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kotykmax [81]
3 years ago
9

Write a balanced chemical equation based on the following description:

Chemistry
1 answer:
OLga [1]3 years ago
7 0

Answer:

IrBr₃(aq) + 3AgC₂H₃O₂(aq) ⟶ Ir(C₂H₃O₂)₃(aq) + 3AgBr(s)  

Explanation:

Iridium(III) bromide(aq) + silver acetate(aq) ⟶ iridium(III) acetate + silver bromide

You have probably learned NAG SAG and "Cats Cradle Old People," Sally Said.

I've listed the rules below.

\begin{array}{lll}\textbf{Soluble} & \textbf{Insoluble}\\\textbf{N}\text{itrates} &\textbf{C} \text{arbonates }\\ \textbf{A}\text{cetates} & \textbf{C}\text{hromates}\\ \textbf{G}\text{roup 1} & \textbf{O}\text{ hydrOxides}\\ &  \textbf{P} \text{hosphates}\\\end{array}

\begin{array}{lll}\textbf{S}\text{ulfates} &\textbf{S} \text{ulfites}\\ \textbf{A}\text{mmonium}& \textbf{S}\text{ulfides}\\& \textbf{P}\text{b halides}\\\textbf{G}\text{roup 17}& \textbf{M}\text{ercury(II) halides}\\&\textbf{S}\text{ilver halides}\\ \end{array}

The PMS group are the exception to the rule that halides are usually soluble.

We can use the solubility rules to decide which product is the precipitate.

Iridium(III) acetate — soluble (Acetate)

Silver bromide — insoluble (PMS,  Silver halide)

So silver bromide is a precipitate.

The word equation becomes

Iridium(III) bromide(aq) + silver acetate(aq) ⟶ iridium(III) acetate(aq) + silver bromide(s)

In symbols, the equation is

IrBr₃(aq) + 3AgC₂H₃O₂(aq) ⟶ Ir(C₂H₃O₂)₃(aq) + 3AgBr(s)

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Answer:

781×10¯² g of MgCl₂.

Explanation:

The balanced equation for the reaction is given below:

Mg + 2HCl —> MgCl₂ + H₂

Next, we shall determine the mass of HCl that reacted and the mass of MgCl₂ produced from the balanced equation. This is illustrated below:

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From the balanced equation above,

73 g of HCl reacted to produce 95 g of MgCl₂.

Finally, we shall determine the mass of MgCl₂ produced by the reaction of 6 g of HCl. This can be obtained as follow:

From the balanced equation above,

73 g of HCl reacted to produce 95 g of MgCl₂.

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