At higher densities, gases will exert a pressure greater than that predicted by the ideal gas...
At higher densities, gases will exert a pressure greater than that predicted by the ideal gas law. Which statement below is the best explanation?
a) The ideal gas law is an estimate. More molecules makes the inaccuracies more obvious.
b) High density requires a higher kinetic energy, thereby increasing the pressure.
c) The volume available for molecules to move in is reduced by the volume occupied by the molecules themselves, leading to more frequent collisions and thus higher pressure.
d) Distances between molecules becomes small enough that intermolecular forces are significant.
e) High density requires high temperature, thus increasing the frequency of collisions.
Homework Answers
The volume available for molecules to move in is reduced by the volume occupied by the molecules themselves, leading to more frequent collisions and thus higher pressure.
(C) is correct option
Add Answer to:
At higher densities, gases will exert a pressure greater than
that predicted by the ideal gas...
At very high pressures (M 1000 atm), the measured pressure exerted by real gases is greater...
At very high pressures (M 1000 atm), the measured pressure exerted by real gases is greater than that predicted by the ideal gas equation. This is mainly because Multiple Choice such high pressures cannot be accurately measured. ces real gases will condense to form liquids at 1000 atm pressure. gas phase colisions prevent molecules from colliding with the walls of the container. of attractive intermolecular forces between gas molecules KPrev 6 of 10 Next> Multiple ChOice SUch high pressures cannot...
Part A) Which of the following statements is true for ideal gases, but is not always...
Part A) Which of the following statements is true for ideal gases, but is not always true for real gases? Choose all that apply. Molecules are in constant random motion. Pressure is caused by molecule-wall collisions. The size of the molecules is unimportant compared to the distances between them. The volume occupied by the molecules is negligible compared to the volume of the container. Part B) Which of the following statements is true for real gases? Choose all that apply....
Equal masses of CO2 and CH4 gas are placed in identical 1.00 L containers, both at the same temperature. Which of the following is true? X. Both gases exert the same pressure. Y. Molecules of...
Equal masses of CO2 and CH4 gas are placed in identical 1.00 L containers, both at the same temperature. Which of the following is true? X. Both gases exert the same pressure. Y. Molecules of CH4 make more frequent collisions with the walls of the container. Z. Both gases have the same average molecular speed. answer can be more than one
1. Which of the following statements is true for ideal gases, but is not always true...
1. Which of the following statements is true for ideal gases, but is not always true for real gases? Choose all that apply. A. Replacing one gas by another under the same conditions, has no effect on pressure. B. Collisions between molecules are elastic. C. There are no attractive forces between molecules. D. Molecules are in constant random motion. 2. Which of the following statements is true for real gases? Choose all that apply. A. As molecules increase in size,...
Which of the following statements is true for real gases? Choose all that apply. As molecules...
Which of the following statements is true for real gases? Choose all that apply. As molecules increase in size, deviations from ideal behavior become more apparent at relatively low pressures. The volume occupied by the molecules can cause a decrease in pressure compared to the ideal gas. As molecules increase in size, deviations from ideal behavior become more apparent at relatively high pressures. The volume occupied by the molecules can cause an increase in pressure compared to the ideal gas.
1a)Which of the following statements is true concerning ideal gases? Select one:a The gas particles in...
1a)Which of the following statements is true concerning ideal gases? Select one:a The gas particles in a sample exert attraction on one another b All of these statements are false cThe temperature of the gas sample is directly related to the average velocity of the gas particles dA gas exerts pressure as a result of the collisions of the gas molecules with the walls of the container e At STP, 1.0 L of gaseous Ar contains about twice the number...
In lab, we noted that pressure (which should be the same for both gases) is a...
In lab, we noted that pressure (which should be the same for both gases) is a product of the strength of the collision times the frequency of collisions. The strength is proportional to mv, and the frequency is proportional to v. If we take the mass of hydrogen to be 4 kg and the speed to be 3 m/s (yes - these numbers are ridiculous for a molecule of gas - but the goal here is to focus on concepts...
This problem will review one of the questions in the ideal gas, but with numbers: You...
