heating 4.05 g of a metal oxide (molar mass of metal x = 55.9 g/mol) in carbon monoxide (co) yields the pure metal and carbon dioxide. the mass of the metal product is 2.83 g. from the data given, use the simplest formula of the oxide to write a balanced equation for the reaction. use x to denote the metal.
part 1 of 2
what is the simplest formula of the oxide? x₂o₃
part: 1 / 2
part 2 of 2
write the balanced equation for the reaction. include the phase abbreviations.

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Accepted Answer

# Explanation:
## Step1: Identify reactants and products
The reactants are metal oxide ($X_2O_3$) and carbon monoxide ($CO$). The products are metal ($X$) and carbon dioxide ($CO_2$).
## Step2: Balance the equation
- Balance $X$ atoms: There are $2$ $X$ atoms in $X_2O_3$. So, put a coefficient of $2$ in front of $X$ on the product side.
- Balance $O$ atoms: In $X_2O_3$, there are $3$ $O$ atoms. In $CO$ and $CO_2$, we can use the following approach. Let the coefficient of $X_2O_3$ be $1$, coefficient of $CO$ be $3$, coefficient of $CO_2$ be $3$ (because from $X_2O_3$ we have $3$ $O$ atoms which combine with $3$ $CO$ to form $3$ $CO_2$). And coefficient of $X$ is $2$

# Answer:
$X_2O_3(s)+3CO(g)
ightarrow 2X(s)+3CO_2(g)$

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Question

Explanation:

Step1: Identify reactants and products

Step2: Balance the equation

Answer: