For the following reaction, 10.8 grams of ammonia are allowed to react with 15.8 grams of oxygen gas. ammonia (g) + oxygen (g) → nitrogen monoxide (g) + water (g) What is the maximum amount of nitrogen monoxide 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

For the following reaction, 10.8 grams of ammonia are allowed to react with 15.8 grams of oxygen gas. ammonia (g) + oxygen (g) → nitrogen monoxide (g) + water (g) What is the maximum amount of nitrogen monoxide 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

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter6: Chemical Calculations: Formula Masses, Moles, And Chemical Equations

Section: Chapter Questions

Problem 6.66EP: For the chemical reaction C3H8O2+4O23CO2+4H2O how many product molecules are formed when nine C3H8O2...

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For the chemical reaction C3H8O2+4O23CO2+4H2O how many product molecules are formed when nine C3H8O2 molecules react?
4.8 In an experiment carried out at very low pressure, 13x1015 molecules of H2 are reacted with acetylene, C2H2, to form ethane, C2H6, on the surface of a catalyst. Write a balanced chemical equation for this reaction. How many molecules of acetylene are consumed?
Calculate the amounts of reactants needed in a chemical reaction to produce a specified amount of product.
You know that chemical A reacts with chemical B. You react 10.0 g A with 10.0 g B. What information do you need to determine the amount of product that will be produced? Explain.
Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A tiny portion of the starting mixture is represented by the diagram, where the blue circles represent N and the white circles represent H. Which of these represents the product mixture? For the reaction of the given sample, which of these statements is true? (a) N2 is the limiting reactant. (b) H2 is the limiting reactant. (c) NH, is the limiting reactant. (d) No reactant is limiting: they are present in the correct stoichiometric ratio.
Consider the following unbalanced chemical equation for the combustion of pentane (C5H12): C5H12(l)+O2(g)CO2(g)+H2O(l) If 20.4 g of pentane are burned in excess oxygen, what mass of water can be produced, assuming 100% yield?
Consider a reaction represented by the following balanced equation :math>2A+3BC+4D u find that it requires equal masses of A and B so that there are no reactants left over. Which of the following is true? Justify your choice. l type='a'> The molar mass of A must be greater than the molar mass of B. i>The molar mass of A must be less than the molar mass of B. i>The molar mass of A must be the same as the molar mass of B.
Consider the following balanced chemical equation: A+5B3C+4D a. Equal masses of A and B are reacted. Complete each of the following with either A is the limiting reactant because ; B is the limiting reactant because ____ ; or we cannot determine the limiting reactant because _____ i. If the molar mass of A is greater than the molar mass of B, then ii. If the molar mass of B is greater than the molar mass of A, then b. The products of the reaction are carbon dioxide (C) and water (D). Compound A has a similar molar mass to carbon dioxide. Compound B is a diatomic molecule. Identify compound B, and support your answer. c. Compound A is a hydrocarbon that is 81.7 1% carbon by mass. Determine its empirical and molecular formulas.
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?
The following quantities are placed in a container: 1.51024 atoms of hydrogen, 1.0 mol of sulfur, and 88.0 g of diatomic oxygen. What is the total mass in grams for the collection of all three elements? What is the total number of moles of atoms for the three elements? If the mixture of the three elements formed a compound with molecules that contain two hydrogen atoms, one sulfur atom, and four oxygen atoms, which substance is consumed first? How many atoms of each remaining element would remain unreacted in the change described in (c)?
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.

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