What volume will 1.0g N2 gas occupy at stp?

Answer 1

A mole of an ideal gas at STP occupies one standard molar volume. This is about 22.4 liters. (If you want the exact figure, PV = nRT; n, T, and P are known (1 mole, standard temperature, standard pressure), R is a constant; solve for V.)

Answer 2

At STP (standard temperature and pressure: 0°C and 1 atm), 1 mol of any gas occupies 22.4 L. The molar mass of N2 is 28 g/mol, so 1 g of N2 is 1/28 mol. Therefore, 1.0 g of N2 gas will occupy (1/28) x 22.4 L = 0.8 L at STP.

Answer 3

One mole of any ideal gas occupies 22.4 liters at STP - this is called molar volume.

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Answer 4

Because water vapor is considered an ideal gas and all ideal gases have a 1 mol: 22.4 L ratio at STP, the volume occupied by 1 mol of water vapor will be 22.4 L.

Answer 5

1g of N2 = 1/28 = 0.036mol. This times 22.4 = 0.81L or 810mL.

Answer 6

The volume is 0,8 L.