Chemistry, 25.03.2020 05:47 ruchierosanp1n3qw

The balanced equation for the reaction of aluminum metal and chlorine gas is 2Al(s) + 3Cl2(g) → 2AlCl3(s) Assume that 0.64 g Al is mixed with 0.36 g Cl2. (a) What is the limiting reactant? Al Cl2 (b) What is the maximum amount of AlCl3, in grams, that can be produced?

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Answer from: nini261

a)Cl₂ is the limiting reaction

b) Maximum amount of AlCl₃ = 0.45g

Explanation:

2Al(s) + 3Cl2(g) → 2AlCl3(s)

54g 212.72g 266.7g

0.64g 0.36

a) 54g Al ------------ 212.72g

0.64g ------------- ?

mass of cl₂ required

$= \frac{0.64 \times 212.72 }{54} \\\\= 2.52g$

we have 0.36g Cl₂, so Cl₂ is the limiting reaction

212.72g Cl₂---------- 266.7g AlCl₃

0.36g Cl₂ ----------- ?

mass of AlCl₃ =

$\frac{0.36 \times 266.7 }{212.72} \\\\= 0.45g$

Maximum amount of AlCl₃ = 0.45g

Answer from: shaheedbrown06

a) Limiting reactant: Cl₂

b) 0.45 g

Explanation:

(a) The balanced equation is:

2Al(s) + 3Cl₂(g) ⇆ 2AlCl₃(s) (1)

0.64g 0.36g

To find the limiting reactant we need to calculate the number of moles of Al and Cl₂:

$\eta_{Al} = \frac{m}{M}$

where m: is the mass and M: is the molar mass

$\eta_{Al} = \frac{0.64}{27 g/mol} = 0.024 moles$

Similarly, for Cl₂ we have:

$\eta_{Cl_{2}} = \frac{m}{M} = \frac{0.36 g}{(35.45 g/mol)*2} = 5.07 \cdot 10^{-3} moles$

From equation (1) we have that 2 moles of Al reacts with 3 moles of Cl₂, hence, we can find the number of moles of Al that reacts with Cl₂ as follows:

2 moles Al → 3 moles Cl₂

0.024 moles Al → x

$x = \frac{0.024 moles Al*3 moles Cl_{2}}{2 moles Al} = 0.036 moles Cl_{2}$

Hence, we need 0.036 moles of Cl₂ to react with Al, and we have 5.07x10⁻³ moles, so, the limiting reactive is Cl₂ since Al is in excess.

(b) The maximum amount of AlCl₃ in grams that can be produced can be calculated using the limiting reactant, that is to say, Cl₂:

From equation (1) we have that 3 moles of Cl₂ produces 2 moles of AlCl₃, therefore the moles of AlCl₃ are:

$\eta_{AlCl_{3}} = \frac{2 moles AlCl_{3}*5.07 \cdot 10^{-3} moles Cl_{2}}{3 moles Cl_{2}} = 3.38 \cdot 10^{-3} moles$

Finally, the mass of AlCl₃ is:

$m = mol*M = 3.38 \cdot 10^{-3} moles*133.5g/mol = 0.45 g$

Therefore, the maximum amount of AlCl₃ that can be produced is 0.45 g.

I hope it helps you!

Answer from: Quest

i do not get it at all

Answer from: Quest

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. $hbr$ completely dissociates to $h^+$ and $br-$ ions. a is incorrect because $h_2s$ does not fully ionize to $h^+$ and $hs^-$ ions and some remain as the compound $h_2s$ . c and d are incorrect because, $li_2o$ and $libr$ do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise, if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both $li_2o$ and $libr$ have a complete octet so can not accept any electrons which disqualifies them as acids.