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An electron in the hydrogen atom makes a transition from an energy state of principle quantum number n to the n=1 state. If the photon emitted has a wavelength of 95nm, what is the value of n?
On this problem I tried using the equation 1/wavelength = R (1/n^2 - 1/n^2)= 1/ (9.5x10^8m) = 1.097x10^7 m^-1 (1/1 - 1/n^2)Not sure if im using the wrong equation, or if im getting tripped up in the math, but I am not getting the answer I am looking for.
One of the lines in the Lyman series of the emission spectrum for hydrogen results when an excited electron in the n=2 level returns to ground state. What is the energy in kJ of the photon emitted when this transition occurs.
So far I have:
E = Ef - EiE = hv = -2.18 x 10^-18J(1/1 - 1/4)= -2.18x10^-18J (.75)= -1.635 x 10^18 J x 1kJ/1000J =
What is the pH of a buffer that results when 0.40 mol NaHCO2 is mixed with 100.0 mL of 2.00 M HCl and diluted with water to 250 mL (Ka of HCO2H=1.8*10^-4.
Calculate the heat required to raise the temperature of 1.5 L of a liquid with a density 0.75 g/mL and a specific heat of 2.2 J/g/K
After doing some analysis, the probe determines that the gas pocket contains an element that has an ionization energy of I= 1350 kJ/mol and an electron affinity of EA=32.0 kJ/mol . What is the identity of this element.
Consider all possible transitions from the initial state to the final state of the hydrogen atom described above. Calculate all possible values of the wavelength of the emitted radiation.
A sample of indium sulfate, In2(SO4)3, contains 0.0446 moles of oxygen. What mass of indium is present?
given the balanced equation representing a reacction: 2C2H6+7O2=4CO2+6H2O determine the total number of moles of oxygen that react completely with 8.0 moles of C2H6
magnesium chloride are used to make a solution with a final volume of 1.74L, then waht is the final Mg2+ ion concentration in ppm?
Important information about Nitration, Explain why nitration of 1,4-dichloro-benzene yields the mononitro derivative while N,N'-diacetyl-1,4-phenylenediamine forms
During the synthesis of methyl 3-nitrobenzoate, when the reaction mixture is poured on ice, the product separates out as a solid. Why
On the right, it is single bonded to the C which is single bonded to each H. The other form I have is the mirror immage of this one. What is the last form
The standard enthalpy change for the reaction of 1.85 moles of CO(g) at this temperature would be -524 kJ. Ho = -506.5 + 344 * -173.1 divide it all by 1000= -566.0kj i dont understand how they got -566.0kj, when i put it in my calculator
Given that delta r H = 40.67 kj/mol for vaporization of H20 at 100 degrees celcius, what is delta S tot for vaporization of 1 mol of water at 1 bar pressure at 125 degrees celcius? Is this process spontaneous?
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