Consider the reaction:N2(g) + 202(g) → 2NO2(g)0.250 mol of N2(g) is reacted with 0.300 mol of O2(g).Calculate the amount of excess reagent in molesremains assuming complete reaction. [Hint: lIdentify theexcess reagent first.]Select one:a. 0.150 mol of excess reagent remains.b. 0.200 mol of excess reagent remains.C. 0.050 mol of excess reagent remains.d. 0.100 mol of excess reagent remains.

According to the balanced chemical equation, 1 mole of N2 reacts with 2 moles of O2.

Consider the reaction: N2(g) + 202(g) → 2NO2(g) 0.250 mol of N2(g) is reacted with 0.300 mol of O2(g). Calculate the amount of excess reagent in moles remains assuming complete reaction. [Hint: Identify the excess reagent first.]

Consider the reaction: N2(g) + 202(g) → 2NO2(g) 0.250 mol of N2(g) is reacted with 0.300 mol of O2(g). Calculate the amount of excess reagent in moles remains assuming complete reaction. [Hint: Identify the excess reagent first.]

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 12CR: What is meant by a limiting reactant in a particular reaction? In what way is the reaction...

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On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
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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