Which of the following statements is true tor 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.
Which of the following statements is true for real gases? Choose all that apply Attractive forces between molecules cause a decrease in pressure compared to the ideal gas. Attractive forces between molecules cause an increase in pressure compared to the ideal gas. As molecules increase in size, deviations from ideal behavior become more apparent at relatively low pressures. As attractive forces between molecules increase, deviations from ideal behavior become more apparent at relatively low temperatures. Compute the root-mean-square speed of...
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....
- A 1.31 mol sample of Kr gas is confined in a 32.4 liter container at 28.0 °C. If the temperature of the gas sample is raised to 43.1 °C holding the volume constant, the average molecular speed will a) not enough information to answer the question b) decrease c)remain the same d) increase -Which of the following statements is true for real gases? Choose all that apply. Attractive forces between molecules cause a decrease in pressure compared to the...
Which one of the following statements is not correct? a. An increase in temperature causes an increase in gas pressure because the average force of molecules colliding with the walls of the container increases. b. An increase in temperature causes an increase in gas pressure because the frequency of molecules colliding with the walls of the container increases. c. Real gases deviate from ideal gases because of the finite size of the molecules and the attractive and repulsive interactions between...
Which of the following statements is true for ideal gases, but is not always true for real gases? Choose all that apply Collisions between molecules are elastic. OThe size of the molecules is unimportant compared to the distances between them. There are no attractive forces between molecules. O Molecules are in constant random motion.
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...
In general, real gases behave most ideally at temperatures and pressures. The behavior of real gases can be described using the van der Waals equation [P+(ma/V2](V-nb) = nRT The values of a and bare given below for the two real gases xenon and argon The gas in which deviations from ideal behavior due to intermolecular forces are expected to be the largest is The gas that would be expected to behave least like an ideal gas at high pressures is...
In general, real gases behave most ideally at temperatures and pressures. The behavior of real gases can be described using the van der Waals equation [P+(nʼa/V2)](V-nb) = nRT The values of a and b are given below for the two real gases oxygen and methane. The gas in which deviations from ideal behavior due to intermolecular forces are expected to be the smallest is The gas that would be expected to behave most like an ideal gas at high pressures...
1. Which of the following statements is not consistent with the kinetic-molecular theory of gas? a. The volume occupied by the gas molecules only becomes significant at very low pressures b. A given volume of gas is mostly empty space except near the condensing point c. Except near condensing point, the attractive forces between gas molecules are very small d. The attractive forces between the molecules only becomes significant at very low temperatures 2. Which of the following statements does...