1 Answers
Call
Talk Doctor Online in Bissoy App
What phase changes, if any, occur if carbon dioxide initially at -80 degrees celsius and 8.0 atm is allowed to warm to -25 degrees celsius at 5.0 atm?
Using law PV = nRT, you can see, that if n,R = const, and T and P are used for some processes,V-volume is the one,that can be changed.
1 Answers 1 views
Calculate q, w, delta E and delta H for the process in which 2.0 moles of N2O gas are cooled from 165 degrees Celsius to 55 degrees Celsius at a constant pressure of 5 atm.
delta E=0 delta H = Cp delta T delta U = Cv delta T + p delta V q = delta H w = p delta V delta U =...
1 Answers 1 views
The density of gas molecule A is double than that of gas molecule B at 27<sup>0</sup>C. How many times the root mean square speed of gas A is slower than that of gas B at this temperature?
Root mean square= 1/√dSo RMS wil be decreas by 1.414 times
1 Answers 1 views
A sample of an ideal gas has a volume of 3.60 L at 13.40 degrees Celsius and 1.30 atm. What is the volume of gas at 24.60 degrees Celsius and 0.990 atm
Combined gas Law P1V1 / T1 = P2V2 / T2 P1 = 1.30 atm V1 = 3.60 L T1 (must be in Kelvin = 13.40 deg C + 273.15) =...
1 Answers 1 views
What is the root mean square of bromine molecules at 23°C and 1.5atm
214.808519 m/s
1 Answers 1 views
A volume of carbon dioxide gas equals 20.0 L was collected at 23 degrees celsius and 1.00 atm pressure. what would be the volume of carbon dioxide collected at 23 celsius and 0.830 atm?
General gas equation:p1*V1/T1=p2*V2/T2p1= 1atmV1= 20 LT1=T2=23 oCp2=0.83 atmV2 - ?V2=p1*V1/p2 = 20/0.83 = 24.1 LAnswer: 24.1 L
1 Answers 1 views
Liquid bromine (Br2) has a density of 2.91g/mL. How many molecules of bromine are contained in a 8.50-mL sample of bromine?
m = V×ρm(Br2) = 8.50 mL × 2.91 g/mL = 24.735 gM(Br2) = 159.808 g/moln = m/Mn(Br2) = 24.735 g / 159.808 (g/mol) = 0.154 molOne mole of Br2 molecules...
1 Answers 1 views
A 79.9g sample of bromine contains approximately 1 mole of bromine atoms. How many bromine atoms are in a .80kg sample of bromine?
At first, kilogrammes should be turned into grams:m=80×1000=80000(g).Then, mass should be divided by molar mass:n=m/M=80000/79.9=1001.3(mol).(The data is not very clear. If the point is not mistake, and there are .80...
1 Answers 1 views
A sample of hydrogen gas, H2, has a volume of 8.56L at 0oC and pressure of 1.5atm. Calculate the mass of H2 present in the gas sample.
We use the ideal gas equation.......PV=nRT n=PV/RT =(1.5 atm)(8.56L)/(0.082 lit-atmp/Kelvin mole)(273 K) n =0.573 moleMoles H2 is=0.573 molesAtomic mass of H is=1.00784 amuMass of H2 is =(1.00784 amu)(0.573 moles)Hence mass...
1 Answers 1 views
In a gas mixture composed of N2, Ne, and He, the partial pressure of N2 is 0.50 atm, that of Ne is 1.1 atm, and that of He is 0.80 atm. Calculate the mole fraction of each gas.
Mole fraction of N2- 0.208Mole fraction of Ne - 0.3Mole fraction of He - 0.458
1 Answers 1 views