A. Magnesium chloride has a formula of MgCl2 · 6H2O. What is its formula weight? B. You desire to make 1 L of 0.1 MgCl2 solu- tion. How much MgCl2 · 6H2O should you weigh? C. You need to make 25 mL of a 25-mM solu- tion of MgCl2. How much of the 0.1 M stock solution do you add to the 25 mL volumetric flask?

A. Magnesium chloride has a formula of MgCl2 · 6H2O. What is its formula weight? B. You desire to make 1 L of 0.1 MgCl2 solu- tion. How much MgCl2 · 6H2O should you weigh? C. You need to make 25 mL of a 25-mM solu- tion of MgCl2. How much of the 0.1 M stock solution do you add to the 25 mL volumetric flask?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.9PAE: 4.9 Sulfur, S8, combines with oxygen at elevated temperatures to form sulfur dioxide. (a) Write a...

See similar textbooks

Similar questions

3.11 Balance the following equations. (a) CaC2(s) + H2O(l)( Ca(OH)2(s) + C2H2(g) (b) (NH4)2CrO7(s) ( Cr2O3(s) + N2(g) + H2O (g) (c) CH3NH2(g) + O2(g) ( CO2(g) + N2(g) + H2O (g)
Consider the balanced chemical equation :math>A+5B3C+4D en equal masses of A and B are reacted, which is limiting, A or B? Justify your choice. If the molar mass of A is greater than the molar mass of B, then A must be limiting. If the molar mass of A is less than the molar mass of B, then A must be limiting. If the molar mass of A is greater than the molar mass of B, then B must be limiting. If the molar mass of A is less than the molar mass of B, then B must be limiting.
Methanol, CH3OH, can be prepared from carbon monoxide and hydrogen. CO(g) + 2 H2(g) CH3OH(l) What mass of hydrogen is required to produce 1.0 L of CH3OH (d = 0.791 g/mL) if this reaction has a 74% yield under certain conditions?
The following pictures show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (A at-oms are shown in blue and B atoms in white). The box on the left represents the box on the right shows what is left once the reaction has gone to completion. Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
4.9 Sulfur, S8, combines with oxygen at elevated temperatures to form sulfur dioxide. (a) Write a balanced chemical equation for this reaction. (b) If 200 oxygen molecules are used up in this reaction, how many sulfur molecules react? (c) How many sulfur dioxide molecules are formed in part (b)?
Aspirin, C6H4 (OCOCH3) CO3H, is produced by the reaction of salicylic acid, C6H4(OH)CO2H, and acetic anhydride, (CH3CO)2O (page 182). C6H4(OH)CO3H(s) + (CH3CO)3O(l) C6H4(OCOCH3)CO2H(s) + CH3CO2H(l) If you mix 100. g of each of the reactants, what is the maximum mass of aspirin that can be obtained
ou know that chemical A reacts with chemical B. You react 10.0 g A with 10.0 g B. What information do you need to know to determine the amount of product that will be produced? Explain.
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. a. What mass of DDT is formed, assuming 100% yield? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is 200.0 g, what is the percent yield?
A weighed sample of iron (Fe) is added to liquid bromine (Br2) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below). (a) What mass of Br2 is used when the reaction consumes 2.0 g of Fe? (b) What is the mole ratio of Br2 to Fe in the reaction? (c) What is the empirical formula of the product? (d) Write the balanced chemical equation tor the reaction of iron and bromine. (e) What is the name of the reaction product? (f) Which statement or statements best describe the experiments summarized by the graph? (i) When 1.00 g of Fe is added to the Br2, Fe is the limiting reagent. (ii) When 3.50 g of Fe is added to the Br2, there is an excess of Br2. (iii) When 2.50 g of Fe is added to the Br2, both reactanu are used up compietely. (iv) When 2.00 g of Fe is added to the Br2, 10.8 g of product is formed. The percent yield must therefore be 20.0%.
Copper(II) sulfate has been used extensively as a fungicide (kills fungus) and herbicide (kills plants). Copper(II) sulfate can be prepared in the laboratory by reaction of copper(II) oxide with sulfuric acid. The unbalanced equation is :math>CuO(s)+H2SO4(aq)CuSO4(aq)+H2O(l) 2.49 g of copper(II) oxide is treated with 5.05 g of pure sulfuric acid, which reactant would limit the quantity of copper(II) sulfate that could be produced?
hat happens to the weight of an iron bar when it rusts? l type='a'> There is no change because mass is always conserved. i>The weight increases. i>The weight increases, hut it the rust is scraped off, the bar has the original weight. i>The weight decreases. stify your choice and, for choices you did not pick, explain what is wrong with them. Explain what it means for something to rust.