QUESTION 4 the attractions between the gas particles should be For a real gas to approach...
Please double check my #3 and help on 4! QUESTION 3 Cl2 CH4 According the the kinetic molecular theory of gases, rank the following molecules at STP by their average kinetic energy: H2 (In each blank type <, =, or > as appropriate.) QUESTION 4 temperature A real gas will deviate least from the properties of an ideal gas, at volume, and pressure, In other words, conditions that make the real gas properties close to the ideal gas properties. (Fill...
QUESTION 3 0.5 points Save Answer According the the kinetic molecular theory of gases, rank the following molecules at STP by their density: H2 CH4 Cl2 {In each blank type <; =, or > as appropriate.} QUESTION 4 0.5 points Save Answer pressure, A real gas will deviate most from the properties of an ideal gas, at volumes, temperature. In other words, what conditions are the least ideal. {Fill in each blank with the word high, large, small or low...
A real gas will deviate most from the properties of an ideal gas, at ______pressure, ______volumes, ______temperature. In other words, what conditions are the least ideal.{Fill in each blank with the word high, large, small or low as appropriate.}
Homework Assignment Week 4 Chapter 10 1. Under which set of conditions will a real gas be least likely to act as an ideal gas? A. High temperature and high pressure B. High temperature and low pressure C. Low temperature and high pressure D. Low temperature and low pressure 4. If the pressure of an ideal gas is doubled from 1.0 atm to 2.0 atm and its temperature is halved from 80.0°C to 40.0 °C, the volume of the gas...
ASAP please type in the answer! ASAP PLEASE TYPE IN THE ANSWER Question 4 (2 points) The shore of the Dead Sea is the lowest point on land, not covered by water. This point is 423 meters below sea level. Using equations 10.3 and 10.4, the temperature required to boil water on the shore of the Dead Sea would be A degrees Celsius. Round your answer to 1 decimal place. Question 5 (2 points) Explain why gases experience more ideal...
Part A Which conditions can cause nonideal gas behavior by 1) decreasing the space between gas particles or 2) by slowing gas particles so that interactions are significant? 1) high pressure; 2) low temperature 1) low pressure; 2) high temperature 1) low pressure; 2) low temperature 1) high pressure, 2) high temperature none of the above Submit Request Answer
The ideal gas law describes the relationship among the volume of an ideal gas (V), its pressure (P), its absolute temperature (T), and number of moles (n): PV=nRT Under standard conditions, the ideal gas law does a good job of approximating these properties for any gas. However, the ideal gas law does not account for all the properties of real gases such as intermolecular attraction and molecular volume, which become more pronounced at low temperatures and high pressures. The van...
22- In what condition a real gas behaves like ideal gas? a) High pressure, high temperature b) High pressure, low temperature c) low pressure, low temperature d) low pressure, high temperature 23- Which of the following statements are true? a) σ bonds form from side to side overlap of atomic orbitals b) TT bonds form from side to side overlap of atomic orbitals c) σ bonds form from head to head overlap of atomic orbitals d) TT bonds form from head to head overlap of atomic orbitals e) Both b...
Question 1 (1 point) Calculate the density of nitrogen gas in a 4.32 L container at 1.0 atm and 25°C. Question 1 options: 0.57 g/L 0.74 g/L 1.15 g/L 1.31 g/L 1.56 g/L Save Question 2 (1 point) What volume is occupied by 1.00 kg of nitrogen gas at 5.00?C at a pressure of 735 Torr? Question 2 options: 1686 L 1242 L 843 L 738 L 621 L Save Question 3 (1 point) The ideal gas law fails to...
In the boxes below, draw a diagram of what you think ten gas particles would look like if you could zoom really close in to see them. Use • for particles, → to show their movement. Bigger arrows mean more velocity. The box is the container. Low temperature High temperature High volume low volume High pressure Low pressure