of 30.6 mL, what would be the percent error in the calculated value of Rwith respect to the originally calculated value (0.0817 L-atm/mol·K)? 6.4 %
6-25. A mixture of gases contains 66.0 g CO2, 2.02 g of H₂, and 16.0 g of O₂. If the total pressure of the mixture is 725 torr, what is the partial pressure of each gas? 6-26. Air, by weight, is essentially a mixture of 79% N₂ and 21% O₂. Calculate the partial pressure of each gas at a total pressure of 99 kPakPa.
What is the pressure (in bar) in a 4.00 L tank with 24.0 grams of oxygen gas at 350.0 K? R = 0.08314 L･bar/mol･K.
100% EXP 3- Determination of universal gas constant Thermal decomposition reaction of KCIO3 can be used to determine the universal gas constant. 2KCIO:(s) 2KCI(s) + 302(g) MnO2 (catalyst) Firstly, KCIO3 and MnO2 (catalyst) is placed in a clean and dry test tube, and it is weighed as 15.92 g. While heating the test tube, thermal decomposition reaction occurs and all the evolved O2(g) is collected in a flask filled with water at 759 mmHg and 20°C. Because of evolved O2(g), 250 mL water is transferred from the flask to a beaker. Additionally, the weight of test tube after heating is determined as 15.60 g. (Note: The partial pressure of water at 20°C is 17.5 mmHg.) (a) Calculate experimental value of the universal gas constant by using the information given above. (b) Compare the theoretical and the experimental values of gas constant and calculate the percentage error in the experiment. (KČIO:: 122.55 g/mol. Oz: 32.00 g/mol, R: 0.082 L atm/mol K) EXP 4- Diffusion
Sketch three isochores for the same gas at three different volumes V1, V2 and V3 where V1 = V3 and V2<V3. How the temperature scale (K vs oC) will change on your plot?
5. There are 1.07 X 103 moles of gas molecules contained in a CO2 cartridge under 5.0-atm of internal pressure. After several uses, the internal pressure is 3.4-atm. How many moles of gas remain in the cartridge? How much gas will remain in the cartridge when the internal pressure equilibrates to standard pressure? (Assume that the temperature and volume remain constant.)
If you have two jars containing the same amount, n1=n2, and type of gas (for example, oxygen) and they are at the same temperature, T, what can you say about their pressure if the first jar has four times the volume of the second, V1 = 4V2? Hint: use pV=nRT Group of answer choices P1 = (1/4)P2 P1 = (1/3)P2 P1 = P2 P1 = 4P2 P1 = 3P2 I believe it is P1 = 4P2 but unsure...
Ammonia, NH3, can react with oxygen to form nitrogen gas and water. 4 NH3(aq) + 30₂(g) →→→ 2N₂(g) + 6H₂O(1) If 3.85 g NH3 reacts with 5.78 g O₂ and produces 0.950 L N₂, at 295 K and 1.01 bar, which reactant is limiting? NH,(aq) 0₂(g) Calculate the percent yield of the reaction. percent yield:
The ideal gas law describes the relationship among the pressure P, volume V, number of moles n, and absolute temperature T of an ideal gas. Here is the relationship expressed mathematically: PV = nRT where R is a proportionality constant. The units of R are determined by the units of pressure and volume used in the equation. When bar used for pressure and L for volume, the appropriate R value is 0.08314 L bar mol-¹ K-¹. Part A How many air molecules are in a 4.05 x 3.66 x 3.05 m³ room? Assume atmospheric pressure of 1.00 bar, a room temperature of 20.0 °C, and ideal behavior. Express your answer using three significant figures. ► View Available Hint(s) VE ΑΣΦ + Review | Constants | molecules