Can someone check my answer? The question is: In order for the reaction 2Al(s) + 6HCl(aq)-> 2AlCl3(aq) + 3H2(g) to occur, which of the following must be true?
a. Al must be above Cl on the activity series.
b. Al must be above H on the activity series.
c. Heat must be supplied for the reaction.
d. AlCl3 must be a precipitate.
It was between a or b and I believe it is b. Thanks
B it is. Look at the reaction. It is a single replacement. What is it replacing? It is replacing H; therefore, it must be above H and where it is with respect to Cl is immaterial.
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To determine which statement is true for the reaction to occur, let's evaluate each option:
a. Al must be above Cl on the activity series.
This statement is incorrect. The activity series is a list that indicates the relative reactivity of metals. Aluminum (Al) is indeed above chlorine (Cl) on the activity series, but the activity series only applies to metal displacement reactions, not to reactions like the one given.
b. Al must be above H on the activity series.
This statement is correct. Hydrogen (H) is normally found in acids such as hydrochloric acid (HCl). When a metal like aluminum reacts with an acid, it displaces the hydrogen from the acid, producing hydrogen gas (H2). So, in this reaction, aluminum (Al) must be above hydrogen (H) on the activity series.
c. Heat must be supplied for the reaction.
This statement is not necessary for the reaction to occur. The reaction between aluminum and hydrochloric acid is exothermic, which means it releases heat. However, it does not require external heat to start or proceed.
d. AlCl3 must be a precipitate.
This statement is incorrect as well. AlCl3 is not a precipitate in this reaction. It forms an aqueous solution, meaning it dissolves in water.
Therefore, the correct answer is b. Al must be above H on the activity series.
To determine the correct answer, we need to understand the factors that determine whether a chemical reaction will occur. In this case, we are given the balanced equation:
2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2(g)
Now, let's evaluate each option:
a. Al must be above Cl on the activity series.
The activity series is a list of metals arranged in order of their reactivity. A metal higher on the activity series will displace a metal lower on the activity series from its compound. However, in the given equation, aluminum (Al) is not displacing chlorine (Cl) from a compound, so this option is not necessary for the reaction to occur.
b. Al must be above H on the activity series.
If aluminum (Al) is above hydrogen (H) on the activity series, it means that aluminum is more reactive than hydrogen. In this reaction, aluminum reacts with hydrochloric acid (HCl) by displacing hydrogen and forming aluminum chloride (AlCl3) and hydrogen gas (H2). Therefore, this option is likely to be true.
c. Heat must be supplied for the reaction.
Although heat is often required in chemical reactions to increase the reaction rate, it is not necessary for this specific reaction. This reaction can occur at room temperature without adding additional heat, as long as aluminum (Al) is more reactive than hydrogen (H).
d. AlCl3 must be a precipitate.
A precipitate is a solid that forms when two aqueous solutions react. In this case, the product AlCl3 is an aqueous solution, not a precipitate. Therefore, this option is not necessary for the reaction to occur.
Based on the above analysis, it can be concluded that option b, "Al must be above H on the activity series," is the correct answer. It suggests that aluminum (Al) must be more reactive than hydrogen (H) for the reaction to occur.