Change the following word equation into chemical equation. Write a complete balanced equation for each reaction and state the type of chemical change involved. 1. Heating of mercuric oxide Ans. Mercuric oxide Mercury + Oxygen gas 2H8O 2Hg + 0, (Decomposition) 2. Potassium chlorate Potassium Chloride + Oxygen Gas 3. Rusting of Iron 4. Magnesium + Nitrogen

Change the following word equation into chemical equation. Write a complete balanced equation for each reaction and state the type of chemical change involved. 1. Heating of mercuric oxide Ans. Mercuric oxide Mercury + Oxygen gas 2H8O 2Hg + 0, (Decomposition) 2. Potassium chlorate Potassium Chloride + Oxygen Gas 3. Rusting of Iron 4. Magnesium + Nitrogen

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter7: Reactions In Aqueous Solutions

Section7.3: Describing Reactions In Aqueous Solutions

Problem 7.2SC: trong>Exercise 7.2 For each of the following reactions, write the molecular equation, the complete...

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PRACTICE WRITING CHEMICAL EQUATIONS FROM WORD PROBLEMS AND 1. Phosphorous reacts with oxygen gas to produce diphosphorous 2.When calcium comes in contact with water, calcium hydroxide and hydrogen gas is 3. When hexane (C6H24) reacts with oxygen a combustion reaction occurs. Thisreaction produces carbon dioxide and
Practice Exercise 1Which is the correct net ionic equation for the reaction ofaqueous ammonia with nitric acid?
Practice Exercise 2In the following diagram, the white spheres represent hydrogenatoms, the black spheres carbon atoms, and the redspheres oxygen atoms.In this reaction, there are two reactants, ethylene, C2H4,which is shown, and oxygen, O2, which is not shown, andtwo products, CO2 and H2O, both of which are shown.(a) Write a balanced chemical equation for the reaction.(b) Determine the number of O2 molecules that should beshown in the left (reactants) box.
For the word equation below, write the symbolic (skeletal) equation with the appropriate state symbols. Aqueous sodium hydroxide reacts with carbon dioxide gas to yield an aqueous sodium carbonate solution and liquid water Practice
Balancing equation Practice PdCl2 + HNO3 → Pd(NO3)2 + HCl RbBr + AgCl → AgBr + RbCl PaI5 → Pa + I2 Fe2O3 → Fe + O2 Cu + Cl2 → CuCl2 Na + O2 → Na2O H2 + O2 → H2O Na2SO4 + CaCl2 → CaSO4 + NaCl Al2O3 → Al + O2 C2H6 + O2 → CO2 + H2O
Practice Exercise 1If you complete and balance the following oxidation–reduction reaction in basic solutionNO2-(aq)+ Al(s)---->NH3(aq) + Al(OH)4-(aq) how many hydroxide ions are there in the balanced equation(for the reaction balanced with the smallest whole-numbercoefficients)?(a) One on the reactant side (b) One on the product side(c) Four on the reactant side (d) Seven on the product side(e) None
PRACTICE WRITING CHEMICAL EQUATIONS FROM WORD PROBLEMS AND BALANCING. Ammonium nitrate (NH4NO3) decomposes explosively to form nitrogen, oxygen, and water Dinitrogen tetrahydride (N2H4) reacts with oxygen(O2) to produce nitrogen(N2) and
ercise 9.4 Hydrofluoric acid, an aqueous solution containing dissolved hydrogen fluoride, is used to etch glass by reacting with the silica, SiO2, in the glass to produce gaseous silicon tetra fluoride and liquid water. The unbalanced equation is :math>HF(aq)+SiO2(s)SiF4(g)+H2O(l) l type='a'> Calculate the mass of hydrogen fluoride needed to react with 5.68 g of silica. Hint: Think carefully about this problem. What is the balanced equation for the reaction? What is given? What do you need to calculate? Sketch a map of the problem before you do the calculations. Calculate the mass of water produced in the reaction described in part a.
Limiting Reacting Practice How many grams of silver, Ag, can be formed from 50.8 grams of calcium, Ca, and 1.55 L of 1.51 M silver nitrate solution, AgNO3? (Atomic mass of calcium = 40.08 g/mol, Atomic mass of silver = 107.9 g/mol)
ercise 9.7 Titanium(IV) oxide is a white compound used as a coloring pigment. In fact, the pages in the hooks you read are white because of the presence of this compound in the paper. Solid titanium( IV) oxide can he prepared by reacting gaseous titanium( IV) chloride with oxygen gas. A second product of this reaction is chlorine gas. :math>TiCl4(g)+O2(g)TiO2(s)+Cl2(g) ppose 6.71103g of titanium(IV) chloride is reacted with 2.45103g of oxygen. Calculate the maximum mass of titanium(JV) oxide that can form.If the percent yield of TiO2 is 75%, what mass is actually formed?
Balance the reaction between NO3- and Co to form NO2 and Co2+ in acidic solution. When you have balanced the equation using the smallest integers possible, enter the coefficients of the species shown. NO3- + Co NO2 + Co2+Water appears in the balanced equation as a fill in the blank 5 (reactant, product, neither) with a coefficient of . (Enter 0 for neither.)How many electrons are transferred in this reaction? Submit Answer
Study the chemical equations in the table. Equation Number Balanced Equation 1 2Al(s)+3Cl2(g)⟶2Al3+(aq)+6Cl−(aq)2Al(s)+3Cl2(g)⟶2Al3+(aq)+6Cl−(aq) 2 Cu2+(aq)+H2S(g)⟶CuS(s)+2H+(aq)Cu2+(aq)+H2S(g)⟶CuS(s)+2H+(aq) 3 10H+(aq)+SO2−4(aq)+8I−(aq)⟶4I2(s)+H2S(g)+4H2O(l)10H+(aq)+SO42−(aq)+8I−(aq)⟶4I2(s)+H2S(g)+4H2O(l) Classify each reactant in the chemical equations as an oxidizing agent, a reducing agent, or neither.

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