A. What mass in grams of potassium chloride is expected to be produced if 30.6 g of potassium chlorate decomposes? Show your work. = 3. The chemical equation for the decomposition of potassium chlorate is 2 KClO3(s) → 2 KCI(s) + 302(g) The molar masses of the elements in this equation are: K 39.1 g/mol, CI 35.4 g/mol, O 16.0 g/mol

A. What mass in grams of potassium chloride is expected to be produced if 30.6 g of potassium chlorate decomposes? Show your work. = 3. The chemical equation for the decomposition of potassium chlorate is 2 KClO3(s) → 2 KCI(s) + 302(g) The molar masses of the elements in this equation are: K 39.1 g/mol, CI 35.4 g/mol, O 16.0 g/mol

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 10QRT: For this reaction, fill in the table with the indicated quantities for the balanced equation. 4...

See similar textbooks

Similar questions

4.8 In an experiment carried out at very low pressure, 13x1015 molecules of H2 are reacted with acetylene, C2H2, to form ethane, C2H6, on the surface of a catalyst. Write a balanced chemical equation for this reaction. How many molecules of acetylene are consumed?
(a) Butane gas, C4H10, can burn completely in air [use O2(g) as the other reactant] to give carbon dioxide gas and water vapor. Write a balanced equation for this combustion reaction. (b) Write a balanced chemical equation for the complete combustion of C3H7BO3, a gasoline additive. The products of combustion are CO2(g), H2O(g), and B2O3(s).
Disulfur dichloride, S2Cl2, is used to vulcanize rubber. It can be made by treating molten sulfur with gaseous chlorine. S8() + 4 Cl2(g) 4 S2Cl2(g) Complete this table of reaction quantities for the production of 103.5 g S2Cl2.
The final step in the manufacture of platinum metal (for use in automotive catalytic converters and other products) is the reaction 3 (NH4)2PtCl6(s) 3 Pt(s) + 2 NH4Cl(s) + 2 N2(g) + 16 HCl(g) Complete this table of reaction quantities for the reaction of 12.35 g (NH4)2PtCl6.
4.107 Existing stockpiles of the refrigerant Freon-12, CF2Cl2 must be destroyed under the terms of the Montreal Protocol because of their potential for banning the ozone layer. One method for doing this involves reaction with sodium oxalate: CF 2 Cl 2 + 2Na 2 C 2 O 4 2NaF+2NaCl+C+ 4CO 2 S If you had 150 tons of Freon-12, describe how you would know how much sodium oxalate you would need to make that conversion. Freon-12, CF2Cl2
list at least three quantities that must be conserved in chemical reactions.
3.88 One Step in the enrichment of uranium for use in nuclear power plants involves the reaction of UO2 with hydro- fluoric acid (HF) solution. The products are solid UF4 and water. Write a balanced chemical equation for this reaction.
In a common experiment in the general chemistry laboratory, magnesium metal is heated in air to produce MgO. MgO is a white solid, but in these experiments it often looks gray, due to small amounts of Mg3N2, a compound formed as some of the magnesium reacts with nitrogen. Write a balanced equation for each reaction.
Acetone, (CH3)2CO, is an important industrial compound. Although its toxicity is relatively low, workers using it must be careful to avoid flames and sparks because this compound burns readily in air. Write the balanced equation for the combustion of acetone.
4.106 An ore sample with a mass of 670 kg contains 27.7% magnesium carbonate, MgCO3. If all of the magnesium carbonate in this ore sample is decomposed to form carbon dioxide, describe how to determine what mass of CO2 is evolved during the process.
Nitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g)+5O24NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) What mass of NH3 must be used to produce 1.0 106 kg HNO3 by the Ostwald process? Assume 100% yield in each reaction, and assume that the NO produced in the third step is not recycled.
4.28 One of the steps in the manufacture of nitric acid is the oxidation of ammonia shown in this equation: 4NH3(g)+5O2(g)4NO(g)+6H2O(g) If 43.0 kg of NH3 reacts with 35.4 kg of O2, what mass of NO forms?