The reaction between potassium chlorate and red phosphorus takes placewhen you strike a match on a matchbox. If you were to react 30.9 g ofpotassium chlorate (KClO3) with excess red phosphorus, what mass oftetraphosphorus decaoxide (P4O10) could be produced?Mass =KClO3(s) + P4(s) → P4O10 (s) + KCl(s) (unbalanced)g

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Answered: The reaction between potassium chlorate…

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...

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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 59.7 g of each reactant? 4 NH, (g) + 50,(g)4 NO(g) + 6 H,O(g) g H,O mass:
Ammonia gas can be prepared by the reaction of a metal oxide such as calcium oxide with ammonium chloride. CaO (aq) + 2 NH4CI (s) -> 2 NH3 (g) + H2O (g) + CaCl2 (s) If 58.098 g of calcium oxide and 268 g ammonium chloride are mixed, what mass of NH3 (in grams) can be produced?
Look at the balanced chemical equation for the reaction between copper and nitric acid: Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2H2O(l) + 2NO2 (g) How many grams of nitrogen dioxide would be produced if 2.47 g of copper were reacted with excess of nitric acid?
The equation for one of the reactions in the process of turning iron ore into the metal is Fe2O3(s)+3 CO(g) --> 2 Fe(s) +3 CO2(g) If you start with 2.00 kg of each reactant, what is the maximum mass of iron you can produce?
Sodium hypochlorite is the active ingredient in most household bleach products. One method of preparing this compound is as follows: Cl2(g) + 2N2OH(aq) → NaOCI (aq) + NaCl(aq) + H2O(1) In a certain experiment, 50.0 g chlorine was reacted with 50.0 g sodium hydroxide to yield 37.8 g sodium hypochlorite. (a) Calculate the theoretical yield (b) Calculate the percent yield.
For the following reaction, 18.2 grams of iron are allowed to react with 37.9 grams of chlorine gas. iron(s) + chlorine(g) → iron(III) chloride(s) What is the maximum mass of iron(III) chloride that can be formed? Mass= g What is the FORMULA for the limiting reactant? What mass of the excess reagent remains after the reaction is complete? Mass= g
The balanced chemical equation is P₄(s) + 6 Cl₂(g) → 4 PCl₃(g). What is the mass in grams of phosphorus trichloride that can be formed from 226.0 grams of chlorine gas based on the balanced chemical equation?
According to the following reaction, how many grams of mercury will be formed upon the complete reaction of 31.3 grams of mercury(II) oxide? 2HgO(s) → 2Hg(l) + O₂(g) ||| g mercury
If 5.9 × 10²⁵ molecules of CO₂ are produced in a combustion reaction, what is the mass in kg of CO₂ that is produced?
If 6.3 × 10²⁵ molecules of CO₂ are produced in a combustion reaction, what is the mass in kg of CO₂ that is produced?
A 50.6 grams sample of magnesium hydroxide (Mg(OH)2) is reacted with 45.0 grams of hydrochloric acid (HCl). What is the theoretical yield of magnesium chloride (MgCl2)?
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

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