This problem will review one of the questions in the ideal gas, but with numbers: You have one container of hydrogen, and another container of oxygen. The number of molecules, temperature and volume are the same for both gases. Oxygen is, however, heavier than hydrogen. How does the average kinetic energy of hydrogen compare to oxygen? Hydrogen has LARGER average kinetic energy than oxygen. Hydrogen has THE SAME average kinetic energy as oxygen. Hydrogen has LESS average kinetic energy than...
L. Under that conditions of temperature and pressure would you expect gases to obey the ideal-gas...
L. Under that conditions of temperature and pressure would you expect gases to obey the ideal-gas equation? 2 Calculate the value of R in L-atm/mol-K by assuming that an ideal gas occupies 3 Why do you equalize the water levels in the bottle and the beaker? 5 What is the value of an error analysis? 224 Lmol at STP 4 Why does the vapor pressure of water contribute to the total pressure in the bottle? Suggest reasons why real gases...
Which of the following statements is true tor real gases? Choose all that apply. As molecules...
Which of the following statements is true tor real gases? Choose all that apply. As molecules increase in size, deviations from ideal behavior become more apparent at relatively high pressures. Attractive forces between molecules cause a decrease in pressure compared to the ideal gas. The volume occupied by the molecules can cause a decrease in pressure compared to the ideal gas. As molecules increase in size. deviations from ideal behavior become more apparent at relatively low pressures.
At very high pressures (M 1000 atm), the measured pressure exerted by real gases is greater than that predicted by the ideal gas equation. This is mainly because Multiple Choice such high pressures cannot be accurately measured. ces real gases will condense to form liquids at 1000 atm pressure. gas phase colisions prevent molecules from colliding with the walls of the container. of attractive intermolecular forces between gas molecules KPrev 6 of 10 Next> Multiple ChOice SUch high pressures cannot...
Which of the following statements is true for real gases? Choose all that apply. As molecules increase in size, deviations from ideal behavior become more apparent at relatively low pressures. The volume occupied by the molecules can cause a decrease in pressure compared to the ideal gas. As molecules increase in size, deviations from ideal behavior become more apparent at relatively high pressures. The volume occupied by the molecules can cause an increase in pressure compared to the ideal gas.
L. Under that conditions of temperature and pressure would you expect gases to obey the ideal-gas equation? 2 Calculate the value of R in L-atm/mol-K by assuming that an ideal gas occupies 3 Why do you equalize the water levels in the bottle and the beaker? 5 What is the value of an error analysis? 224 Lmol at STP 4 Why does the vapor pressure of water contribute to the total pressure in the bottle? Suggest reasons why real gases...
Which of the following statements is true tor real gases? Choose all that apply. As molecules increase in size, deviations from ideal behavior become more apparent at relatively high pressures. Attractive forces between molecules cause a decrease in pressure compared to the ideal gas. The volume occupied by the molecules can cause a decrease in pressure compared to the ideal gas. As molecules increase in size. deviations from ideal behavior become more apparent at relatively low pressures.
Most questions answered within 3 hours.
-
Where is the error in this code sequence?
String s1 = "Hello";
String s2 = "ello";...
asked 10 months ago -
Financial data for Joel de Paris, Inc., for last year
follow:
Joel de Paris, Inc.
Balance...
asked 10 months ago -
Consider this reaction:
Al2(SO4)3 (aq)+ BaCl3
(aq) Al2Cl6 (aq)- +
3BaSO4(s) . What is the...
asked 10 months ago -
Suppose that Savneet is considering increasing her
recent random sample from 20 car rentals to 40...
asked 10 months ago -
Trucks arrive at an unloading terminal at an average rate of 120
per hour.
Trucks arrive...
asked 10 months ago -
Why are methanol and ethanol completely soluble in water while
octanol is not very little soluble....
asked 10 months ago -
A facilities manager at a university reads in a research report
that the mean amount of...
asked 10 months ago -
When the CuSO4 is rehydrated by adding water to the anhydrous
compound, is this an endothermic...
asked 10 months ago -
A ray of sunlight is passing from diamond into crown glass; the
angle of incidence is...
asked 10 months ago -
A block of mass 0.249 kg is placed on top of a light, vertical
spring of...
asked 10 months ago -
how do the kidneys compensate in the presences of acidosis
a) trigger hyperventilate
b) reserve acid...
asked 10 months ago -
Question 501 pts
The rental rate of capital to the firm increases. Which of the
following...
asked 10 months ago