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A 50.0 gram piece of iron at 152 degrees celsius is dropped into a 20.0 grams of Water at 89 degrees Celsius in an open thermally insulated container. How much water would you expect to vaporize, assuming no water splashes out? The specific heats of iron and water are 0.45 and 4.21 J/gC respectively, and Delta Hvap= 40.7 kJ/mol of Water.
Air is a mixture of N2,O2,Ar,Co2,Ne,He,CH4,lessor amounts of the other gases and possibly substantial amount of H2O in vapor form.
When the sodium atom becomes a sodium ion, how does the size and electron configuration of the sodium atom change?
The concentration of phosphoric acid in Coke is approximately 106.0 mg/mL. Assuming phosphoric acid is the only acid in Coke, calculate the pH of a 355 mL can of Coke.
Furoic acid, HC5H3O3, has a Ka value of 6.76 10-4 at 25C. Calculate the pH at 25C for a solution formed by mixing 28.0 mL of 0.260 M HC5H3O3 and 23.0 mL of 0.21 M NaC5H3O3 and diluting the total volume to 125 mL.
A 29.0-g sample of ice at -11.0°C is mixed with 113.0 g of water at 71.0°C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings.
The reactant concentration in a first-order reaction was 6.80×10-2 M after 10.0 s and 4.40×10-3 M after 65.0s . What is the rate constant for this reaction?
A graduated cylinder contains 133 mL of water. A 17.0 g piece of iron (density = 7.86 {g/cm^3}) and a 23.0 g piece of lead are added. What is the new water level in the cylinder?
How much heat is liberated by the combustion of 183 g of hydrogen? ΔHcomb = -286 kJ/mol.
The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) PCl3(g) + Cl2(g) Calculate the equilibrium partial pressures of all species when PCl5(g)
A 4.369 g sample of metal is placed in a flask. Water is added to the flask and the total volume in the flask is read to be 126.4 ml. The mass of the water
Write the formula of the reactants and products-including the symbols for the state- (s), (l), (g), (aq)- then balance the equation.
A sample of MgCl2 is known to be contaminated with NaCl. A 3.47-g portion of the sample is dissolved in water and treated with an excess of AgNO3 solution.
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