Estimate the average spacing between the molecules of 1 mol of an ideal gas at a pressure of 1 atm and a temperature of 300 K
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A: Hi! Thank you for the question. As per honor code, we are allowed to answer three sub-parts at a…
a) Estimate the average spacing between the molecules of 1 mol of an ideal gas at a pressure of 1
atm and a temperature of 300 K.
b) 1 mol of liquid water occupies a volume of 18 cm. Estimate the spacing between molecules.
c) Use your result from part (a) to estimate the diameter of a water molecule.
d) Estimate the factor by which water expands when it boils
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- A sample of carbon dioxide (CO₂) has a volume of 0.04 m³. The gas has a pressure of 1.6 x 106 Pa and its temperature is 24 degrees C. List of atomic mass units can be found HERE a) What is the mass of the whole sample of gas? b) How many molecules are in the cylinder? c) What is the average kinetic energy per molecule? d) What is the rms speed of the molecules?The temperature of an ideal monatomic gas is increased from 25C to 50C. Does the average translational kinetic energy of each gas atom double? Explain. If your answer is no, what would the final temperature be if the average translational kinetic energy was doubled?8. The average energy of a mole of Einstein solid is given by: ӨЕ 3R0E Ē = 3R + 2 ӨЕ ет — 1 where E is the Einstein temperature and R the gas constant. Obtain expressions for the average energy at the limits of zero and infinite temperature and comment on your results.
- Learning Goal: To understand the ideal gas law and be able to apply it to a wide variety of situations. The absolute temperature T, volume V, and pressure p of a gas sample are related by the ideal gas law, which states that PV = nRT Here n is the number of moles in the gas sample and R is a gas constant that applies to all gases. This empirical law describes gases well only if they are sufficiently dilute and at a sufficiently high temperature that they are not on the verge of condensing. In applying the ideal gas law, p must be the absolute pressure, measured with respect to vacuum and not with respect to atmospheric pressure, and I must be the absolute temperature, measured in kelvins (that is, with respect to absolute zero, defined throughout this tutorial as -273°C). If p is in pascals and V is in cubic meters, use R = 8.3145 J/(mol · K). If p is in atmospheres and V is in liters, use R = 0.08206 L atm/(mol-K) instead. Part A A gas sample enclosed in a rigid metal container at…A container of nitrogen molecules is at a temperature of 37.0°C. What is the mass of a nitrogen molecule in atomic mass units? [Note: nitrogen is a diatomic gas.] а. b. What is the mass of a nitrogen molecule in kilograms? C. What is the average translational kinetic energy of the nitrogen molecules? d. What is the rms speed of the nitrogen molecules? е. What is the average rotational energy of a nitrogen molecule?Amanda discovers that the gauge pressure in her car tires is 2.50 ×105 Pa at a temperature of 35.0oC. The average volume of a single tire at that temperature is 10.0 L. 1.) Find how many moles of gas (air) are in one of Steve’s tires. 2.) Later Amanda travels to a place where the temperature is –40.0oF. She notices that the tires are looking low and estimates that each tire has lost approximately 1.0 L of its volume. What is the gauge pressure in the tire now?
- Problem 3. The viral coefficients of a gas at 20 °C and 11.5 bar are B = -138 cm³ mol¹ and C=7222 cmº mol². Calculate the V (molar volume) Z (compressibility factor) of the gas. Use the equation below (R = 83.14 cm³ bar mol-¹ K-¹). PV 2 = ² = (1 + = + =) Z RTa) An ideal gas occupies a volume of 1.6 cm3 at 20°C and atmospheric pressure. Determine the number of molecules of gas in the container. molecules (b) If the pressure of the 1.6 cm3 volume is reduced to 1.2 ✕ 10-11 Pa (an extremely good vacuum) while the temperature remains constant, how many moles of gas remain in the container? mol example of question a An ideal gas occupies a volume of 2.4 cm3 at 20°C and atmospheric pressure. Determine the number of molecules of gas in the container. 6.01e+19 molecules