Ch.13 - Chemical KineticsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Which combination of factors will affect the rate of the following reaction?Zn(s)  +  2HCl (aq)  →  ZnCl2(aq)  + H2(g)A. Temperature and surfaces onlyB. Temperature and concentration onlyC. Concentration and surface area onlyD. Temperature, concentration, and surface area

Solution: Which combination of factors will affect the rate of the following reaction?Zn(s)  +  2HCl (aq)  →  ZnCl2(aq)  + H2(g)A. Temperature and surfaces onlyB. Temperature and concentration onlyC. Concentrat

Problem

Which combination of factors will affect the rate of the following reaction?

Zn(s)  +  2HCl (aq)  →  ZnCl2(aq)  + H2(g)

A. Temperature and surfaces only

B. Temperature and concentration only

C. Concentration and surface area only

D. Temperature, concentration, and surface area

Solution

We’re asked to determine which of the given factors affect the rate of the given chemical reaction.


Reaction rates are influenced by 4 factors:

1. Concentration: for a reaction to occur, molecules must collide.

Increasing the number of molecules in a container increases their collisions and thereby causes the rate to increase.

2. Surface area: the greater the surface area, the greater the chance for the reaction to occur and the faster the reaction can occur.

The surface area depends on the geometry or structure of the compound.

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