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Consider 20.0 moles of CO2 in a 1.0 liter container at 300.0 K. What is the pressure predicted by the van der Waals equation? The ideal gas law constant is 0.08206 [L•atm] / [mol•K]. For CO2, the pressure correction constant is 3.658 L2•atm / mol 2, and the volume correction constant is 0.04286 L / mol.
How is acetyl chloride produced? If 915 gallons is produced and shipped, will DOT require the carrier to display the flammable placard? Explain your answer.
If the volume of ocean water is 5.4*10^20 contains 4.1 percent sodium chloride ("salt") by mass and the density of the water is 1.86 g/mL.
2SO2(g) + O2(g) 2SO3(g) Suppose the volume of this system is compressed to one-half its initial volume and then equilibrium is reestablished.
A quantity of gas under a pressure of 1.78 atm has a volume of 550 cm square. the pressure is increased 2.50atm while the pressure remains constant what is the new volume.
Solving this question helps the student to understand how to find molecular formula using moles and mass and What is the molecular formula of this compound?
How many moles of CF4 can be produced when 5.00 mol C react with 12.00 mol F2.
Imagine that you have a 5.00L gas tank and a 4.50L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch.
Determine the temperature change is caused by heat energy and using a beaker that contains 100 mL of H 2 O thermally insulated from its surroundings, one mol of solid CaCl 2 is mixed and solution is stirred
Explain what is methylphenidates purpose and its chemical structure? Also determine how does it affect the body of human beings ,what makes up that compound , what organs do it impact?
The tabulated mass of Cl is 35.45 amu. The two dominant isotopes of naturally occurring Cl are 35Cl (34.97 amu) and 37Cl (36.97 amu).
Compute the molar mass of the noble gas krypton(Kr) in a natural sample, which is 2.2% 80 Kr (molar mass 79.91 g/mol),
Compute the difference in pressure between CH4 and an ideal gas if 14.0 moles of gas are in a 6.00 litres tank at the temperature of 21.1 degree celsius . The van der Waals constants for CH4 are a =2.300 L^2 x atm/mol ^2 and b=0.0430 L/mol.
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