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XI Chem New Chap 6 Equilibirum 400 Profound True or False Statements
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XI Chem New Chap 6 Equilibirum 400 Profound True or False Statements
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XI_Chem_New Chap-6_Equilibrium_[True or False Statement Questions]Sl #Statements [6.1 Introduction] TRUE/FALSE
Chemical equilibria are in biological and environmental processes, such as O2 transport by
1 TRUE
hemoglobin in our bodies and CO toxicity due to its equilibrium with hemoglobin.
Equilibrium in physical processes involves a dynamic, stable state where opposing processes occur
2 TRUE
at the same rate.
Equilibrium in physical processes is attainable only in a closed system at a specific temperature.
3 TRUE
Equilibrium in physical processes occurs spontaneously in an open system at any temperature.
4 FALSE
Equilibrium is characterized by the constancy of measurable properties, such as vapor pressure or
5 TRUE
solute concentration.
Equilibrium is marked by the variability of measurable properties like vapor pressure and solute
6 FALSE
concentration.
7 For solid-liquid equilibrium, there is a fixed melting point at constant pressure. TRUE
Henry's Law governs the equilibrium of gases in liquids, where the concentration of a gas in a
8 TRUE
liquid is proportional to the gas pressure.
In solid-liquid equilibrium, such as ice and water at 273K, both processes, i.e., dissolution and
9 TRUE
crystallization, occur simultaneously.
Physical processes achieve equilibrium in closed systems, where measurable properties remain
10 TRUE
stable due to equal rates of opposing processes.
Physical processes never reach equilibrium in closed systems; properties continually fluctuate.
11 FALSE
12 Saturated solutions exhibit fluctuating solute concentrations at different temperatures. FALSE
13 Saturated solutions have a constant solute concentration at a given temperature. TRUE
The equilibrium vapor pressure of water increases with temperature, and the normal boiling point
14 TRUE
depends on atmospheric pressure.
15 The extent of a reaction at equilibrium is fixed and unaltered by conditions. FALSE
The extent of a reaction at equilibrium varies with conditions; optimization of conditions in
16 TRUE
industrial and lab settings is vital for favorable equilibrium.
1 OF 19 RI_Best Wishes
, XI_Chem_New Chap-6_Equilibrium_[True or False Statement Questions]
Statements [6.2 EQUILIBRIUM IN CHEMICAL PROCESSES – DYNAMIC EQUILIBRIUM; 6.3 LAW OF
Sl # TRUE/FALSE
CHEMICAL EQUILIBRIUM AND EQUILIBRIUM CONSTANT
At a constant temperature, the equilibrium constant remains the same, regardless of changes in
1 TRUE
initial concentrations.
Changing the stoichiometric coefficients in a chemical equation by a factor n leads to an
2 TRUE
equilibrium constant equal to the original constant raised to the power of n.
3 Equilibrium constants (K) are determined solely by the concentration of reactants. FALSE
Equilibrium constants (K) have no connection to stoichiometric coefficients in chemical equations.
4 FALSE
Equilibrium constants (K) result from product concentrations raised to coefficients divided by the
5 TRUE
same for reactants.
Equilibrium constants (K) show product-to-reactant concentration ratio with stoichiometric
6 TRUE
coefficients in a balanced equation.
Equilibrium constants are expressed in terms of molar concentrations and are independent of the
7 TRUE
physical state of the substances involved.
Equilibrium constants can change if the stoichiometric coefficients in a chemical equation are
8 TRUE
modified by multiplying the entire equation by a factor.
Equilibrium constants for reverse reactions are always different from those for the forward
9 FALSE
reactions.
Equilibrium constants for reverse reactions are the reciprocals of the equilibrium constants for
10 TRUE
the forward reactions.
Equilibrium constants provide a quantitative measure of the extent to which a chemical reaction
11 TRUE
proceeds toward products at a given temperature.
Equilibrium constants, like Kc, are expressed in concentrations of moles per liter (mol/L) and
12 TRUE
reflect the dynamic nature of chemical equilibrium.
Equilibrium in chemical processes is dynamic, involving both forward and reverse reactions. It can
13 TRUE
be reached from either direction.
Equilibrium occurs when forward and reverse reaction rates equalize, maintaining constant
14 TRUE
reactant and product concentrations.
If a chemical equation is multiplied by a factor, the equilibrium constant for the new equation is
15 TRUE
the original constant raised to the power of that factor.
