Chapter 7: Chemical Reactions

Properties, characteristics and changes of substances are the central topics of—

Transformation of a substance to a different state without changing its chemical structure is called—

Formation of a new substance with new set of properties is called—

Ice melting to water is an example of—

The molecular formula of ice, water and water vapor is the same and equal to—

Liquid water turns into vapor on heating to—

Burning of methane gas in oxygen is a—

In a chemical change, the bond between atoms—

The products of complete combustion of methane in oxygen are—

$\mathrm{CaCO_3} + 2\mathrm{HCl} \to \mathrm{CaCl_2} + \mathrm{CO_2} + ?$ The missing product is—

In an irreversible reaction—

The arrow sign used in irreversible reaction equations is—

The sign used in reversible reaction equations is—

$\mathrm{CaCO_3} \xrightarrow{\Delta} \mathrm{CaO} + \mathrm{CO_2}$ in an open container is—

In a reversible reaction, the conversion of products back to reactants is called—

Ethanol + ethanoic acid → ethyl ethanoate ester + water uses which catalyst?

$\mathrm{H_2 + I_2 \rightleftharpoons 2HI}$ is an example of—

According to the text, in reality—

In a reversible reaction at any time, the two reactions—

Some reactions appear irreversible because—

A reaction that produces heat is called—

A reaction that absorbs heat is called—

In Haber process, $\mathrm{N_2 + 3H_2 \to 2NH_3}$ produces heat equal to—

The catalyst used in the Haber process is—

The pressure used in the Haber process is—

The temperature range in the Haber process is—

For an exothermic reaction, the value of ΔH is—

For an endothermic reaction, the value of ΔH is—

The reaction $\mathrm{N_2 + O_2 \to 2NO}$ absorbs—

The heat change associated with a chemical reaction is denoted by—

The term "redox" is the combination of—

In a redox reaction, electrons are transferred from—

The substance that donates electrons in a redox reaction is called—

The substance that accepts electrons in a redox reaction is called—

In $\mathrm{Na + Cl \to NaCl}$, sodium acts as—

In $\mathrm{Na + Cl \to NaCl}$, chlorine acts as—

$\mathrm{Fe^{2+} \to Fe^{3+} + e^-}$ is a—

$\mathrm{Cu^{2+} + e^- \to Cu}$ is a—

The oxidation number of free Na metal is—

The oxidation number of H in metal hydride such as $\mathrm{LiH}$ or $\mathrm{LiAlH_4}$ is—

The oxidation number of O in peroxide $\mathrm{H_2O_2}$ is—

The oxidation number of O in superoxide $\mathrm{KO_2}$ is—

The oxidation number of alkali metals (e.g., K) in compounds is—

The oxidation number of alkaline earth metals (e.g., Ca, Mg) in compounds is—

The oxidation number of halogen in metal halide (e.g., Cl in $\mathrm{MgCl_2}$) is—

The total of oxidation numbers of all atoms in a neutral compound is—

The total of oxidation numbers of all atoms in an ion equals—

The oxidation number of Mn in $\mathrm{KMnO_4}$ is—

The oxidation number of S in $\mathrm{H_2SO_4}$ is—

The oxidation number of Cr in $\mathrm{K_2Cr_2O_7}$ is—

The oxidation number of Cu in $\mathrm{CuSO_4}$ is—

The oxidation number of N in $\mathrm{HNO_3}$ is—

The oxidation number of P in $\mathrm{H_3PO_4}$ is—

The oxidation number of N in $\mathrm{NH_4^+}$ is—

The oxidation number of S in $\mathrm{SO_4^{2-}}$ is—

The oxidation number of an atom in a homonuclear molecule like $\mathrm{H_2, O_2, N_2, Cl_2}$ is—

Oxidation number and valency are—

The valency of an inert gas is—

The reaction $\mathrm{2FeCl_2 + Cl_2 \to 2FeCl_3}$ is an example of—

$\mathrm{N_2 + 3H_2 \to 2NH_3}$ is an addition reaction that is also called—

A reaction in which a compound breaks into one or more elements or molecules is called—

Heating $\mathrm{PCl_5}$ gives $\mathrm{PCl_3 + Cl_2}$ — this reaction is—

Electrolysis of water $\mathrm{2H_2O \to 2H_2 + O_2}$ is a—

In electrolysis of water, hydrogen gas is produced at the—

In electrolysis of water, oxygen gas is produced at the—

$\mathrm{Zn + H_2SO_4 \to ZnSO_4 + H_2}$ is an example of—

In a substitution reaction, an element or radical—

In $\mathrm{Zn + H_2SO_4 \to ZnSO_4 + H_2}$, zinc displaces—

Combustion of any compound or element in atmospheric oxygen produces—

Combustion $\mathrm{CH_4 + 2O_2 \to CO_2 + 2H_2O}$ is best classified as a—

When sulfur burns in oxygen, the product is—

Burning of carbon in oxygen produces—

Combustion of magnesium in oxygen gives—

Combustion of hydrogen in oxygen produces—

In every combustion reaction, the role of oxygen is to—

In non-redox reactions, there is—

An acid + base → salt + water reaction is called—

$\mathrm{NaOH + HCl \to NaCl + H_2O}$ is a—

The neutralization heat for a strong-acid–strong-base reaction is—

In the actual ionic form of strong-acid/strong-base neutralization, the spectator ions are—

