Question

2.8g of silicon react with 3.2g of oxygen to give a compound, which is shown below. The relative atomic mass of silicon is 28 and of oxygen is 16. What is the value of y in the formula below?​

Answer 1

Answer:

For Silicon = \frac{0.1}{0.1}=1

0.1

0.1

=1

For Oxygen = \frac{0.2}{0.1}=2

0.1

0.2

=2

Step 3: Taking the mole ratio as their subscripts.

The ratio of Si : O = 1 : 22.8g of silicon react with 3.2g of oxygen to give a compound, which is shown below. The relative atomic mass of silicon is 28 and of oxygen is 16. What is the value of y in the formula below?Moles of Silicon =\frac{\text{Given mass of Silicon}}{\text{Molar mass of Silicon}}=\frac{2.8g}{28g/mole}=0.1moles

Molar mass of Silicon

Given mass of Silicon

=

28g/mole

2.8g

=0.1moles

Moles of Oxygen = \frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{3.2g}{16g/mole}=0.2moles

Molar mass of oxygen

Given mass of oxygen

=

16g/mole

3.2g

=0.2moles

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number ofAnswer: The value of 'y' in the formula given is 2

Explanation:

We are given:

The given chemical formula of the compound is SiO_ySiO

y

Mass of Si = 2.8 g

Mass of O = 3.2 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Silicon =\frac{\text{Given mass of Silicon}}{\text{Molar mass of Silicon}}=\frac{2.8g}{28g/mole}=0.1moles

The chemical formula of the compound becomes SiO_2SiO

2

Hence, the value of 'y' in the formula given is 2

Answer 2

Answer:

I don't know

Explanation:

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