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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.
An equilibrium mixture of this reaction(NH4HS(s)?NH3(g)+H2S(g)) at a certain temperature was found to have [H2S]= 0.350M and [NH3]= 0.276M .What is the value of the equilibrium constant (Kc) at this temperature.
Historically, the solid residue that is left after the Dichloromethane -or methylene chloride (CH2Cl2 )solution is evaporated has a lower melting point that its literature value, due to impurities.
Compute the number of moles of Chlorine atoms in 3.01×10^24 formula units of magnesium chloride,MgCl2 .
In Horner-Wadsworth-Emmons reaction, a 1,2-disubstituted alkene was produced in which the olefinic protons exhibited at vicinal coupling of 9.0 Hz in the 1H NMR. What is the stoichiometry of the double bond.
Calculate the minimum energy a photon must have to produce an electron hole pair in an extrinsic semiconductor of band gap 1.0 electron volts.
Determine the numbers of moles of S8 that are required to make 0.600 moles of SF4.
Step-wise solution to a numerical problem related to a flocculation-based water treatment plant having a flow of 25 MGD. The plant is to employ alum coagulation.
Determine how will this error control the final computed percentage of CH3COOH in the vinegar
Given that Iron(III) oxide or ferric oxide (molar mass = 159.7 g/mol) reacts with Carbon monoxide (molar mass = 28.0 g/mol).
Determine ?H for the formation of one mole of aluminium(III) oxide, Al2O3(s) from the elements?
compute the energy levels for the rotation perpendicular to its symmetry axis at J=1. T he bond length in the 14NH 3 =101.2 pm and NHN bond angle 106
Describe in brief the risk connected with solutions of 1M NH 3 , 1M HCl, and 1M NaOH?
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