NO2 has a higher boiling point than CO2 because the nitrogen radii is larger than carbon. The bigger the atom the more intermolecular force that is created...this requires more energy to break causing a higher boiling point.
Sulfur is larger and therefore has a larger intermolecular force than oxygen. Intermolecular force increases the amount of energy needed to break the bonds, and increases the boiling point.
CO HAS A HIGHE BOILING POINT BECAUSE THE INTEMOLECULAR FORCES ARE STRONGER THEN N2 WHICH IS NON POLAR.
Boiling points:
CO: −191.50 °C
O2: −182.95 °C so this is higher!
CO is a polar (charge asymetric) molecule, N2 is symetrical and therefore non-polar
NO will have a slight dipole and N2 does not. Thus, the intermolecular forces between NO molecules is stronger than those between N2 molecules.
CO has greater intermolecular forces holding the CO molecules together than does N2, so it has a higher boiling point.
N2 would have the lowest BP because it has the weakest intermolecular forces.
The boiling point in degree Celsius are given below:Na: 883K: 774Si: 2355Ne: -246Silicon has the highest boiling point among the elements given.
Hydrogen is produced by reacting methane (CH4(g),(natural gas)) with steam (H2O(g)), producing carbon dioxide (CO2(g)) and hydrogen (H2(g)). Nitrogen (N2(g)) is obtained by the fractional distillation of air (~78% N2(g)). Fractional distillation is a process by which the components in a chemical mixture are separated according to their different boiling points. Vapours from a boiling solution are passed along a cooled column. The temperature of the column gradually decreases along its length. Components with a higher boiling point condense on the column and return to the solution; components with a lower boiling point pass through the column, are condensed, and are collected in a suitable collecting vessel.
H2
Co+ , ch4+ , n2+ ,c2h6 etc are example of molecular ion.
N2 would have the lowest BP because it has the weakest intermolecular forces.
Yes, nitrogen exists in a gaseous form (N2) at at temperatures above its boiling point. It can also exist as a liquid at 77 K.
To lower the amount of harmful emissions in the exhaust. It converts HC, CO and NOx into H20, CO2, and N2.
The boiling point in degree Celsius are given below:Na: 883K: 774Si: 2355Ne: -246Silicon has the highest boiling point among the elements given.
Nitrogen boiling point at Standard Pressure (1 atm) is 77.355 K (−195.795 °C or −320.431 °F)
CO
Nitrogen is a colourless gas at room temperature due to the weak intermolecular bonds between the diatomic molecules N2. Its boiling point is -195.7 C and has a melting point of -210.0 C.
N2, H2, H2O, H2S and CO
Hydrogen is produced by reacting methane (CH4(g),(natural gas)) with steam (H2O(g)), producing carbon dioxide (CO2(g)) and hydrogen (H2(g)). Nitrogen (N2(g)) is obtained by the fractional distillation of air (~78% N2(g)). Fractional distillation is a process by which the components in a chemical mixture are separated according to their different boiling points. Vapours from a boiling solution are passed along a cooled column. The temperature of the column gradually decreases along its length. Components with a higher boiling point condense on the column and return to the solution; components with a lower boiling point pass through the column, are condensed, and are collected in a suitable collecting vessel.
It will depend on atmospheric pressure. You can use the Clausius-Clapeyron equation In this form ln (P2/P1) =( or approximately equals )= -ΔHm ( 1/T2 - 1/T1 )/R The normal bp of N2 is 77.4 K at 760 Torr, ΔHm for N2 is 5.58 kJ/mol, R is 8.314 J/mol.K. Plug in above constants, and you can supply your own temp or pressure into T1 or P1 and solve for the other. Make sure you get your units right! I leave it up to you to work them out. This only works for ideal gases close to the normal boiling point.
There are 6.023x10^23 molecules in one mole of a compound. So now, you have to find how many moles of each compound you have. CO's molecular weight is (12+16) = 28 g/mol N2's molecular weight is (14+14) = 28 g/mol So you find the moles of each. moles of N2 = 20g/ 28g/mol = .714 moles moles of CO = 16g / 28 g/mol = .571 moles So, N2 has (.714 *6.023x10^23) has 4.3 x10^23 molecules and CO (.571 *6.023x10^23) has 3.4x10^23 molecules. So, 20g of N2 has more molecules than 16g of CO
H2