Question

Consider the complete reaction of 43.0 g of silicon with excess nitrogen gas in the reaction shown below. What mass of product forms?3Si + 2N2 → Si3N4 Answer = _________ grams of product

Answer 1

To determine the mass of product formed in the reaction between silicon and nitrogen gas, we can use the given mass of silicon and the balanced chemical equation. Using the molar mass of silicon, we can calculate the moles of silicon that react and then use the stoichiometry of the reaction to determine the moles of silicon nitride formed. Finally, we can calculate the mass of silicon nitride using its molar mass.

Step-by-step explanation:

To determine the mass of product formed in the reaction, we need to calculate the amount of product formed using the given mass of silicon. From the balanced chemical equation, we can see that 3 moles of silicon react with 2 moles of nitrogen gas to form 1 mole of silicon nitride. Using the molar mass of silicon (28.0855 g/mol), we can calculate the moles of silicon that react by dividing the given mass of silicon (43.0 g) by the molar mass. This will give us the moles of silicon nitride formed.

Then, using the equation:
1 mol Si3N4 = 43.0 g Si3N4

We can find the mass of silicon nitride formed by multiplying the moles of silicon nitride by the molar mass of silicon nitride (140.2864 g/mol).

Therefore, the mass of silicon nitride formed is 140.2864 g.

Answer 2

The answer to your question is : no.of moles of Si = 43/atomic mass of Si = 43/28.1 = 1.53

according to reaction 3 moles of Si gives 1 mole of Si3N4

so 1.53 mole of Si will give 1.53/3 = 0.51 mole of Si3N4

molar mass of Si3N4 = 140.28 g/mole

it means that 1 mole of Si3N4 = 140.28 g

so 0.51 mole of Si3N4 = 0.51 X 140.28 = 71.543 g