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Questions and Answers
Consider a reaction where 10.0 g of reactant A (molar mass = 50.0 g/mol) reacts with 15.0 g of reactant B (molar mass = 75.0 g/mol) to produce product C. If the reaction is $A + 2B \rightarrow C$, which reactant is the limiting reagent?
Consider a reaction where 10.0 g of reactant A (molar mass = 50.0 g/mol) reacts with 15.0 g of reactant B (molar mass = 75.0 g/mol) to produce product C. If the reaction is $A + 2B \rightarrow C$, which reactant is the limiting reagent?
- Reactant A is the limiting reagent because it has fewer moles than B relative to the stoichiometric requirement. (correct)
- Reactant B is the limiting reagent because it has more mass, thus there's excess of it.
- Reactant B is the limiting reagent because the stoichiometry requires twice as much B as A.
- Reactant A is the limiting reagent because it has a lower mass.
A student dilutes 50.0 mL of a 2.0 M NaCl solution by adding 150.0 mL of water. The final concentration of the solution is 0.5 M.
A student dilutes 50.0 mL of a 2.0 M NaCl solution by adding 150.0 mL of water. The final concentration of the solution is 0.5 M.
True (A)
Write the balanced net ionic equation for the reaction between aqueous solutions of lead(II) nitrate and potassium iodide.
Write the balanced net ionic equation for the reaction between aqueous solutions of lead(II) nitrate and potassium iodide.
Pb^{2+}(aq) + 2I^-(aq) → PbI_2(s)
In a combustion reaction, a hydrocarbon reacts with ________ to produce carbon dioxide and water.
In a combustion reaction, a hydrocarbon reacts with ________ to produce carbon dioxide and water.
Match the following types of chemical reactions with their descriptions:
Match the following types of chemical reactions with their descriptions:
Which of the following statements best describes the role of intermolecular forces in the dissolution process?
Which of the following statements best describes the role of intermolecular forces in the dissolution process?
According to solubility rules, all nitrate ($NO_3^−$) salts are soluble in water, therefore, mixing a solution of silver nitrate with any other soluble salt will always result in a precipitate.
According to solubility rules, all nitrate ($NO_3^−$) salts are soluble in water, therefore, mixing a solution of silver nitrate with any other soluble salt will always result in a precipitate.
A solution contains 20.0 g of NaCl in 250.0 mL of water. Calculate the molarity of the solution. (Molar mass of NaCl = 58.44 g/mol)
A solution contains 20.0 g of NaCl in 250.0 mL of water. Calculate the molarity of the solution. (Molar mass of NaCl = 58.44 g/mol)
Given the following balanced equation: $2H_2(g) + O_2(g) \rightarrow 2H_2O(g)$. If 4.0 g of $H_2$ reacts with 32.0 g of $O_2$, what mass of $H_2O$ is produced, assuming the reaction goes to completion?
Given the following balanced equation: $2H_2(g) + O_2(g) \rightarrow 2H_2O(g)$. If 4.0 g of $H_2$ reacts with 32.0 g of $O_2$, what mass of $H_2O$ is produced, assuming the reaction goes to completion?
The process by which water molecules surround ions in solution is called ________.
The process by which water molecules surround ions in solution is called ________.
Flashcards
Word Equation
Word Equation
A representation of a chemical reaction using words to indicate reactants and products.
Skeleton Equation
Skeleton Equation
A chemical equation using chemical formulas to indicate the reactants and products without indicating the quantities.
Chemical Equation
Chemical Equation
A representation of a chemical reaction using chemical formulas and coefficients to show the relative quantities of reactants and products.
Physical Change
Physical Change
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Chemical Change
Chemical Change
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Law of Conservation of Mass
Law of Conservation of Mass
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Synthesis Reaction
Synthesis Reaction
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Decomposition Reaction
Decomposition Reaction
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Combustion Reaction
Combustion Reaction
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Limiting Reagent
Limiting Reagent
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Study Notes
- Chemical reactions can be modeled using word equations, skeleton equations, and chemical equations.
- Ball and stick models can also represent chemical reactions, requiring familiarity with nomenclature.
Chemical vs. Physical Changes
- Chemical changes result in the formation of new substances with different properties.
- Physical changes alter the form or appearance of a substance, but not its chemical composition.
Law of Conservation of Mass
- The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction.
- The mass of the reactants equals the mass of the products.
Balancing Chemical Reactions
- Balancing chemical reactions involves adjusting coefficients to ensure the number of atoms of each element is the same on both sides of the equation.
Types of Reactions
- Synthesis reactions involve the combination of two or more reactants to form a single product.
- Decomposition reactions involve the breakdown of a single reactant into two or more products.
- Combustion reactions involve the rapid reaction between a substance with an oxidant, usually oxygen, to produce heat and light.
- Single replacement reactions involve one element replacing another in a compound.
- Double replacement reactions involve the exchange of ions between two compounds to form two new compounds.
Stoichiometry
- Stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction.
- It encompasses all variations of calculations based on mole ratios.
Limiting/Excess Reagents
- The limiting reagent is the reactant that is completely consumed in a reaction.
- The excess reagent is the reactant that remains after the limiting reagent is completely consumed.
Percent Yield
- Percent yield is the ratio of the actual yield to the theoretical yield, multiplied by 100%.
Solutions
- Solutions are homogeneous mixtures.
- Making solutions involves dissolving a solute in a solvent.
Dissolution
- Dissolution is the process of dissolving a solute in a solvent.
Factors Affecting Rate of Solvation
- Factors affecting the rate of solvation include temperature, surface area, and stirring.
Water's Properties
- Water has unique properties such as high surface tension, cohesion, adhesion, and acts as a universal solvent owing to its polarity and ability to form hydrogen bonds.
Concentration and Molarity
- Concentration refers to the amount of solute present in a solution.
- Molarity is defined as the number of moles of solute per liter of solution.
Dilutions
- Dilutions involve reducing the concentration of a solution by adding more solvent.
Solubility
- Solubility is the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature.
- Solubility can be determined using solubility tables and curves.
- Solubility rules provide guidelines for predicting the solubility of ionic compounds in water.
Ionic & Net Ionic Equations
- Ionic equations represent soluble ionic compounds as dissociated ions in solution.
- Net ionic equations show only the species that participate in the reaction, excluding spectator ions.
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