Can someone explain this to me?
In the reaction:
-->
AgCl(s)<_______ Ag+(aq) + Cl-(aq) the shorter arrow pointing to the right shows that the qe. mixture consists mostly of ______.
--->
In the reaction HC2h302 + H20<_______ H30+ + C2h302-, when the concentration of H30+ is decreased, the concentration of HC2H302 will ?
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On a concentration x time graph, H2(g) + 02 (g) is in equilibrium with 2HI(g) + energy.
What will the concentration of I2 is increased will the:
HI curve rise, the I2 curve rise and H2 curve drops?
TIA
also if a catalyst is present at the initial introduction of reactants, how would the graph differ ?
In the reaction:
-->
AgCl(s)<_______ Ag+(aq) + Cl-(aq) the shorter arrow pointing to the right shows that the qe. mixture consists mostly of ______.
--->
You can see that spacing is a real problem on these boards and you have both arrows pointing the same direction; however, I assume the question is to fill in the blank. AgCl is so insoluble in water that the majority of the material at equilibrium is as the solid form and only minor amounts of Ag^+ and Cl^- are present.
In the reaction HC2h302 + H20<_______ H30+ + C2h302-, when the concentration of H30+ is decreased, the concentration of HC2H302 will ?
This is a common ion/Le Chatelier question. Increasing one of the products shifts the equilibrium to the left; increasing one of the reactants shifts the equilibrium to the right. Therefore, decreasing H3O^+ will decrease HC2H3O2. Think of it this way. Decreasing H3O^+ makes the reaction try to make up for that by increasing it; it can do that by more HC2H3O2 ionizing to form H3O^+ and C2H3O2^-. So HC2H3O2 decreases, C2H3O2^- increases, and H3O^+ increases.
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On a concentration x time graph, H2(g) + 02 (g) is in equilibrium with 2HI(g) + energy.
What will the concentration of I2 is increased will the:
HI curve rise, the I2 curve rise and H2 curve drops?
You haven't copied this problem correctly.
In the first reaction: AgCl(s) -> Ag+(aq) + Cl-(aq), the shorter arrow pointing to the right indicates that the reaction is a dissociation reaction. This means that AgCl is breaking apart into Ag+ ions and Cl- ions when it is dissolved in water. Therefore, the mixture consisting mostly of Ag+(aq) and Cl-(aq) indicates that the AgCl has largely dissociated into its constituent ions.
In the second reaction: HC2H302 + H2O -> H3O+ + C2H302-, when the concentration of H3O+ is decreased, the concentration of HC2H302 will increase. This is because the reaction is an acid-base reaction, and H3O+ is acting as an acid by donating a proton to form HC2H302. When the concentration of the acid (H3O+) decreases, according to Le Chatelier's principle, the reaction will shift to the right to counteract the decrease in H3O+. As a result, more HC2H302 will be formed to maintain equilibrium.
Moving on to the third question: When the concentration of I2 is increased in the reaction H2(g) + O2(g) <-> 2HI(g) + energy, the concentration of HI will increase, the concentration of I2 will decrease, and the concentration of H2 will remain unchanged. This is because an increase in the concentration of I2 will shift the equilibrium position of the reaction to the left, according to Le Chatelier's principle, in order to counteract the increase in I2 concentration. As a result, more HI will be formed, leading to an increase in its concentration. Conversely, the concentration of I2 will decrease, and the concentration of H2 will remain unchanged as it is not directly affected by the change in I2 concentration.
I hope this explanation helps clarify the reactions and the effects of specific changes on their concentrations.