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A coffee-cup calorimeter contains 140.0 g of water at 25.2 *C. A 122.0 g block of copper metal is heated to 100.4 *C by putting it in a beaker of boiling water. The specific heat of Cu(s) is 0.385 J/g*K . The Cu is added to the calorimeter, and after a time the contents of the cup reach a constant temperature of 30.2 *C.
A 12.0 gas cylinder has been filled with 5.40 moles of gas. You measure the pressure to be 5.00 atm. What is the temperature inside the tank? Express your answer numerically in degrees Celsius.
Calculate the time needed for the amount of ethane to fall from 1.43 10-3 mol to 2.00 10-4 mol in a 500. mL reaction vessel at 700.°C.
The second-order reaction, 2 Mn(CO)5 Mn2(CO)10 has a rate constant equal to 3.0 x 109 M-1s-1 at 25°C. If the initial concentration of Mn(CO)5 is 1.0 x 10-5 M.
Write the Bronsted-Lowry chemical equation describing how HC4H7O2 behaves when add to water
You prepare a buffer solution by dissolving 1.77 g each of benzoic acid, HC7H5O2, and sodium benzoate, NaC7H5O2, in 900.0 mL of water.The pH of the buffer is 4.19. How much (in grams) of the buffer (benzoic acid), would you add to the 900.0 mL of ..
A sample of gas occupies 1.55L at STP. Remember, pressure at STP is 1.0 atm. What will the volume be if the pressure is increased to 50 atm while the temperature remains constant
describes the chemical change. what about for a solution of calcium chloride and a solution of mercury (I) nitrate
Calculate the pH at the equivalence point for titrating 0.170 M solutions of each of the following bases with 0.170 M HBr. a)sodium hydroxide
Calculate the empirical formula for a chemical compound which gives the following analysis: 65.2 g scandium and 34.8 g oxygen.
While shutdown, the core accidentally went critical and the reactor pressure vessel rose in temperature and was hot for two hours, but all instrumentation has failed and no one is sure what the temperature was.
A solution to replace potassium loss contains 40.mEq/L each of K+ and Cl-. How many moles each of K+ and Cl- are in 1.5L solution
The molecular mass of an unknown compound was determined by measuring the freezing point depression of an aqueous solution of the compound
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