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A hot air balloon can contain upwards of 16,000 L of gas (at STP)
how many combined molecules/atoms of air will be present?
how can the rate of reaction be accurately measure between calcium carbonate chips and hydrochloric acid
how many grams of oxygen are completely consumed in the production of 1.00 mole of Na2O
Aqueous solutions of potassium hydrogen sulfate and potassium hydroxide react to form aqueous potassium sulfate and liquid water. How many moles of potassium hydroxide are necessary to form 0.636 moles of potassium sulfate?
A quantity of NaOH of mass 1.1g is dissolved in water and made up to 250cm³ in a graduated flask. A 20cm³ of the solution neutralizes 20.4cm³ of a solution of acetic acid of ph=2.85
Calculate
a. Number of moles of NaOH in the 250cm³ solution
b. Number of moles of acetic acid in 1dm³ of the solution
State the volume of hydrogen gas produced at s.t.p when using 30g of Zinc is added to excess dilute hydrochloric acid at 33⁰C and pressure ( H= 1, Zn =65, Cl = 35.5 ) molar mass of gas ay s.t.p = 22.4dm³
The reaction goes to completion, but in the process of washing and drying the precipitate, some was lost. The percent yield for the reaction is 79.9%
79.9%. How many grams of precipitate are recovered?
precipitate recovered:
How many grams of the excess reactant remain? Assume the reaction goes to completion.
excess reactant remaining:
The reaction goes to completion, but in the process of recovering the product, some of it was lost. The the percent yield for the reaction is 82.2%.
82.2%. How many grams of product are recovered?
mass of product recovered:
How many grams of the excess reactant remain? Assume the reaction goes to completion.
mass of excess reactant:
Consider the following equation:
Ca(OH)2(s) + 2 HCl(aq) —> CaCl2(aq) + 2 H2O(l)
a) How many liters of 0.100 M HCl is required to completely react with 5.00 grams of calcium hydroxide?
b) If 15.0 grams of calcium hydroxide is combined with 75.0 mL of 0.500 M HCl, how many grams of calcium chloride
would be formed?
A solution is prepared by mixing 1.00 gram of ethanol (C2H6O) with 100.0 gram water to give a final volume of 101 mL.
Calculate the mole fraction for the solute and solvent, and the molality of ethanol in the solution
