How many molecules are there in an ideal gas with a volume of 8.59 L at...
How many molecules are there in an ideal gas with a volume of 8.59 L at STP?
number of molecules:
(I did 8.59*1mol/22.4L=0.3843, but when I enter it in my homework it says its wrong and tells me after finding the mols of the gas I need to calculate the number of molecules from avogadros number... plz help
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How many molecules are there in an ideal gas with a volume of
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How many molecules are there in an ideal gas with a volume of 3.97 L at STP?
QUESTION 16 One mole of gas at STP will take up what volume of space? 100...
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Imagine that you have an ideal gas in a 6.90 L container, and that 1350 molecules...
Imagine that you have an ideal gas in a 6.90 L container, and that 1350 molecules of this gas collide with a square-inch area of the container at any given instant. If the volume is increased to 55.2 L at constant temperature, how many collisions will occur per square inch of this larger container? Enter the number of collisions per square inch.
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An ideal gas has a pressure of 1.534 atm, a volume of 29.634 L at a temperature of 37.569 oC. How many molecules are there in the gas?
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1. (a) How many molecules are present in a sample of an ideal gas that occupies a volume of 2.10 cm3, is at a temperature of 20°C, and is at atmospheric pressure? (b) How many molecules of the gas are present if the volume and temperature are the same as in part (a), but the pressure is now 3.00 ✕ 10−11 Pa (an extremely good vacuum)? 2. An air bubble released by a submersible vehicle, 120 m below the surface...
How many grams of Al are in 1.38 * 1023 molecules of Al2O3 if the atomic...
How many grams of Al are in 1.38 * 1023 molecules of Al2O3 if the atomic mass of Al is 27.0 g/mole, O is 16.0 g/mole, and Al2O3 is 102.0 g/mole (the final answer should have the correct number of significant figures)? Here is my work: (1.38*10^23 molecules) (1mol / 6.022*10^23 molecules) (27.0 gram/ mol)= 6.1873 I counted 3 Sig Fig so I rounded my answer to 6.19.... Another thought was (1.38*10^23 molecules) (54grams /1 mol) (1mol/6.022*10^23) but that answer...
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The ideal gas law relates the temperature, pressure and volume of an ideal gas. Suppose the gas inside a particular balloon has an absolute pressure of 3.15×105 Pa and occupies a volume of 5.33×10-3 m3 at a temperature of 16.7°C. How many moles of gas are inside the balloon? (do not enter units) How many molecules of gas are inside the balloon? (do not enter units)
Using the Ideal Gas Law, what volume in L would 1 mole of an ideal gas occupy at standard temperature and pressure? Reme...
Using the Ideal Gas Law, what volume in L would 1 mole of an ideal gas occupy at standard temperature and pressure? Remember: STP is 273.15 K and 101.325 kPa.
Imagine that you have an ideal gas in a 4.70 L container, and that 2750 molecules...
Imagine that you have an ideal gas in a 4.70 L container, and that 2750 molecules of this gas collide with a square-inch area of the container at any given instant. If the volume is increased to 18.8 L at constant temperature, how many collisions will occur per square inch of this larger container?
Based on the ideal gas law, there is a simple equivalency that exists between the amount...
Based on the ideal gas law, there is a simple equivalency that exists between the amount of gas and the volume it occupies. At standard temperature and pressure (STP; 273.15 K and 1 atm, respectively), one mole of gas occupies 22.4 L of volume. What mass of methanol (CH3OH) could you form if you reacted 4.24 L of a gas mixture (at STP) that contains an equal number of carbon monoxide (CO) and hydrogen gas (H2) molecules?
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