How does adding NH3 to the reaction below affect the equilibrium of the reaction?
N2(g) + 3H2(g) <=> 2NH3(g)
Increasing the amount of NH3 will make Q larger than K. A net reaction occurs in the direction to increase NH3, or the forward reaction.
Increasing the amount of NH3 will make Q larger than K. A net reaction occurs in the direction to reduce NH3, or the reverse reaction.
Increasing the amount of NH3 will make Q smaller than K. A net reaction occurs in the direction to increase NH3, or the forward reaction.
Increasing the amount of NH3 will make Q smaller than K. A net reaction occurs in the direction to reduce NH3, or the reverse reaction.
!@#$%^& you bob
The answer is: Increasing the amount of NH3 will make Q larger than K. A net reaction occurs in the direction to reduce NH3, or the reverse reaction.
Join the club dawg
So is it the third one?
Nevermind I think it would be the first one
To determine how adding NH3 to the reaction affects the equilibrium, we need to compare the values of Q and K. Q is the reaction quotient, which is calculated using the concentrations of the reactants and products in the reaction at a given moment. K, on the other hand, is the equilibrium constant, which represents the ratio of the concentration of the products to the concentration of the reactants at equilibrium.
In this particular reaction, N2(g) + 3H2(g) ↔ 2NH3(g), the balanced equation shows that two molecules of NH3 are formed from one molecule of N2 and three molecules of H2. Therefore, according to the stoichiometry of the reaction, the forward reaction forms more NH3, while the reverse reaction breaks down NH3 to form N2 and H2.
Now, let's evaluate the statements:
Increasing the amount of NH3 will make Q larger than K. A net reaction occurs in the direction to increase NH3, or the forward reaction.
This statement is incorrect. If the amount of NH3 is increased, it will increase the numerator of Q, but since K is the ratio of products to reactants at equilibrium, increasing the numerator will not necessarily result in Q being larger than K. Therefore, there is no guarantee that the forward reaction will occur to increase NH3.
Increasing the amount of NH3 will make Q larger than K. A net reaction occurs in the direction to reduce NH3, or the reverse reaction.
This statement is also incorrect. Similarly to the previous statement, increasing the amount of NH3 affects the numerator of Q, but it doesn't necessarily make Q larger than K. Therefore, it does not mean the reverse reaction will occur to reduce NH3.
Increasing the amount of NH3 will make Q smaller than K. A net reaction occurs in the direction to increase NH3, or the forward reaction.
This statement is correct. If the amount of NH3 increases, it will contribute to an increase in the numerator of Q. If Q is smaller than K, it indicates that the concentration of NH3 is lower than the equilibrium concentration, and therefore, the forward reaction will occur to increase NH3 until equilibrium is reached.
Increasing the amount of NH3 will make Q smaller than K. A net reaction occurs in the direction to reduce NH3, or the reverse reaction.
This statement is incorrect. Increasing the amount of NH3 will increase the numerator of Q, potentially making Q larger than K. If Q is larger than K, it indicates that the concentration of NH3 is higher than the equilibrium concentration, and therefore, the reverse reaction will occur to reduce NH3 until equilibrium is reached.
Overall, the correct statement is: Increasing the amount of NH3 will make Q smaller than K. A net reaction occurs in the direction to increase NH3, or the forward reaction.
Le Chatelier's Principle says in very unsophisticated terms that if we do something to a system at equilibrium that the equilibrium will shift so as to undo what we did to it.
So if you increase NH3 the reaction will shift so as to reduce the NH3 concn which means it will move to the left. 1 and 3 move it to the left with the difference being in whether Q is larger or smaller. Will Q be larger or smaller.?