Help Calculate Chlorine Volume @STP: 2.99x10^23 molecules

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To calculate the volume occupied at standard temperature and pressure (STP) by 2.99 x 10^23 molecules of chlorine, the Ideal Gas Law can be applied, or a simpler ratio method can be used. At STP, one mole of an ideal gas occupies 22.4 liters, and one mole contains Avogadro's number of molecules, approximately 6.02 x 10^23. By using the ratio of the number of molecules to Avogadro's number, the volume can be determined. Specifically, the calculation involves multiplying 22.4 liters by the ratio of 2.99 x 10^23 to 6.02 x 10^23, which yields the volume of chlorine gas at STP.
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Can someone please calculate the volume occupied at STP by 2.99times10 to the 23rd power molecules of Chlorine. Thank you Very much.
 
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All gases have a specific size at STP. I think it's 22.4L IIRC. Just multiply 22.4 * (2.99 * 10^23) / (avogadro's number)
 
ShawnD said:
All gases have a specific size at STP. I think it's 22.4L IIRC. Just multiply 22.4 * (2.99 * 10^23) / (avogadro's number)

avogadro's number = 6.02*10^23

incase you didn't know
 
1. Use the Ideal Gas Law, PV =nRT, with n= \frac {2.99*10^{23}} {6.02*10^{23}}, to find V. You know, P, T, R, n.

OR

2. At STP, one mole of an ideal gas occupies 22.4 liters. One mole has 6.02*10^23 molecules. Use ratios to find the volume of 2.99*10^23 molecules.
 

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