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Dr Rebel
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Yes! Find something that's 1-million years old and listen to what it has to say about it's existence 1-million years ago. I'm not trying to be funny here... Einstein said, 'To understand the secrets of the universe, one must first learn it's language'. The
I don't know what the 'morality' would be but the Molarity = moles solute / Volume of Solution in Liters Molarity = [(moles NaHCO3/Soln Vol in Liters)] moles NaHCO3 = (10.60g/84g/mol)= 0.1262 mole Vol(L) = 0.250 L Molarity(M)= (0.1262/0.250)Molar = 0.505M
Carbonate becomes a diprotic acid
1. Calculate moles of H2S from Rxn 2. Cal. Vol H2S at STP = moles H2S x 22.4 l/mole at STP 3. Convert Vol H2S at STP to Vol at 18C & 729 mmHg using Ideal Gas Law Ans => 2.489 Liters H2S
VP(HOH) = 12.8 Torr at 15C* (Google VP(HOH)at 15C) VP(HOH) + VP(CO)= Total Pressure 12.8Torr + VP(CO) = 752Torr VP(CO) = (752-12.8)Torr = 739.2 Torr
Use Ideal Gas Law PV = nRT. R = 0.08206 L-Atm/mol-K V = 29.85 L P = 1.83 Atm n = 1.83 mole T = ? in Kelvin => Celcius = K - 273
gms of CuSO4-5HOH = [Molarity needed][Volume needed (Liters)][formula Wt CuSO4] / [Purity fraction CuSO4 in pentahydrate] =[(0.03M)(0.100L)(160g/mol)]/[0.64]=0.75gms CuSO4-5HOH + Solvent up to but not to exceed 100 ml total volume.
See Anonymous on Friday, October 28, 2016 at 4:38pm.
2Na(s) + Cl2(g) => 2NaCl(s) Convert given data to moles and divide each by the respective coefficient in the balanced equation. The smaller value is the limiting reagent and the larger value is the one that will remain in excess. moles Na =
Molarity = moles solute / Vol Solution in Liters. Al2(SO4)3 => 2Al^+3 + 3SO4^2- [Al2(SO4)3] = [18/fwt Al2(SO4)3]/0.201 L Then [Al^+3] = 2[Molarity of Al2(SO4)3], and [(SO4)^2-} = 3[Molarity of Al2(SO4)3]
At 1 atm = 760 Torr and 0^oC, 1 mole of any gas contains 6.02E23 particles of gas and occupies a volume of 22.4 Liters. This number of particles would be reduced by (1.96E-8/760)if at 0^C. At 23^oC = 296K the number of particles would be also be reduced
OK, if the equation is as written, Ms Sue is 100% correct.
Your equation should be Y=0.04x+192 Slope 0.04 and Y-intercept at x=0 is 192. You can plot the equation by choosing a series of x-values, substituting each into the equation to obtain the related y-value. Plot (x,y) series.
Density = mass/Volume solving for mass mass = Density x Volume mass = (0.9977g/ml(45.5-ml) = 45.3953 grams. Are you sure 'mass of water' is all you needed? How about 'Heat of Reaction'? q=mc(delta Temp) q = (45.3953g)(4.184J/g-C)(41.5 - 22.6)C =
q=mc(delta-T) = 80g(4.184j/g-C)(1.5 C)= 502 joules x (1 Kj/1000 joules) = 0.00502 Kj = 5.02E-4Kj
Review 'Method of Mixtures' type problems.
You will need at least the initial concentration of SO2 and equilibrium concentration of SO3.
There is no one best way. Generally speaking, Keq values would depend upon the method of measuring concentration values of components of reaction at equilibrium. In some cases titrations can give great results while for reactions with visible chromaphores,
Correction - BaCl2 on product side of rxn.
(65ml)(0.320M Ba(OH)2)+(65ml)(0.640M HCl) =>0.065(0.32)mole Ba(OH)2+ 0.065(0.64)mole HCl =>0.0208mole Ba(OH)2 + 0.0416mole HCl =>0.0208mole Ba(OH)2 + 0.0416 mole HOH gram yield HOH = 0.0416mole(18g/mole) = 0.749g HOH Delta T = (26.34-21.98)C = 4.36C q =
q(Al) + q(HOH) = 0 mcT(Al) + mcT(HOH)= 0 [(25)(0.903)(T-57.4)] + [(25)(4.184)(T-25) = 0 Solve for T.
(0.084/22.4)= (0.15)V ... solve for V
[16.6(0.128)(t-138]+[23.4(4.184)(t-8.68)]=0 Solve for t.
Making solutions... Solutions are prepared form one of 3 sources, Manufactured Solid Stock, Manufactured Liquid Stock or Laboratory Concentrate. For mass of solid mfg stock needed (grams) use formula... gms = [(Molarity needed x Vol needed(in liters) x
It means your answer (experimental result) is 1.4% above the accepted value. To call this 'accurate' based on a %Error calculation would be unwise unless there is a published accepted %Error 'range' for the experiment instruments used to collect the raw
As I understand it, the ‘frequency factor’ does not have units. What you are showing in the posted question is ‘rate constant’ calculated from the Arrhenius Equation. The Arrhenius Equation is derived from the frequency factor. From the KM Theory f
