Gaseous methane (CH4) reacts with gaseous oxygen gas (0₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O) . What is the theoretical yield of water formed from the reaction of 0.96 g of methane and 6.5 g of oxygen gas? Be sure your answer has the correct number of significant digits in it.

Gaseous methane (CH4) reacts with gaseous oxygen gas (0₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O) . What is the theoretical yield of water formed from the reaction of 0.96 g of methane and 6.5 g of oxygen gas? Be sure your answer has the correct number of significant digits in it.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter3: Molecules, Moles, And Chemical Equations

Section: Chapter Questions

Problem 3.115PAE: 3.115 The average person exhales 1.0 kg of carbon dioxide in a day. Describe how you would estimate...

See similar textbooks

Similar questions

Propane, C3H8, is the fuel of choice in a gas barbecue. When burning, the balanced equation is C3H8+5O23CO2+4H2O a What is the limiting reactant in cooking with a gas grill? b If the grill will not light and you know that you have an ample flow of propane to the burner, what is the limiting reactant? c When using a gas grill you can sometimes turn the gas up to the point at which the flame becomes yellow and smokey. In terms of the chemical reaction, what is happening?
4.69 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. 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.
In an experiment designed to produce calcium oxide by the chemical reaction 2Ca + O2 2CaO 177.2 g of CaO was obtained out of a possible 203.9 g ofCaO. a. What is the theoretical yield of CaO? b. What is the actual yield of CaO? c. What is the percent yield of CaO?
For the chemical reaction C3H8O2+4O23CO2+4H2O how many product molecules are formed when nine C3H8O2 molecules react?
The sugar sucrose, which is present in many fruits and vegetables, reacts in the presence of certain yeast enzymes to produce ethanol and carbon dioxide gas. Balance the following equation for this reaction of sucrose. C12H22O11(aq) + H2O(l) C2H5OH(aq) + CO2(g)
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).
The principal constituent of natural gas is methane, which burns in air according to the reaction CH4+2O2CO2+2H2O How many grams of O2 are needed to produce 3.50 g of CO2?
Copper(II) sulfate has been used extensively as a fungicide (kills fungus) and herbicide (kills plants). Copper(II) sulfate can be prepared in the laboratory by reaction of copper(II) oxide with sulfuric acid. The unbalanced equation is :math>CuO(s)+H2SO4(aq)CuSO4(aq)+H2O(l) 2.49 g of copper(II) oxide is treated with 5.05 g of pure sulfuric acid, which reactant would limit the quantity of copper(II) sulfate that could be produced?
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.
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?
Methane (CH4) is the main component of marsh gas. Heating methane in the presence of sulfur produces carbon disulfide and hydrogen sulfide as the only products. a. Write the balanced chemical equation for the reaction of methane and sulfur. b. Calculate the theoretical yield of carbon disulfide when 120. g of methane is reacted with an equal mass of sulfur.
You react nitrogen and hydrogen in a container to produce ammonia, NH3(g). The following figure depicts the contents of the container after the reaction is complete. a Write a balanced chemical equation for the reaction. b What is the limiting reactant? c How many molecules of the limiting reactant would you need to add to the container in order to have a complete reaction (convert all reactants to products)?