If a 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature? 10. Equation/ formula: 11.Universal Gas Constant: 12. Solution:
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- Explain the relations between microscopic and macroscopic quantities in a gas?Hi, could I get some help with this macro-connection physics problem involving the Ideal Gas Law? The set up is: What is the average volume in nm3 (cubic nanometers) taken up by molecules of an ideal gas at room temperature (taken as 300 K), and 1 atm of pressure or 101325 N/m2 to 4 digits of precision if kB = 1.38e-23 J/K and 1 nm = 10-9 m? Thank you.(II) What is the pressure inside a 38.0-L container holding105.0 kg of argon gas at 21.6°C?
- (II) Compare the value for the density of water vapor atexactly 100°C and 1 atm with the value predictedfrom the ideal gas law. Why would you expect a difference?Would you expect γ to be larger for a gas or a solid? Explain how?2. If the pressure exerted by a gas at 77 °F in a volume of 1L is 5 atm, how many moles of gas are present?
- 3. How many moles of gas are in a bike tire with a volume of 0.002 m3, a pressure of 700,000 Pa (a gauge pressure of just under 101.53 PSI), and at a temperature of 18°C?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.Hi, could I get some help with this macro-connection physics problem involving moles and the Ideal Gas Law? The set up is: How many moles are there in a cubic meter of an ideal gas at 100 degree celsius (C) to 4 digits of precision with a pressure of 0.25 atm, assuming 1 atm = 101325 N/m2 with kB = 1.38e-23 J/K and NA = 6.022e23? Thank you.
- What is the volume of 67 mol of gas, in the unit of m3, when the pressure is 87 kPa and the temperature is 68°C? Use R = 8.314 J/(K mol) for the gas constant. Be careful with units, and remember that the temperature must be in Kelvin when you use the ideal gas equation.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.At standard temperature and pressure, a gas has a density of 0.089 kg/m3. What volume (in m3) does 1.84 kg of hydrogen occupy at standard temperature and pressure [round your final answer to one decimal place]?