Nitric Oxide can be made from the oxidation of ammonia as shown below. A reaction between 8.5 g of NH3 and 25.0 g of O₂ produces 12.0 g of NO. What is the percent yield for this reaction? 4 NH₂(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g) Molar masses (in g mol ¹): NH3 17.034, 0₂ 32.00, NO 30.01, H₂O 18.016

Nitric Oxide can be made from the oxidation of ammonia as shown below. A reaction between 8.5 g of NH3 and 25.0 g of O₂ produces 12.0 g of NO. What is the percent yield for this reaction? 4 NH₂(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g) Molar masses (in g mol ¹): NH3 17.034, 0₂ 32.00, NO 30.01, H₂O 18.016

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...

See similar textbooks

Similar questions

If 18.2 kg NH3 is produced by a reaction mixture that initially contains 6.00 kg H2 and an excess of N2, what is the percent yield of the reaction? N2(g) + 3H2(g) → 2NH3(g)
For the following reaction, 17.1 grams of iron are allowed to react with 36.2 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? grams What is the FORMULA for the limiting reagent? What mass of the excess reagent remains after the reaction is complete? grams
For the following reaction, 16.7 grams of chlorine gas are allowed to react with 8.90 grams of water.3 Cl2(g) + 3 H2O(l) 5 HCl(aq) + HClO3(aq) What is the FORMULA for the limiting reagent? What is the maximum mass of hydrochloric acid that can be formed? gramsWhat mass of the excess reagent remains after the reaction is complete? grams
Consider the following balanced equation for the combustion of butane, a fuel often used in lighters.2 C4H10(g) + 13 O2(g) → 8 CO2(g) + 10 H2O(g)Complete the following table, showing the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that is formed. Mass C4H10 Mass O2 Mass CO2 Mass H2O _____ 2.11 g _____ _____ 5.32 g _____ _____ _____ _____ _____ 13.12 g _____ _____ _____ _____ 8.44 g 252 mg _____ _____ _____ _____ _____ 198 mg _____
Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s)+3Cl2(g)→2AlCl3(s) What is the maximum mass of aluminum chloride that can be formed when reacting 23.0 g of aluminum with 28.0 g of chlorine?
In the reaction Cl2 (g) + I2 (s) --> 2 ICI (g) 22.1 grams of chlorine are reacted in the presence of an excess of iodine. 39 grams of iodine chloride are obtained. Determine the percent yield.
The simple reaction A(s) + 2B(s) → 3C(s) has a theoretical yield of 17.2 g C. What is the percent yield when 12.72 g of C are isolated?
What is the theoretical yield of magnesium oxide when 0.3487 grams of magnesium is mixed with 0.2310 grams of oxygen to produce magnesium oxide? Do not type units into your answer. 2Mg(s) + O2(g) → 2MgO(s)
In the following reaction, which element is the limiting reactant? 2Fe(s) 3Cl2(g) → 2FeCl3(s) iron chlorine neither both Cannot be determined without the original starting mass of both reactants.
For the following reaction, 18.1 grams of iron are allowed to react with 28.0 grams of hydrochloric acid. iron (s) + hydrochloric acid (aq) →iron(II) chloride (aq) + hydrogen (g) What is the maximum amount of iron(II) chloride that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams Submit Answer Try Another Version 2 item attempts remaining ot pt pt pt 1 pt 1 pt Previous
If 25.0 g of NH₃ and 50.1 g of O₂ react in the following reaction, what is the mass in grams of NO that will be formed? 4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g)
Balance the following reaction and predict the amounts of excess (XS) reactant used and products, in grams, assuming the NH3 is the limiting reactant. NH3 (g) + O2 (g) → NO (g) + H2O (l) 16.00 g XS ? ?