1. Solving ideal Gas Law Problems Directions: Use the ideal gas law, "PV-nRT", and the universal gas constant R-0.0821 L'atm to solve the following problems: K*mol if pressure is needed in kPa then convert bymultiplying by 101.3KPA / latm to get R =8.31 kPa"L/ (K*mole). Show your answers legibly, concisely, andcompletely. Use separate sheet of paper.If i have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is thetemperature?If I have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and atemperature of 870 C, how many moles of gas do I have?Ifi have 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 560 C, what is the1.1.1.2.1.3.volume of the container that the gas is in?If i contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K,what is the pressure inside the container?1.4.

As per our guideline we will solve first three parts for you. To get remaining parts solved please…

1. Solving ideal Gas Law Problems Directions: Use the ideal gas law, "PV-nRT", and the universal gas constant R -0.0821 L'atm to solve the following problems: K*mol if pressure is needed in kPa then convert by multiplying by 101.3KPA / latm to get R =8.31 kPa"L/ (K*mole). Show your answers legibly, concisely, and completely. Use separate sheet of paper. 11. Hi have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature? 1.2. Ifi have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 870 C, how many moles of gas do I have? Ifi have 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 560 C, what is the volume of the container that the gas is in? If i contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, what is the pressure inside the container? 1.3. 1.4.

1. Solving ideal Gas Law Problems Directions: Use the ideal gas law, "PV-nRT", and the universal gas constant R -0.0821 L'atm to solve the following problems: Kmol if pressure is needed in kPa then convert by multiplying by 101.3KPA / latm to get R =8.31 kPa"L/ (Kmole). Show your answers legibly, concisely, and completely. Use separate sheet of paper. 11. Hi have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature? 1.2. Ifi have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 870 C, how many moles of gas do I have? Ifi have 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 560 C, what is the volume of the container that the gas is in? If i contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, what is the pressure inside the container? 1.3. 1.4.

Physics for Scientists and Engineers

10th Edition

ISBN:9781337553278

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter20: The Kinetic Theory Of Gases

Section: Chapter Questions

Problem 26P: The law of atmospheres states that the number density of molecules in the atmosphere depends on...

See similar textbooks

Similar questions

Under what circumstances would you expect a gas to behave significantly differently than predicted by the ideal gas law?
The dwarf planet Pluto has an average surface temperature of 44 K and an escape speed (divided by six) of 0.2 km/s. Based on Figure 5.5, which gases, if any, would this body be likely to have retained as an atmospheric constituent over the past 3 billion years?
(a) If tossing 100 coins, how many ways (microstates) are there to get me three most likely macro states of 49 heads and 51 tails, 50 heads and 50 tails, and 51 heads and 49 tails? (b) What percent of the total possibilities is this? (Consult Table 15.4.)
One container is filled with helium gas and another with argon gas. Both containers are at the same temperature. Which molecules have the higher rim speed? Explain.
The law of atmospheres states that the number density of molecules in the atmosphere depends on height y above sea level according to nV(y)=n0en0gy/kaT where n0 is the number density at sea level (where y = 0). The average height of a molecule in the Earths atmosphere is given by yavg=0ynV(y)dy0nV(y)dy=0yen0gy/kaTdy0en0gy/kaTdy (a) Prove that this average height is equal to kBT/m0g. (b) Evaluate the average height, assuming the temperature is 10.0C and the molecular mass is 28.9 u, both uniform throughout the atmosphere.
(a) Construct a table showing the macro states and all of the individual microstates for tossing 13 coins. (Use Table 15.5 as a guide.) (b) How many macro states are there? (c) What is the total number of microstates? (d) What percent chance is here of tossing 5 heads and 1 tail? (e) How much more likely are you to toss 3 heads and 3 tails than 5 heads and 1 tail? (Take me ratio of the number of microstates to find out.)
(a) Hydrogen molecules (molar mass is equal to 2.016 g/mol) have vrms equal to 193 m/s. What is the temperature? (b) Much of the gas near the Sun is atomic hydrogen (H rather than H2). Its temperature would have to be 1.5107 K for the speed vrms to equal the escape velocity from the Sun. What is that velocity?
(a) What is me 1imlume (in km3) of Avogadro’s number of sand grains if each grain is a cube and has sides mat are 1.0 mm long? (b) How many kilometers of beaches in length would this cover it me beach averages 100 m in width and 10.0 m in depth? Neglect air spaces between grains.
2. Explain how ideal gas equation summarizes all the gas laws.
1. A three-liter tank contains two gram-moles of nitrogen at − 150.8o C. Estimate the tank pressure using the ideal gas equation of state and then using the Virialequation of state truncated after the second term. Taking the second estimate to be correct, calculate the percentage error that results from the use of the ideal gas equation at the system conditions. Data for nitrogen: Tc = 126.2 K, pc = 33.5 atm, and ω = 0.04012. 2. One mole of propane gas is to be expanded from 0.001 m3 to 0.040 m3 while incontact with a heating bath at 100o C. The expansion is not reversible. The heatextract from the bath is 600 J. Determine the work for the expansion using theVan der Waals equation of state.
2. If 150.00 mL of N2 gas was collected at 760 torr, what is the new volume of the gas when the pressure is compressed to 740 torr at the same temperature? 1. The gas inside the tire has a volume of 20.00 L at a pressure of 5.00 atm. Calculate the pressure of the gas if its volume is reduced to 10.0 at the same temperature.
1. Why is it that the Metal Rod no longer expands when it reaches a constant temperature? 2. Why is it necessary to know the coefficient of linear expansion of solids? 3. Give examples of solids that expand or contract due to temperature changes?