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Suppose 25.0 g of solid NaOH is added to 1.5 L of an aqueous solution that is already 2.4 M in NaOH. Then water is added until the final volume is 4.00 L. Determine the concentration of the NaOH in the resulting solution.
If 125 calories of heat is applied to a 60.0 grams piece of copper at 21.0 degrees Celsius, what will the final temperature be? The specific heat of copper is 0.0920 calories per grams times Celsius.
Assume that only a single stream exits the fuel cell. What is the flow rate of each of the species leaving the fuel cell? Not that the flow rates given to correspond a fuel cell rate at approximately 50kW using 2004 technology.
Calculate the quantity of NH3 is produced upon reaction of 4.0 moles of water and 65.0 g of CaCN2.
How many moles of methane occupy a volume of 2.00 l at 50.0*C and0.500 atm? (R=0.0821 atm*L/molxK)
consider the following reaction, equilibrium concentrations and equilibrium constant at a particular temperature. determine the equilibrium concentration of NO2 (g)
If 3.00 moles of ZnS are combined with 4.00 moles of O2 how many moles of ZnO can be produced and how many moles of the excess reactant will be left over?
what is the concentration of H2 in the water in grams per milliliter? (See Appendix G in your textbook for the vapor pressure of water.)
The Planck distribution gives the energy in the wavelength range dA at the wavelength A. Calculate the energy density in the range 650 nm to 655 nm inside a cavity of volume
What is the buffer solution? What characteristics make this solution a buffer solution?
Important information about balanced chemical equation, 1. If 1 mole of Al4C3 has a mass of 144g and carbon has a mass of 12g, what is the atomic mass of aluminum?
Calculate the pH after the addition of 0.00mL, 20.00mL, 24.00mL, 25.00mL, 26.00mL, 35.00mL, 44.00mL, 45.00mL, 46.00mL and 50.00mL of 0.200 M HClO4.
A solution of ethanol (C2H5OH) in water is prepared by dissolving 57.0 mL of ethanol (density = 0.79 g/cm3) in enough water to make 255.0 mL of solution.
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