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
2 answers
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.
-->
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.
1 answer