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An excess of zinc metal reacts with 500. mL of 12M hydrochloric acid and produces 48.8 L of hydrogen gas at 20 degrees C and 750 torr. a)Determine the mass of zinc metal reacted b)Determine the percent yield for the reaction
a solution is made by mixing 20.0 mL 0.4 M NaCH3COO with 30.0 mL 0.4 M CH3COOH, calculate the pH? For acetic acid, Ka = 1.76 x 10-5.
determine the freezing point of this solution If 18.0 grams of a nonelectrolyte that has molar mass = 44.2 g/mol are combined with 110.0 grams of the solvent,?
What masses of calcium sulfate and phosphoric acid can be produced from the reaction of 1.0kg calcium phosphate with 1.0kg concentrated sulfuric acid (98% H2SO4 by mass)?
Calculate the solubility of Ni(OH)2 in a) distilled water and b) at pH of 4.0. Justify your answer. I know I need to use a mass balance ans the reaction for disolution is
How many liters of H_2 would be formed at 704 mm Hg and 14 degrees C if 21.5 g of zinc was allowed to react?
Four (4.00) moles of a perfect gas at 250.0 K and 1.50 bar pressure undergo a reversible isothermal compression until the pressure becomes 3.00 bar.
How much ice(in grams) would have to melt to lower the temperature 352ml of water from 25degrees celcus to 5 degrees celcus? ( assume the density of water is 1.0g/ml)
A solution has a volume of 2.0 L and contains 36.0 g of glucose (C6H12O6). If the molar mass of glucose is 180 g/mol, what is the molarity of the solution.
Describe in brief the risk connected with solutions of 1M NH 3 , 1M HCl, and 1M NaOH?
Is heat absorbed or evolved in the course of this reaction? Calculate the amount of heat transferred when 45.0 g of CH3OH (g) is decomposed by this reaction at constant pressure.
How many moles of CO(NH2)2 are present in 105 g of water, if the freezing point of the solution is -4.02C? kf(water) = 1.86 K · kg/mol.
How much heat is required to warm 221 g of ice from -44.7°C to 0.0°C, melt the ice, warm the water from 0.0°C to 100.0°C, boil the water, and heat the steam to 173.0°C?
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