HOWhat is the chemical formula for the limiting reactant in the reaction shown?chemical formula:NOWrite the balanced chemical equation for the reaction, using lowest whole-number coefficients.chemical equation:4NO + SH,4H,O + 2N, + H,Incorrect

Limiting reactant is the reactant which limits the extent of reaction or the reaction proceed…

Answered: N но What is the chemical formula for…

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 4.70PAE: 4.70 The particulate scale drawing shown depicts the products of a reaction between H2 and O2...

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For each of the following unbalanced chemical equations, suppose exactly 5.0 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expected, assuming that the limiting reactant is completely consumed. msp;Na(s)+Br2(l)NaBr(s) msp;Zn(s)+CuSO4(aq)ZnSO4(aq)+Cu(s) msp;NH4Cl(aq)+NaOH(aq)NH3(g)+H2O(l)+NaCl(aq) msp;Fe2O3(s)+CO(g)Fe(s)+CO2(g)
3.81 The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients.
For each of the following unbalanced chemical equations, suppose 25.0 g of each reactant is taken. Show by calculation which reactant is limiting. Calculate the theoretical yield in grams of the product in boldface. msp;C2H5OH(l)+O2(g)CO2(g)+H2O(l) msp;N2(g)+O2(g)NO(g) msp;NaClO2(aq)+Cl2(g)NaCl(aq) msp;H2(g)+N2(g)NH3(g)
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.
4.71 The particulate scale drawing shown depict the products of a reaction between N2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients. (c) Identify the limiting reactant, and explain how the pictures allow you to do so.
Although many sulfate salts are soluble in water, calcium sulfate is not (Table 7. 1). Therefore, a solution of calcium chloride will react with sodium sulfate solution to produce a precipitate of calcium sulfate. The balanced equation is :math>CaCl2(aq)+Na2SO4(aq)CaSO4(s)+2NaCl(aq) a solution containing 5.21 g of calcium chloride is combined with a solution containing 4.95 g of sodium sulfate, which is the limiting reactant? Which reactant is present in excess?
3.75 The following pictures show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (A atoms are shown in blue and B atoms in white). The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reac- tion 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.
In a blast furnace at high temperature, iron(III) oxide in ore reacts with carbon monoxide to produce metallic iron and carbon dioxide. The liquid iron produced is cooled and weighed. The reaction is run repeatedly with the same initial mass of iron(III) oxide, 19.0 g, but differing initial masses of carbon monoxide. The masses of iron obtained arc shown in this graph. (a) Write the balanced chemical equation for this reaction. (b) Calculate the mass of CO required to react completely with 19.0 g iron(III) oxide. (c) Calculate the mass of carbon dioxide produced when the reaction converts 10.0 g iron(III) oxide completely to products. (d) From the graph, determine which reactant is limiting when less than 10.0 g carbon monoxide is available to react with 19.0 g iron(III) oxide. (e) From the graph, determine which reactant is limiting when more than 10.0 g carbon monoxide is available to react with 19.0 g iron(III) oxide. (f) Calculate the percent yield if 24.0 g iron(III) oxide reacted with 20.0 g carbon monoxide to produce 15.9 g metallic iron. (g) Calculate the minimum mass of additional limiting reactant required to react with all of the excess of nonlimiting reactant from part (f).
Classify each of the following statements as true or false: a Coefficients in a chemical equation express the molar proportions among both reactants and products. b A stoichiometry problem can be solved with an unbalanced equation. c In solving a stoichiometry problem, the change from quantity of given substance to quantity of wanted substance is based on masses. d Percentage yield is actual yield expressed as a percentage of ideal yield. e The quantity of product of any reaction can be calculated only through the moles of the limiting reactant. f rH is positive for an endothermic reaction and negative for an exothermic reaction.
The left box of the following diagram shows the hypothetical elements A green atoms and B blue diatomic molecules before they react. Write a balanced chemical equation, using the lowest possible whole-number coefficients, for the reaction that occurs to form the product in the right box.
A possible practical way to eliminate oxides of nitrogen(such as NO2 ) from automobile exhaust gases uses cyanuricacid, C3N3(OH)3 . When heated to the relatively lowtemperature of 625°F, cyanuric acid converts to gaseousisocyanic acid (HNCO). Isocyanic acid reacts with NO2 inthe exhaust to form nitrogen, carbon dioxide, and water,all of which are normal constituents of the air. (a) Write balanced equations for these two reactions. (b) If the process described earlier became practical, howmuch cyanuric acid (in kilograms) would be requiredto absorb the 1.71010kgNO2 generated annuallyin auto exhaust in the United States?
Explain how one determines which reactant in a process is the limiting reactant. Does this depend only on the masses of the reactant present? Give an example of how to determine the limiting reactant by using a Before-Change-After (RCA) table with a balanced chemical equation and reactant starling amounts.

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N но What is the chemical formula for the limiting reactant in the reaction shown? chemical formula: NO Write the balanced chemical equation for the reaction, using lowest whole-number coefficients. chemical equation: 4NO + SH, → 4H,0 + 2N, + H, - Incorrect