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Write a balance equations for both half-reactions for the redox. combine them to determine the overall balanced redox equation?
Calculate the pressure that must be applied in order to increase its density by 0.08 percent.
Calculate the molar enthalpy of combustion of Phosphorous when this combustion process was carried out under the constant pressure?
Compare this temperature with the true boiling point of N2. The boiling temperature is the temperature at which the areas under the two van der Waals loops are equal. In order to solve the problem
If 4 g of CuSO4 is dissolved in 9.0x10^2 mL of 0.40 M aqueous NH3, what are the concentrations of Cu2+, Cu(NH34 2+, and NH3 at equilibrium? (Kf = 5x10^13)
Determine the value of K (the thermodynamic equilibrium constant) at each temperature. b) Assuming that ?H°rxn is independent of temperature, determine the value of ?H°rxn from these data.
Use Charles's law to calculate the volume the gas will occupy if the temperature is increased to 170.5^circ C while the pressure is held constant.
A solution of ethanol (C2H5OH) in water is prepared by dissolving 60.0 mL of ethanol (density = 0.79 g/cm3) in enough water to make 235.0 mL of solution. What is the molarity of the ethanol in this solution?
A 20.00mL sample of H3Y was titrated with 0.1000 M NaOH. The first equivalence point was reached after the addition of 14.98mL of base. The second equivalence point was reached after the addition of 30.03mL.
What is the theoretical concentration of the 2,6-dichloroindophenol solution? What is the theoretical volume of 2,6-dichloroindophenol needed to neutralize 10mL of the vitamin C standard solution?
This indicates that the solution is now more acidic, and the reaction shifts to the right, working to lower the concentration of hydrogen ions, and return to equilibrium
When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 27.6 g of carbon were burned in the presence of 87.2 g of oxygen, 13.6 g of oxygen remained unreacted. What mass of carbon dioxide was produced?
What is the maximum amount of silver (in grams) that can be plated out of 4.8 {rm L} of an {rm{AgNO}}_3 solution containing 3.6 % {rm Ag} by mass? Assume that the density of the solution is 1.01.
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