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Write a net ionic equation for the precipitation reaction, if any, that occurs when aqueous solutions of the following ionic compounds are mixed. Cu(Ch3COO)2 and Na3PO4.
A gas has a volume of 10 L at 0 degrees C. What is the final temperature of the gas in C if its volume increases to 27 L? Assume that amount of the gas and its pressure remain unchanged.
Determination of the partial pressures of the gases - Find the partial pressure of each of these gases in the final product mixture.
Sketch the typical stress-strain curve for a metal and a ceramic. Using the sketch, indicate the following properties; elastic and plastic regions, yield points, Ultimate Tensile Strength (UTS), strain energy and fracture toughness.
Explain why the boiling point of an aqueous solution that is 1.0 m in glucose (C6H12O6) is 100.51oC whereas The boiling point of an aqueous solution that is 1.0 m in NaCl is 101.02 oC .
The rate constant for a certain reaction is = 5.70×10-3 s^-1. If the initial reactant concentration was 0.650 M, what will the concentration be after 14.0 minutes.
It required 16ml of a sodium hydroxide solution titrated against a standard solution of 0.79g of potassium hydrogen phthalate in water to reach equivalence point. What is the molarity of the sodium hydroxide?
An antacid tablet contraining calcium carbonate as an active ingredient required 9.53 mL or 0.0956 M H2S04 for comlete neutralization.
How many moles of CO(NH2)2 are present in 150 g of water, if the freezing point of the solution is -4.02C? kf(water) = 1.86 K · kg/mol.
how many milliliters of a stock solution of 2.00 m kno3 would you need to prepare 100.0 ml of 0.150M KNO3
Should you install a solar water heater? The average home has a 200 liter hot-water tank, which is effectively drained and replenished three times per day.
Data for the decomposition of hydrogen peroxide at some set temperature T is provided below. The rate law depends only on the concentration of H2O2
A 4.07 L sample of H2O(g) reacts at a temperature of 375°C and a pressure of 679 mm Hg. How many grams of NH3 can be produced?
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