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If 0.4826 g of a mixture of Al(OH)3 and Mg(OH)2 is neutralized with 17.30 mL of 1.000 M HNO3, what is the mass % of Al(OH)3 in the mixture?
A mixture of CaCO3 and CaO weighing 0.693 g was heated to
produce gaseous CO2. After heating, the remaining solid weighed
0.508 g. Assuming all the CaCO3 broke down to CaO and CO2,
calculate the mass percent of CaCO3 in the original mixture.
A sample of a liquid hydrocarbon known to consist of molecules with five carbon atoms is vaporized in a 0.204-L flask by immersion in a water bath at 101 C. The barometric pressure is 767 torr, and the remaining gas weighs 0.469 g. What is the molecular formula of the hydrocarbon?
Typical speeds of the ejected electron are 10 exponents 7 m/s. the mass of an electron is 9.1 times 10 exponent negative 31 kg. what is the kinetic energy of the beta particle in joules
A sample of 30Kg copper absorbs 436000 J of heat, resulting in a temperature rise to 60ºC. What was the initial temperature of the sample if the heat capacity of copper is 0.385 J/gºC.
I want to perform an addition reaction in which I add a single carbon to Diphenylteramide (C24H19N3O). How would I perform this reaction to produce (C25H19N3O)?
3. Given the following reaction: Zn + CuCl2 → ZnCl2 + Cu
a. How many grams of ZnCl2 will be produced from 7.00 g of Zn and 8.00 g of CuCl2?
b. What is the limiting reagent?
c. What is the excess reagent and by how much?
DLP ACTIVITY #4
Direction: Calculate the following word problems involving limiting and excess reagents, theoretical
and percent yield. Show your solution.
1. Silver metal reacts with sulfur to form silver sulfide according to the following reaction:
2Ag+S→Ag2S
a. Identify the limiting reagent if 50.0 g Ag reacts with 10.0 g S.
b. What is the theoretical yield in g of Ag2S produced from the reaction?
c. What is the amount in g of the excess reactant expected to remain after the reaction?
d. When the reaction occurred, the amount of Ag2S obtained was 45.0 g. What is the percent yield
of the reaction?
2. Calculate the mass of magnesium oxide possible if 2.40 g Mg reacts with 10.0 g O2.
Mg+O2 →MgO
a. What is the limiting reagent?
b. What is the theoretical yield?
c. What is the excess reagent and by how much?
3. Given the following reaction: Zn + CuCl2 → ZnCl2 + Cu
a. How many grams of ZnCl2 will be produced from 7.00 g of Zn and 8.00 g of CuCl2?
b. What is the limiting reagent?
If 1 mole = 6.022 x 1023 particles and 1 mole= molar mass, then how many particles are in 2.016 grams of Hydrogen?
Titanium is a transition metal used in many alloys because it is extremely strong and lightweight. Titanium tetrachloride (TiCl4) is extracted from titanium oxide (TiO2) using chlorine and carbon:TiO2(s) + C(s) + Cl2(g) → TiCl4(s) + CO2(g)1.1Calculate the mass of Cl2 gas needed to react with 1.25 moles of TiO2.(4)1.2Say 2.45 grams of TiO2 reacted with 3.25 grams of chlorine gas. During this reaction 4.35 grams of TiCl4was produced. Identify and quantify the limiting reagent. (5)1.3Calculate the amount of excess reagent remaining on completion of the reaction
