Direct reaction of iodine (I2) and chlorine (Cl2) produces an iodine chloride, I,Cly, 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 I,Cly, what is the empirical formula of the compound? A later experiment showed that the molar mass of I,Cl, was 467 g.mol. What is the molecular formula of the compound? Antwoorde: / Answers:

Direct reaction of iodine (I2) and chlorine (Cl2) produces an iodine chloride, I,Cly, 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 I,Cly, what is the empirical formula of the compound? A later experiment showed that the molar mass of I,Cl, was 467 g.mol. What is the molecular formula of the compound? Antwoorde: / Answers:

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

A given compound is analyzed and found to contain only C, H and O. When a 35.79 g sample of this compound is completely combusted in the presence of excess oxygen, the reaction yields 49.19 g of carbon dioxide and 13.43 g of water. What is the empirical formula of this compound?
When 5.974 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 18.74 grams of CO2 and 7.675 grams of H2O were produced.In a separate experiment, the molar mass of the compound was found to be 56.11 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.
Chromium(III) oxide can be made from the reaction of sodium dichromate and ammonium chloride. What is the maximum mass, in grams, of chromium(III) oxide that can be produced from the complete reaction of 108.7 g of sodium dichromate, Na2Cr2O7, with 61.6 g of ammonium chloride? The other products are sodium chloride, nitrogen gas, and water.
Copper(II) sulfate forms several hydrates with the general formula CuSO4·xH2O, where x is an integer. If the hydrate is heated, the water can be driven off, leaving pure CuSO4 behind. Suppose a sample of a certain hydrate is heated until all the water is removed, and it's found that the mass of the sample decreases by 31.%. Which hydrate is it? That is, what is x?
The fuel used in many disposable lighters is liquid butane, C4H10. Butane has a molecular weight of 58.1 grams in one mole. How many carbon atoms are in 2.00 g of butane?
P4(s) + 6Cl2(g) → 4PCl3(l) Given an initial mass of 19.14 g P4, an excess of Cl2, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of PCl3 produced by the reaction. g
52.3 g of Zinc metal is reacted with a solution containing 51.0 grams of hydrochloric acid, HCl. The reaction yields zinc chloride, ZnCl2, and hydrogen, H2, gas. At the end of the reaction, what is the mass (in grams) of Zinc that remains? At the end of the reaction, what is the mass (in grams) of much HCl that remains?
Consider the following balanced chemical reaction: N2 (g) + 3 H2 (g) → 2 NH3 (g) What is the maximum mass (in grams) of ammonia (NH3) that can be produced from 9.36 g of N2 and 4.92 g of H2?
Combustion analysis of 2.796 g of an unknown compound containing carbon, hydrogen, and oxygen produced 5.597 g of CO2 and 2.268 g of H2O. What is the empirical formula of the compound?
Calculate the mass in grams of 1.35 x 104 molecules of methanol. The chemical formula for methanol is CH, O. mass:
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H,O that can be produced by combining 81.4 g of each reactant? 4 NH, (g) + 50,(g) 4 NO(g) + 6 H, O(g) > g H,O mass:
For the reaction represented by the equation C12+ 2KBr 2KC1 + Br2, how many grams of potassium chloride (KC1) are produced from 3.75 x 1023 molecules of chlorine gas?