A sample of a substance with the empirical formula XCl₂ weighs 0.5984 g. When it is dissolved in water and all its chlorine is converted to insoluble AgCl by addition of an excess of silver nitrate, the mass of the resulting AgCl is found to be 1.2756 g. The chemical reaction is (a) Calculate the formula mass of XCI₂. (b) Calculate the atomic mass of X. XCI2+ 2 AgNO3 Formula mass XCl₂ = Atomic mass X = 2AgCl + X(NO3)₂ g mol-1 g mol-1

A sample of a substance with the empirical formula XCl₂ weighs 0.5984 g. When it is dissolved in water and all its chlorine is converted to insoluble AgCl by addition of an excess of silver nitrate, the mass of the resulting AgCl is found to be 1.2756 g. The chemical reaction is (a) Calculate the formula mass of XCI₂. (b) Calculate the atomic mass of X. XCI2+ 2 AgNO3 Formula mass XCl₂ = Atomic mass X = 2AgCl + X(NO3)₂ g mol-1 g mol-1

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Direct reaction of iodine (I2) and chlorine (Cl2) produces an iodine chloride, IxCly, a bright yellow solid. If you completely consume 0.678 g of I2 in a reaction with excess Cl2 and produce 1.246 g of IxCly, what is the empirical formula of the compound? A later experiment showed that the molar mass of IxCly was 467 g.mol-1. What is the molecular formula of the compound?
A mixture consisting of only copper(II) chloride (CuCl₂) and calcium chloride (CaCl₂) weighs 1.0052 g. When the mixture is dissolved in water and an excess of silver nitrate is added, all the chloride ions associated with the original mixture are precipitated as insoluble silver chloride (AgCl). The mass of the silver chloride is found to be 2.3492 g. Calculate the mass percentages of copper(II) chloride and calcium chloride in the original mixture. Mass percent CuCl₂ Mass percent CaCl₂ = % %
A compound containing only carbon, hydrogen, and oxygen is subjected to elemental analysis. Upon complete combustion, a 0.7916 g sample of the compound produced 1.581 g of CO2 and 0.6474 g of H2O. What is the empirical formula of the compound ?
3) If 25.5 mL of a 0.123 M solution of iodide was added to 22.3 mL of a 0.209 M solution of iodate ions (IO3) in the presence of acid, I3 ions form. What is the resulting molarity of IO3 ions after the two solutions are added and allowed to react completely?
B. Write the net ionic equation for the formation of each of the following insoluble compounds in aqueous solution: (a) lead(II) chromate, PbCrO4, the yellow pigment that has been used for centuries in oil paints; (b) aluminum phosphate, AlPO4, used in cements and as an antacid; (c) iron(II) hydroxide, Fe(OH)2. (d) Select two soluble ionic compounds that, when mixed in solution, form each of the insoluble compounds in parts (a), (b), and (c). Identify the spectator ions.
What is the mass in grams of magnesium chloride that can be produced from 9.10 moles of chlorine gas reacting with excess magnesium? Mg(s) + Cl₂(g) → MgCI₂(s)
A sample of gallium bromide, GaBr3, weighing 0.165 g was dissolved in water and treated with silver nitrate, AgNO3, resulting in the precipitation of 0.299 g AgBr. Use these data to compute the %Ga (by mass) GaBr3.
Thallium(I) sulfate is an active ingredient in rat poison. We can analyze a sample for the mass percentage for this active ingredient by adding potassium iodide to precipitate yellow thallium(I) iodide. If the sample of rat poison weighed 999.5 mg and you obtained 279.4 mg of the dry precipitate, then what is the mass percentage of the thallium(I) sulfate in the rat poison?
A 3.859 g sample containing impure CuCl2· 2 H20 was heated to constant mass. The sample mass after heating to drive off the water was 3.161 g. What was the mass percent of CuCl2· 2 H2O in the original sample?
Which of the following reactions can be described as an atom combination reaction?(a) Ca(g) + S(g) + 4 O(g) → CaSO4(s)(b) C(graphite) + 2 H2(g) → CH4(g)(c) C3H8(g) + 5O2(g) → 3 CO2(g) + 4 H2O(g)(d) C6H6(g) → 6 C(g) + 3 H2(g)(e) K(s) + Mn(s) + 2 O2(g) → KMnO4(s
Urea, [NH2)2CO] is prepared by reacting ammonia with carbon dioxide. In one process, 637.2 g of NH3 are treated with 1142 g of CO2. Which of the reactant is limiting reagent? Calculate the mass of (NH2)2CO How much excess reagent (in grams) is left at the end of the reaction?
A mixture consisting of only chromium(III) bromide (CrBr3) and aluminum bromide (AlBr3) weighs 1.1218 g. When the mixture is dissolved in water and an excess of silver nitrate is added, all the bromide ions associated with the original mixture are precipitated as insoluble silver bromide (AgBr). The mass of the silver bromide is found to be 2.2708 g. Calculate the mass percentages of chromium(III) bromide and aluminum bromide in the original mixture. Mass percent CrBr3 Mass percent AlBr3 = % %