Quoting the value of an equilibrium constant should specify the form of the balanced chemical
16 TRUE
equation to avoid confusion when multiple forms exist.
The equilibrium constant (Kc) for a reaction is expressed in concentrations (mol/L) of the
17 TRUE
reactants and products.
18 The equilibrium constant changes with temperature, even at a constant temperature. FALSE
The equilibrium constant, K, depends on the temperature, not the concentrations of reactants
19 FALSE
and products.
The equilibrium constant, K, is a numerical value that reflects the relationship between the
20 TRUE
concentrations of reactants and products in a chemical reaction at equilibrium.
The expression for the equilibrium constant reflects the stoichiometric coefficients in the
21 TRUE
balanced chemical equation, emphasizing the importance of a balanced equation.
2 OF 19 RI_Best Wishes
, XI_Chem_New Chap-6_Equilibrium_[True or False Statement Questions]
Sl # Statements [6.4 HOMOGENEOUS EQUILIBRIA; 6.5 HETEROGENEOUS EQUILIBRIA] TRUE/FALSE
Concentration-based equilibrium constants have no connection to partial pressures, creating
1 FALSE
confusion in gas reactions.
Equilibrium constants can be dimensionless if standard states are specified for concentrations of
2 TRUE
solutes or partial pressures of gases.
Equilibrium constants can be expressed as dimensionless quantities when the standard state is
3 TRUE
specified, making them independent of units.
Equilibrium constants can be expressed in terms of concentrations or partial pressures without
4 TRUE
affecting their dimensionless nature.
Equilibrium constants can be expressed in terms of molar concentrations or partial pressures,
5 TRUE
depending on the phase of the reactants and products.
Equilibrium constants can change with temperature and are influenced by the stoichiometry of
6 TRUE
the balanced equation.
Equilibrium constants can only be expressed in terms of molar concentrations, rendering partial
7 FALSE
pressures irrelevant.
Equilibrium constants expressed in different units still hold the same significance in describing the
8 TRUE
extent of a reaction at equilibrium.
Equilibrium constants expressed in terms of partial pressures offer convenience when dealing
9 TRUE
with reactions involving gases.
Equilibrium constants for different reactions involving gases can be calculated based on their
10 TRUE
respective partial pressures at a given temperature.
Equilibrium constants for gaseous reactions are identical to their concentration-based
11 FALSE
counterparts, eliminating the need for multiple expressions.
Equilibrium constants for gaseous reactions can be related to concentration-based equilibrium
12 TRUE
constants using the ideal gas equation.
Equilibrium constants for gaseous reactions can differ in magnitude from their concentration-
13 TRUE
based counterparts due to the influence of partial pressures.
Equilibrium constants for reactions involving gases are usually expressed in terms of partial
14 TRUE
pressure, represented as Kp, using the ideal gas equation.
Equilibrium constants for various reactions involving gases are indistinguishable, making them
15 FALSE
irrelevant for practical purposes.
Equilibrium constants remain consistent irrespective of alterations in temperature or adjustments
16 FALSE
in stoichiometry.
For reactions involving gases, equilibrium constants can be expressed using partial pressures as in
17 TRUE
Kp = pCO2 / pCO, based on the gas phase.
For reactions involving pure solids or liquids, their concentrations remain constant and do not
18 TRUE
affect the equilibrium constant expression.
For the thermal decomposition of calcium carbonate, the equilibrium constant expression
19 TRUE
becomes Kp = pCO2, where pCO2 is the partial pressure of CO2.
Heterogeneous equilibria involve more than one phase, such as a gas and a solid. Concentrations
20 of pure solids or liquids do not appear in the equilibrium constant expression, e.g., CaCO3(s) ⇌ TRUE
CaO(s) + CO2(g).
Heterogeneous equilibria involve multiple phases, such as a solid and a gas, like the thermal
21 TRUE
decomposition of CaCO3: CaCO3(s) ⟶ CaO(s) + CO2(g).
In a homogeneous equilibrium, all reactants and products are in the same phase, as in the
22 TRUE
gaseous reaction N2(g) + 3H2(g) ⇌ 2NH3(g).
In a homogeneous equilibrium, reactants and products are in different phases, causing chaos in
23 FALSE
reactions like N2(g) + 3H2(g) ⇌ 2NH3(g).
In a homogeneous system, reactants and products exist in the same phase, as seen in gas-phase
24 TRUE
reactions like N2(g) + 3H2(g) ⟶ 2NH3(g).
3 OF 19 RI_Best Wishes
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