Question

After substantial heating, 0.194g of uranium produced 0.246g of a compound with oxygen the empirical formula is uo2 u5o2 uo4 u2o5 uo3

Answer 1

The empirical formula of the compound formed after heating uranium is UO₂ .

Step-by-step explanation:

Upon substantial heating, uranium reacts with oxygen to form a compound. To determine the empirical formula, we must find the ratio of the elements present. The given data states that 0.194g of uranium produces 0.246g of the compound.

First, find the moles of each element:

1. Moles of uranium U : 0.194 g / molar mass of U

2. Moles of oxygen O : 0.246g / molar mass of O

Next, determine the simplest ratio by dividing the moles of each element by the smallest mole value. In this case, if the ratio is not already a whole number, multiply each value by the same factor to achieve a whole number ratio. The resulting ratio represents the subscripts in the empirical formula.

For instance, if the ratio is
`\( U_aO_b \)`, multiply both a and b by a factor to ensure they are whole numbers. The final empirical formula is
`\( U_{\text{whole number}}O_{\text{whole number}} \)`, representing the simplest ratio of uranium to oxygen in the compound.

In this specific case, the ratio simplifies to UO₂ , indicating that the empirical formula of the compound formed through the heating of uranium is uranium dioxide.