For a given equilibrium reaction for which #K_"eq"=6.4#...what scenario will alter the equilibrium value?
#"i. the use of a catalyst;"#
#"ii. an increase in the concentration of reactants;"#
#"iii. the equilibrium constant will remain unchanged;"#
#"iv. the use of a catalyst."#
Option
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Any change in temperature, pressure, or concentrations of reactants or products will alter the equilibrium value of a reaction. Specifically, increasing the temperature will shift the equilibrium position in the direction of the endothermic reaction, while decreasing the temperature will favor the exothermic reaction. Similarly, changing the pressure (for reactions involving gases) or concentrations of reactants/products will cause the system to adjust to reach a new equilibrium position.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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- At a certain temperature, 4.0 mol #NH_3# is introduced into a 2.0 L container, and the #NH_3# partially dissociates to #2NH_3(g)\rightleftharpoonsN_2(g)+3H_2(g)#. At equilibrium, 2.0 mol #NH_3# remains. What is the value of #K_c#?
- For the following reaction delta H = 2816 kJ. 6 CO2 (g) + 6 H2O (l) <---> C6H12O6 (s) + 6 O2 (g). What will be the effect on the equilibrium yield of C6H12O6 (s) if: ?
- What is the equilibrium constant for the following reaction at #"298 K"#? And what is the partial pressure of #"S"_8(g)# above #"S"(s, "orthorhombic")# at equilibrium at #25^@ "C"#?
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