0
At standard temperature and pressure (STP), 1 mole of gas occupies 22.4 L. Therefore, a 1500 L room would contain 1500/22.4 moles of gas. One mole contains 6.022 x 10^23 molecules, so you would multiply the number of moles by Avogadro's number to find the total number of molecules in the room.
What else can I help you with?
How many molecules are in 1 mol of H2 at STP?
At standard temperature and pressure (STP), 1 mole of any substance contains Avogadro's number of molecules, which is approximately (6.022 \times 10^{23}) molecules. Therefore, 1 mole of (H_2) (hydrogen gas) contains (6.022 \times 10^{23}) molecules of (H_2).
How many molecules are in 7.3 L of H2 at STP?
At STP, 1 mole of any gas occupies 22.4 L. So, 7.3 L of H2 corresponds to 7.3/22.4 = 0.3263 mol. Since 1 mol of H2 contains 6.022 x 10^23 molecules, the number of molecules in 7.3 L of H2 at STP would be 0.3263 mol x 6.022 x 10^23 molecules/mol = 1.963 x 10^23 molecules.
Can the volume of a gas at STP can be calculated from the number of molecules of a gas?
Yes, the volume of a gas at Standard Temperature and Pressure (STP) can be calculated from the number of molecules using the ideal gas law. At STP (0°C and 1 atm), one mole of an ideal gas occupies 22.4 liters. Since Avogadro's number (approximately (6.022 \times 10^{23}) molecules) defines one mole, you can convert the number of molecules to moles and then multiply by 22.4 liters to find the volume at STP.
What is the STP state of a radium?
At room temperature and pressure radium is a solid metal.
What is the physical state of radium at STP?
At room temperature and pressure radium is a solid metal.
How many molecules are in 30 liters of methane (CH4) at STP?
At STP (standard temperature and pressure), 1 mole of any gas occupies 22.4 liters. So, in 30 liters of methane, there would be 30/22.4 = 1.3393 moles. One mole of methane contains 6.022 x 10^23 molecules, therefore 30 liters of methane at STP would contain 1.3393 * 6.022 x 10^23 = 8.07 x 10^23 molecules.
How many liters are in 5.4x1024 molecules of nitric oxide at STP?
Using the ideal gas law (PV = nRT), we can calculate the volume of gas at STP. First, we need to convert the number of molecules to moles by dividing by Avogadro's number. Then, we can use the volume of 1 mole of gas at STP, which is 22.4 liters. Calculate V = (5.4x10^24 / 6.022x10^23) * 22.4 to find the volume in liters.
How many hydrogen molecules are in 31.8 L H2(g) at STP?
To find the number of hydrogen molecules, first calculate the number of moles in 31.8 L of H2 at STP using the ideal gas law. Then use Avogadro's number (6.022 x 10^23 molecules/mol) to convert moles to molecules.
How many butane molecules are in 22.4 liters of C4H10 gas at STP?
There are 6.02 x 10^23 molecules in one mole of a substance (Avogadro's number). At STP, 22.4 liters of any ideal gas contains 1 mole of gas. Therefore, there are 6.02 x 10^23 butane molecules in 22.4 liters of C4H10 gas at STP.
How many nitrogen molecules are in 12 dm3 of nitrogen gas at room temperature?
There are approximately 1.35 x 10^24 nitrogen molecules in 12 dm^3 of nitrogen gas at room temperature, which is around 25°C. This calculation is based on Avogadro's Law, which states that at standard temperature and pressure (STP) one mole of any gas contains 6.022 x 10^23 molecules.
How many oxygen molecules are in 9.1 L of oxygen gas at STP?
at stp 1 mole of a gas contains 22.4 litres. 9.1/22.4= .40625 moles o2. 1 mole of a gas contains 6.022E23 molecules so .40625 moles x 6.022E23 = 2.4464325E23 molecules, but you have to multiply by two due to it being diatomic, so answer x 2 = 4.892875E23 molecules
How many molecules are in 7.3 L of H2 at STP?
At STP, 1 mole of any gas occupies 22.4 L. So, 7.3 L of H2 corresponds to 7.3/22.4 = 0.3263 mol. Since 1 mol of H2 contains 6.022 x 10^23 molecules, the number of molecules in 7.3 L of H2 at STP would be 0.3263 mol x 6.022 x 10^23 molecules/mol = 1.963 x 10^23 molecules.
How many molecules of ethane are present in 64.28 liters of ethane gas (C2H6) at STP?
at STP 1 mole occupies 22.4 litres. 64.28 / 22.4 is 2.8696428 moles. Multiply this by avagadro's constant (6.022*10^23) gives 1.7281x10^24 molecules
Which group 15 element exists as diatomic molecules at STP?
Nitrogen (N2) is the Group 15 element that exists as diatomic molecules at standard temperature and pressure (STP).
What is the average distance between oxygen molecules at Standard Temperature and Pressure (STP)?
The average distance between oxygen molecules at Standard Temperature and Pressure (STP) is approximately 3.3 nanometers.
What sample at STP has the same number of molecules as 5 liters of NO2 at STP?
At STP, 1 mole of any ideal gas occupies 22.4 liters. Therefore, 5 liters of NO2 at STP will represent 0.22 moles (5/22.4), and this is the case for any other ideal gas. So, the answer is that 5 liter of ANY ideal gas will have the same number of molecules as 5 liters of NO2.
Which two samples of gas at STP contain the same total number of molecules?
Two samples of gas at STP containing the same total number of molecules would have equal volumes, as Avogadro's Principle states that equal volumes of gases contain equal numbers of molecules at the same temperature and pressure. Thus, 1 mole of any gas at STP will have the same number of molecules as 1 mole of any other gas at STP.
