part 4: double replacement reactions
10. __rboh + __licl → __li(oh) + __rbcl

Question

Accepted Answer

# Explanation:
## Step1: Identify the reaction type
This is a double - replacement reaction. In a double - replacement reaction, the general form is $AB + CD
ightarrow AD+CB$. Here, $AB = RbOH$, $CD = LiCl$, $AD$ should be $RbCl$ and $CB$ should be $LiOH$. The unbalanced equation is $RbOH+LiCl
ightarrow LiOH + RbCl$.

## Step2: Balance the equation
For double - replacement reactions involving ionic compounds, we check the balance of each element.
- For $Rb$: There is 1 $Rb$ on the left (in $RbOH$) and 1 $Rb$ on the right (in $RbCl$).
- For $O$: There is 1 $O$ on the left (in $RbOH$) and 1 $O$ on the right (in $LiOH$).
- For $H$: There is 1 $H$ on the left (in $RbOH$) and 1 $H$ on the right (in $LiOH$).
- For $Li$: There is 1 $Li$ on the left (in $LiCl$) and 1 $Li$ on the right (in $LiOH$).
- For $Cl$: There is 1 $Cl$ on the left (in $LiCl$) and 1 $Cl$ on the right (in $RbCl$).

Since the number of each type of atom is the same on both sides of the equation, the balanced equation is $RbOH + LiCl=LiOH+RbCl$. So the coefficients are $1$ for each compound.

# Answer:
$1RbOH + 1LiCl
ightarrow1LiOH + 1RbCl$

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QUESTION IMAGE

Question

Explanation:

Step1: Identify the reaction type

Step2: Balance the equation

Answer: