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If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium. If a chemical reaction is at equilibrium and experiences a change in pressure, temperature, or concentration of products or reactants, the equilibrium shifts in the opposite direction to offset the change. This page covers changes to the position of equilibrium due to such changes and discusses briefly why catalysts have no effect on the equilibrium position.
For example, if the system is changed in a way that increases the concentration of one of the reacting species, it must favor the reaction in which that species is consumed. In other words, if there is an increase in products, the reaction quotient, Qc, is increased, making it greater than the equilibrium constant, Kc.
Answer:
Explanation:
= Half-life of carbon = 5700 years
t = Time at which the remaining mass is to be found = 10400 years
= Initial mass of carbon = 11 g
Decay constant is given by

Amount of mass remaining is given by

The amount of the substance that remains after 10400 years is
.
Answer:
Weight % of NH₃ in the aqueous waste = 2.001 %
Explanation:
The chemical equation for the reaction

Moles of HCl = Molarity × Volume
= 0.1039 × 31.89 mL × 
= 0.0033 mole
Total mass of original sample = 25.888 g + 73.464 g
= 99.352 g
Total HCl taken for assay = 
= 0.1083 g
Moles of NH₃ = 
= 0.03047 moles
Mass of NH₃ = number of moles × molar mass
Mass of NH₃ = 0.03047 moles × 17 g
Mass of NH₃ = 0.51799
Weight % of NH₃ =
%
Weight % of NH₃ in the aqueous waste = 2.001 %