Question

For the reaction 146C⟶147N+?, if 100.0 g of carbon reacts, what volume of nitrogen gas (N2) is produced at 273K and 1 atm? a) 22.4 L

b) 11.2 L
c) 44.8 L
d) 56.0 L

Answer 1

To determine the volume of nitrogen gas produced in the given reaction, we need to first balance the equation and calculate the number of moles of carbon (C) that react.

The balanced equation is: 146C -> 147N + 1H. We can see that for every mole of carbon, we get one mole of nitrogen gas. Since the molar mass of carbon is 12.01 g/mol, we can calculate the number of moles of carbon using its mass. The volume of nitrogen gas produced can be calculated using the ideal gas law.

Step-by-step explanation:

To determine the volume of nitrogen gas produced in the given reaction, we need to first balance the equation and calculate the number of moles of carbon (C) that react.

The balanced equation is:

14^6C -> 14^7N + 1^1H

We can see that for every mole of carbon, we get one mole of nitrogen gas.

Since the molar mass of carbon is 12.01 g/mol, we can calculate the number of moles of carbon using its mass:

Number of moles of carbon = mass of carbon / molar mass of carbon

Number of moles of carbon = 100.0 g / 12.01 g/mol = 8.33 moles (approximately)

Since the number of moles of nitrogen gas is equal to the number of moles of carbon, the volume of nitrogen gas produced can be calculated using the ideal gas law:

Volume of nitrogen gas = Number of moles of nitrogen gas * molar volume of gas at STP

Volume of nitrogen gas = 8.33 moles * 22.4 L/mol = 186.41 L (approximately)