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Ionization energy is the energy needed to eject an electron from an atom. Compute the ionization energy of a hydrogen atom in its fourth excited state (n = 5).
An evacuated (empty) 276 mL glass bulb weighs 129.6375 g. Filled with an unknown gas, the bulb weighs 130.0318 g. Calculate the gas density in g/L.
volume of 20.0 mL of a 0.190 M HNO3 solution is titrated with 0.550 M KOH. Calculate the volume of KOH required to reach the equivalence point.
Radio waves are very low energy forms of electrmagnetic radiation. What is the energy of a mole of radio wave photons with a
The vapor pressure for methanol and ethanol at 50 C is 406 and 222 Torr, respectively. Calculate the total vapor pressure of a mixture at 50 C that contains 0.2 mol of methanol and 0.1 mol of ethanol.
Calculate the partial pressure of ozone and the number of ozone molecules per liter of air if the tempreture and pressure were 20.0 degrees C and 758 mmHg, respectively.
Determine the concentration of CO32- ions in a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 x 10-7 and Ka2 = 5.6 x 10-11."
A hydrogen molecule in it's ground vibrational state with KE=10eV coollides with heavy atom metal surface and no energy is transferred to the surface. The surface can be modeled as an infinite potential wall.
When 0.800 g of Ca metal is added to 200.0 mL of 0.500 M HCl(aq), a temperature increase of 13C is observed.Assume the solution's final volume is 200.0 mL, the density is 1.00 g/mL.
An increase in the temperature of the reactants causes an increase in the rate of reaction. The best explanation for this behavior is that as the temperature increases
A 65.00 mL sample of HNO3 solution is neutralized by exactly 34.16 mL of 0.5841 M Ba(OH)2. What is the molarity of the HNO3 solution?
Calculate the enthalpy change in kJ when 21.6g of H2S is burned. 2H2S(g) + 3O2(g) --> 2SO2(g) + 2H20(g) Change in H=-1036kJ/mol
Calculate the standard heat of reaction, or for this reaction using the given data. Also consider that the standard enthalpy of the formation of elements in their pure form is considered to be zero.
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