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So, there will be 0.122 moles of oxygen gas.

## How many moles are in 2l of oxygen gas at STP?

Assuming that the gas is at standard temperature and pressure (STP), one mole of any gas occupies 22.4 L . This means the number of moles of O2 is 222.4=0.089 mol .

## How many moles of oxygen will occupy a volume of 2.5 liters at 1.2 atm and 25ºc?

1. How many moles of oxygen will occupy a volume of 2.5 liters at 1.2 atm and 25° C? PV = V (1.2 n. 0821) (298) = 123 mols 2.

## How many moles of oxygen are in 5.5 L canister at STP?

There are 0.25mol of O2 in the 5.5-L canister.

## What is the volume of one mole of oxygen at STP?

Finally, use the fact that one mole of oxygen would occupy a volume of 22.4 L at STP to figure out the volume of the oxygen in this question at STP.

## What is the volume of 2 moles of gas at STP?

2: A mole of any gas occupies 22.4L at standard temperature and pressure (0oC and 1atm).

## What is the volume in liters of 2.00 moles of hydrogen at STP?

According to this, one mole of hydrogen gas at STP will occupy 22.4 L of volume. Therefore, 2 moles of hydrogen gas will occupy a volume twice of 22.4 L i.e. 44.8 L. So, we can see from the above discussion that 2 moles of hydrogen gas occupies 44.8L volume.

## How many moles of gas does it take to occupy 120 liters at a pressure of 2.3 atm and a temperature of 340 K?

n = PV (2.3atm/120 L) =9.89 mols P = 2.3 atm RT (0,0821 (afm) ( 340k) T = 340k n=?

## What is the density of nh3 at 800 torr and 25 degrees C?

0.7327 g/L.

## What is the volume of 0.5 moles of gas at STP?

0.5 moles⋅22.4 L/mol=11.2 L , and so on.

## What volume does 16.0 g of O2 occupy at STP?

1 mole of a gas occupy =22.4L volume at STP therefore, 16gO2 gas =0.5 mole of O2 gas will occupy =0.5×22.41=11.2L at STP.

## What is the mass of 2 mole of NaOH?

Answer: The molar mass of the compound NaOH is 40 g/mol.

## How do you calculate oxygen volume?

Calculate the volume (in cubic meters) of gaseous oxygen using the ideal gas law: multiply the amount of oxygen (in moles) by temperature and the molar gas constant followed by dividing the product by pressure.