Temperature measures kinetic energy on a molecular level, and kinetic energy depends upon two things, speed and mass. So, if the temperature is a constant (since you have specified STP) the lighter the molecule is, the faster it will be moving. The lightest molecule, of course, is hydrogen. So hydrogen moves the fastest of any molecule at a given temperature.
The estimated value of the density of francium at STP is 1,87 g/cm3.
STP stands for Standard Temperature and Pressure. At STP, the pressure of natural gas is 1 atm, and 1 mole of gas takes up 22.4 liters.
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The pressure of a has at STP is 1 bar.
STP = Standard Temperature and Pressure After the IUPAC rules the standard temperature is 0 0C and the standard pressure is 100 kPa (0,986 atm). The molar volume of an ideal gas at STP is 22,710 980(38) L.
the symbol that represent molecule at stp is energy or force
Rms= sqrt(((3)(8.314)(273.15k))/(1g/mole)) = 82.54 is the speed of one hydrogen molecule. Assuming stp
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343 m/s
In 22.4 litres there are Avogadro's number of molecules. Divide one by the other to get liters per molecule.
10 to 1000 Mbps for less than +/- 100m
To determine how many atoms are present in 56 liters of oxygen gas at STP you first need to know that there are two atoms in a single molecule. Then, you would work the scientific formula to determine the number of molecules in the oxygen gas.
the answer is 8.45 molecules. Yay a 45th molecule. Weird huh.
If these atoms are loose unities, not bonded in a molecule, it would be about 22 dm3 at 0oC and standard pressure (STP). If the atoms would have formed gas molecules, e.g. CO2 or SF6, the answer would be different, because 6.02 x 1023 molecules always take in a volume of about 22 dm3 at STP. But with CO2 you would have then 18 x 1023 atoms because there are 3 atoms in one molecule.
Any gas at STP is 0 degrees Celsius and 1 ATM when at 22.414L.
We know that one mole of any gas at STP occupies 22.4 liters of volume. We also know that one mole of carbon dioxide is 44.01 grams of CO2. If there are 44.01 grams of this gas in 22.4 liters at STP, then there will be about 0.98 grams of CO2 in half a liter (500 ml) of the gas at STP.
To find it's density