Find out the mass of sodium sulphate is required to prepare
Find out the mass of sodium sulphate is required to prepare the 1.26 liters of such a solution when a solution is to be prepared with a sodium ion concentration of 0.542 mol/L.
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Assume you invest $580 at 10% compounded continuously. Write the exponential function to model amount in the investment account.
At 25.0C determine the entropy of fusion of a compound given that its enthalpy of fusion is having 32 kJ/mol at its melting point of 146C and the molar heat capacities of the liquid and solid forms are 28 J/(K mol) and 19 J/(K mol), respectively.
Determine the total pressure and the partial pressure of the final mixture when an 11L vessel contains 1.0 molN2 and 2.0 mols H2 at 298.15 K initially. H2 reacts withN2 to form NH3.
Determine the function which models number of hours of daylight t days after January 1. Suppose that year has 365 days and that spring equinox, when day is 12 hours long, is on 80th day of year.
If the sodium is irradiated with light of 439 nm, determine the maximum possible kinetic energy of the emitted electrons? Discuss in detail.
Calculate the maximum number of electrons that can be freed by a burst of light whose total energy is 1.00μJ? Explain in detail.
Find out the concentration of the final solution when a 24.7 mL, 1.66 MKMnO4 solution is mixed with the 16.7 mL of 0.755 M KMnO4 solution.
Account pays 4% compounded annually. Suppose that income tax on earned interest is 30%. Which of the given plans produces the larger balance after all income tax is paid?
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