The actual product-forming step in any neutralization is—

When two soluble compounds react and the new product is insoluble in the solvent, the reaction is called—

In $\mathrm{NaCl + AgNO_3 \to AgCl{\downarrow} + NaNO_3}$, the precipitate is—

In $\mathrm{Na_2SO_4 + BaCl_2 \to BaSO_4{\downarrow} + 2NaCl}$, the precipitate is—

$\mathrm{FeSO_4 + 2NaOH \to Fe(OH)_2{\downarrow} + Na_2SO_4}$ — the colour of the precipitate is—

A reaction in which water reacts with another compound to produce new compounds is called—

$\mathrm{AlCl_3(s) + 3H_2O(l) \to Al(OH)_3(s) + 3HCl(aq)}$ is both a hydrolysis and a—

Reaction of $\mathrm{SiCl_4}$ with $\mathrm{H_2O}$ is an example of—

The combination of water molecules with ionic compounds during crystal lattice formation is called—

$\mathrm{CuSO_4 \cdot 5H_2O}$ is called—

$\mathrm{ZnSO_4 \cdot 7H_2O}$ is called—

$\mathrm{CaCl_2 \cdot 6H_2O}$ is called—

Compounds with the same molecular formula but different properties are called—

Heat applied to ammonium cyanate ($\mathrm{NH_4CNO}$) gives—

The chemical reaction in which atoms in a molecule rearrange themselves to form one isomer from another is called—

A reaction in which numerous small molecules combine to form a large molecule of heavy atomic mass at high T and P is called—

In the polymerization of ethylene to polythene, the catalyst used is—

The pressure required for ethylene polymerization is—

The temperature required for ethylene polymerization is—

In a polymerization reaction, the small repeating unit is called—

The difference between hydration and addition reactions is that—

The chemical formula of rust is—

The reactants involved in rusting of iron are—

The intermediate compound formed during rusting before becoming rust is—

In the formula $\mathrm{Fe_2O_3 \cdot nH_2O}$ for rust, the value of n is—

The protective layer formed on copper exposed to air is—

The protective layer formed on aluminum exposed to air is—

The acid carried by an ant or bee that causes pain at the bite spot is neutralized by—

To neutralize excess HCl in the stomach, antacid medicine usually contains—

$\mathrm{2HCl + Mg(OH)_2 \to MgCl_2 + ?}$ — the missing product is—

The major component of natural gas is—

Methane combustion $\mathrm{CH_4 + 2O_2 \to CO_2 + 2H_2O + Energy}$ is mainly used as—

Glucose oxidation in cellular respiration produces—

Painting iron prevents rust because—

Coating zinc on iron to prevent rust is called—

Coating tin on iron is called—

The general process of coating one metal on another metal by electrolysis is called—

Sand spread on a slippery wet roof neutralizes the alkaline substance because $\mathrm{SiO_2}$ is—

Sewing needles are kept in coconut oil to prevent—

Combustion of CNG, diesel, petrol, kerosene and octane all mainly produce—

The rate of a reaction is defined as—

The reaction $\mathrm{AgNO_3 + NaCl \to AgCl + NaNO_3}$ takes about—

Rusting of an iron bridge takes—

The faster a reaction proceeds, the rate of reaction is—

In the experiment with sodium carbonate, gas comes out from a tube only when—

Adding hot water to $\mathrm{Na_2CO_3}$ + acid produces gas—

The state in a reversible reaction where forward and backward rates are equal is called—

At equilibrium, concentrations of reactants and products—

According to Le Chatelier's principle, when an external change is applied to a system at equilibrium, the system shifts to—

For $\mathrm{N_2 + 3H_2 \rightleftharpoons 2NH_3}$ (forward exothermic), increasing temperature—

For $\mathrm{N_2 + 3H_2 \rightleftharpoons 2NH_3}$, decreasing temperature—

For $\mathrm{N_2 + O_2 \rightleftharpoons 2NO}$ (forward endothermic), increasing temperature—

For $\mathrm{N_2 + 3H_2 \rightleftharpoons 2NH_3}$, increasing pressure shifts equilibrium—

For $\mathrm{N_2 + 3H_2 \rightleftharpoons 2NH_3}$, decreasing pressure shifts equilibrium—

For $\mathrm{N_2 + O_2 \rightleftharpoons 2NO}$, change of pressure—

Increasing the concentration of a reactant in equilibrium shifts the equilibrium—

Increasing the concentration of a product in equilibrium shifts the equilibrium—

At the start of a reversible reaction, the rate of forward reaction is—

At the start of a reversible reaction, the rate of backward reaction is—

At equilibrium, both forward and backward reactions—