4. Sodium hydroxide reacts with carbon dioxide as follows:2 NaOH (s) + CO2 (g) → NażCO3 (s) + H2O (1)Which is the limiting reactant when 1.85 mol NaOH and 1.00 mol CO2 are allowed toreact? How many moles of Na2CO3 can be produced? How many moles of the excessreactant remain after the completion of the reaction? Direction: Analyzed and solve each problem given on each item. Write your calculation on aseparate sheet of paper.Note: In calculation involving atomic mass, use 4 significant figure for the atomic mass of eachelement needed in the calculation. Use scientific notation, if necessary.

Consider the given balanced equation is as follows; 2 NaOH s + CO2g → Na2CO3s + H2Ol…

Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH (s) + CO2 (g) → Na2CO3 (s) + H2O () Which is the limiting reactant when 1.85 mol NaOH and 1.00 mol CO2 are allowed to react? How many moles of Na2CO3 can be produced? How many moles of the excess reactant remain after the completion of the reaction?

Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH (s) + CO2 (g) → Na2CO3 (s) + H2O () Which is the limiting reactant when 1.85 mol NaOH and 1.00 mol CO2 are allowed to react? How many moles of Na2CO3 can be produced? How many moles of the excess reactant remain after the completion of the reaction?

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

Section3.7: Limiting Reactants

Problem 3.18E: Urea is used as a fertilizer because it can react with water to release ammonia, which provides...

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Urea is used as a fertilizer because it can react with water to release ammonia, which provides nitrogen to plants. (NH2)2CO(s) + H2O() 2 NH3(aq) + CO2(g) (a) When 300. g urea and 100. g water are combined, calculate the mass of ammonia and the mass of carbon dioxide that form. (b) Calculate the mass of the excess reactant that remains after reaction.
What is meant by a limiting reactant in a particular reaction? In what way is the reaction “limited”? What does it mean to say that one or more of the reactants are present in excess? What happens to a reaction when the limiting reactant is used up?
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The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH 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 reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
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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.
4-93 Ammonia is prepared industrially by the reaction of nitrogen and hydrogen according to the following equation: If 29.7 kg of N2 is added to 3.31 kg of H2, (a) Which reactant is the limiting reagent? (b) How many grams of the other reactant are left over? (c) How many grams of NH3 are formed if the reaction goes to completion?
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4.70 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. (c) identify the limiting reactant, and explain how the pictures allow you to do so.
Ammonia gas can be prepared by the following reaction: CaO(s) + 2 NH4Cl(s) 2 NH3(g) + H2O(g) + CaCl2(s) If 112 g of CaO and 224 g of NH4Cl are mixed, the theoretical yield of NH3 is 68.0 g (Study Question 12). If only 16.3 g of NH3 is actually obtained, what is its percent yield?
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