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Q.2 For the nitrogen molecule, calculate the following: i) Translation energy per molecule at 300K ii) Translation energy per mole at 300K iii) Number density at 298.2K iv) Concentration at 298.2K
KE per molecule = 3/2 kT = 3/2 * 1.38e-23 * 300 = 6.21e-21 (J) KE per mole: 3/2 RT = 3.74 kJ In the next calculations, it is suggested...
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What is the molarity of a solution with a volume of 5 L made with 600g of NaOH?
Molarity= Mole of the Solute/Volume of SolutionMole of Solute=Mass/Molar Mass of NaOHMolar Mass of NaOH=40g/moleMole=600g÷40g/mole= 15MolMolarity=15÷5= 3MMolarity = 3M
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0.690 moles of solid CO2 is put in an empty sealed 4.40 L container at a temperature of 90ºC, what is the pressure in the container?
Pressure in the container=1.28atm
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600g of CaCOg decomposes in 2 minutes, what is The rate of reaction
Rate = Mol/minMolar Mass of CaCo = 100= 600/100 = 6 mols6/2 = 3 Mols/minute
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The mass of an empty container is 93g the mass of the container filled with water is 119g what is the volume of the container? the density of water is 1g/cm^3 answer in terms of cm^3
119-93 = 26V = Mass/density= 26/1= 26ml
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Calculate the temperature to which a .400 L sample of gas at 1.00 atm and 0 degrees celcius must be heated at a constant pressure for the volume to change to 1.00L
If P = const we can use Charles's law. Due to it we have V1/T1 = V2/T2 From this equation we get that T2 = (T1*V2)/V1 = (273 K*1 L)/4...
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A sample of gas expands from 2.00L to 3.00L against a constant pressure of 1.0atm. Calculate the work done in joules. (1L.atm= 101.3J)
101.3 Jouls
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. A steel tank contains CO2 at 300K and a pressure of 10 atm calculate the internal
gas pressure when the tank gas
We need to calculate the internal gas pressure when the gas tank is heated or cooled (not provided in the question). Let's say that final temperature of the tank and...
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A vessel of 2×10⁻³m³ volume contains 0.036 kg of Argon at 300K. Calculate its pressure using ideal gas equation. ( Atomic mass of Ar = 39.9u).
V= 2x10-3m3 = 2dm3m= 0.036Kg = 36gT= 300KR= 0.0821L.atm/k.molnumber of moles, n= mass/Molar mass = 36/39.9= 0.9molPV= nRTP= nRT/Vp= 0.9x0.0821x300/2P= 11.08atm
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The volume of a sample of hydrogen gas at 0.997 atm. is 5.00L. What will be the new volume if the pressure is decreased to 0.977 atm. Temperature is constant.
P1 x V1 = P2 x V20.997 x 5.00 = 0.977 x V2V2 = (0.997 x 5.00) / 0.977 = 5.10 L
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