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## What is the number of moles of 11.2 liters of nitrogen gas at STP?

At STP, there will be **1/2 moles** of N2 in 11.2 litres of N2.

## How many molecules are there in 11.2 L of N2 at STP?

So we simply divide the volume by the molar volume: 11.2⋅L 22.4⋅L ⋅mol−1×NA=12×11mol×NA . 12×mol×6.022×1023⋅mol−1=**3.01×1023 gaseous molecules**……..

## How many moles of oxygen will occupy a volume of 2.5 liters?

So, there will be **0.122 moles** of oxygen gas.

## What is the formula for STP?

It can be written as: **V = nRT/P**. “P” is pressure, “V” is volume, n is the number of moles of a gas, “R” is the molar gas constant and “T” is temperature.

## What is the volume of 4 moles of n2 gas at STP?

I get **3.3 liters**.

## What is the value of PV for 11.2 Litres of an ideal gas at STP?

At STP for 11.2 litres of a gas pv is equal to **1RT**.

## How many molecules are there in 22.4 liters of a gas at STP?

More specifically, **6.02 x 10 ^{23} particles** (1 mole) of ANY GAS occupies 22.4 Liters at STP.