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Stoichiometry

Electrochemistry

3. Nickel is electrolytically refined at 40°C using an electrolyte containing 50 g/liter of nickel ion. The anodes contain copper impurities (< 2 wt.%) which may go into solution as the nickel anode dissolves. Calculate the concentration of Cu2+ ions in solution that is sufficient to result in the depos

Simple explanation needed

10kg petrol is burned in a car engine. What two main chemicals come from the exhaust and how much of each in kilograms?

For the reaction CL2 + 2KBr yields 2KCL + Br2

For the reaction CL2 + 2KBr yields 2KCL + Br2, how many grams of potassium chloride can be produced from 300 g each of chlorine and potassium bromide? 98.7 g, or 188 g or 111g, or 451g.

Theoretical Yield

150.0 g of AsF3 was combined w/ 180.0g CCl4 to yield AsCl3 & CCl2F2. The theoretical yield CCl2F2 produced in moles should be: 1.705, .7802, 1.274, .5685, 1.170?

Density: Mass and Volume

A sphere made of nickel (d=8.908g/cm^3) has a diameter of 8.20 cm. What mass of nickel was used in making the sphere? (V of sphere = 4/3 pi r^3).

Empirical Formula

How to start from from grams to determine % to then calculate the empirical formula. As and O combine 1.626g sample of a compound has 1.232g of As

Given % yield, calculate grams obtained

Balance the following equation: AsF3 + CCl4 ---> AsCl3 + CCl2F2 the theoretical yield of CCl2F2 = 1.68 moles if the actual yield was 74.3% in the reaction, how many grams of CCl2F2 were obtained

Precipitate from Reactions

Silver nitrate reacts with iron(III)chloride Fe Cl3 to give AgCl and Iron(III)nitrate Fe(NO3)3. A solution with 18 grams of AgNO3 was mixed with a solution. 32.4 grams of FeCl3. How many grams of which reactant remains after reaction?

Calc molecules, given mass

I'm thoroughly confusing myself, I know how to calc a formula mass and to determine from moles how to get the mass. But I'm not making the connection to count #atoms/molecule. ex) What are the number of atoms of C-12 are there in 3.5 gram sample

Moles and Molarity Pproblems

A 12.0% sucrose solution has a density of 1.05g/cm^3. The number that gives the best value for the mass of sugar in 55mL of this solution is? I need step by step answer for this question please. What is the Molarity(m) of a solution that contains 73.5g of 1,4-dichlorobenzene,C6H4Cl2, in 500mL of carbon tetrachloride? (The

Molarity of NaCl solution

How much 0.54M NaCl, "physiologic saline" can be prepared via the dilution of 100mL of 6.0 M NaCl solution?

Chemistry calculations including calculating molecular formulas

What is the molecular formula of a compound that contains 42.87% carbon, 3,598% hydrogen, 25.00% nitrogen and 28.55 oxygen and has a molar mass between 165 and 170? How many grams of lithium contain the same number of atoms as 2.50 Kg of zirconium? If the molar mass of a binary compound has a molar mass between 27 and 28 a

One process for the commercial production of baking soda, sodium hydrogen carbonate, involves the following reaction: aqueous sodium chloride + gaseous ammonia + solid carbon dioxide + liquid water yields aqueous ammonium chloride + solid

1. One process for the commercial production of baking soda, sodium hydrogen carbonate, involves the following reaction: aqueous sodium chloride + gaseous ammonia + solid carbon dioxide + liquid water yields aqueous ammonium chloride + solid sodium hydrogen carbonate. Because they are relatively cheap, sodium chloride and water

A hypothetical compound has a formula of X2YZ3.

A hypothetical compound has a formula of X2YZ3. If the atomic masses of X, Y, and Z are 41.2, 57.7 and 63.9 respectively, calculate the % by mass of the compound. If the molecular formula is actually X6Y3Z9, what is the percentage of each element present?

Stoichiometry and Heating Zinc Sulfide

Heating zinc sulfide in the presence of oxygen yields the following: ZnS + O2 (arrow) ZnO + SO2 If 1.72 mol of ZnS is heated in the presence of 3.04 mol of O2, which reactant will be used up? Balance the equation first.

Concentration of Stock Solution

Please explain how I would figure out this problem: From 0.80 L of a glucose stock solution, 4.0L of a 1.8% w/v solution of glucose was prepared. What was the concentration of the stock solution?