Which is not balanced?O C3H8 + 502 → 3CO2 + 4H2OO P4 + 6C2 →4PCI32AI3022A2O3->O K 2CO3 + 2 HNO3 → 2 KNO3 + H2O + CO2O2 AGNO3 + Fe → 2 Ag + Fe(NO3) 2

According to the law of conservation of mass, the quantity of each element does not change in a…

Answered: Which is not balanced? O C3H8 + 502 →…

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 3.11PAE: 3.11 Balance these equations. (a) Al(s) + O2(g)( Al2O3(s) (b) N2(g) + H2(g) (NH3(g) (c) C6H6(l) +...

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Similar questions

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?
How many molecules of the sweetener saccharin can be prepared from 30 C atoms, 25 H atoms, 12 0 atoms, 8 S atoms, and 14 N atoms?
The reaction of methane and water is one way to prepare hydrogen for use as a fuel: CH4(g) + H2O(g) CO(g) + 3 H2(g) If this reaction has a 37% yield under certain conditions, what mass of CH4 is required to produce 15 g of H2?
In a common experiment in the general chemistry laboratory, magnesium metal is heated in air to produce MgO. MgO is a white solid, but in these experiments it often looks gray, due to small amounts of Mg3N2, a compound formed as some of the magnesium reacts with nitrogen. Write a balanced equation for each reaction.
Ammonia can be formed from a combination reaction of its elements. A small fraction of an unreacted mixture of elements is illustrated in the following diagram, in which white spheres represent hydrogen atoms and blue spheres represent nitrogen atoms. The temperature is such that all species are gases. a Write and balance the equation for the reaction. b Which of the following correctly represents the product mixture? c Which species is the limiting reactant? Explain.
3.11 Balance these equations. (a) Al(s) + O2(g)( Al2O3(s) (b) N2(g) + H2(g) (NH3(g) (c) C6H6(l) + O2(g) ( H2O(l) + CO2(g)
3.93 Adipic acid is used in the production of nylon, so it is manufactured in large quantities. The most common method for the preparation of adipic acid is the reaction of cyclohexane with oxygen. Balance the skeleton equation shown be1ow.
Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.
One mol of ammonia reacts with 1.00 mol of oxygen to form nitrogen oxide and water according to the reaction 4NH3(g)+5O2(g)4NO(g)+6H2O(l)State which statements are true about the reaction and make the false statements true. (a) All the oxygen is consumed. (b) 4.00 mol NO are produced. (c) 1.50 mol H2O are produced. (d) The description of the experiment does not provide enough information to determine percent yield. (e) Three moles of water are produced for every two moles of NO obtained.
High cost and limited availability of a reactant often dictate which reactant is limiting in a particular process. Identify the limiting reactant when the reactions below are run, and come up with a reason to support your decision. a. Burning charcoal on a grill: C(s)+O2(g)CO2(g) b. Burning a chunk of Mg in water: Mg(s)+2H2O(l)Mg(OH)2(aq)+H2(g) c. The Haber process of ammonia production: 3H2(g)+N2(g)2NH3(g)
Write an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.
Nitrogen (N2) and hydrogen (H2)react to form ammonia (NH3). Consider the mixture of N2 and H2 in a closed container as illustrated below: Assuming the reaction goes to completion, draw a representation of the product mixture. Explain how you arrived at this representation.

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Which is not balanced? O C3H8 + 502 → 3CO2 + 4H2O O P4 + 6C12 4PCI3 O 2AI + 302 2AI2O3 -> O K 2CO3 + 2 HNO3 → 2 KNO3 + H2O + CO2 O2 AGNO3 + Fe→ 2 Ag + Fe(NO3) 2