`P_(4)O_(6)` and `P_(4)O_(10)` are formed by burning `P_(4)` with `O_(2)` as:
`P_(4) + 3O_(2) to P_(4)O_(6)`
`P_(4) + 5O_(2) to P_(4)O_(10)`
What are the masses of `P_(4)O_(6)` and `P_(4)O_(10)` that will be produced by the combustion of 2.0 g of `P_(4)` in 2.0 g of oxygen leaving no `P_(4)` and `O_(2)` ?

Explanation

To determine the masses of \( P_4O_6 \) and \( P_4O_{10} \) produced by the combustion of 2.0 g of \( P_4 \) in 2.0 g of oxygen, we can follow these steps:

### Step 1: Write the balanced equations
The balanced equations for the combustion of \( P_4 \) are:
1. \( P_4 + 3O_2 \rightarrow P_4O_6 \)
2. \( P_4 + 5O_2 \rightarrow P_4O_{10} \)

### Step 2: Calculate the molar masses
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