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.
Among the options provided, nitrogen gas (N2) should have the lowest boiling point. Nitrogen is a diatomic molecule with weak van der Waals forces between its molecules, leading to a relatively low boiling point compared to ammonia (NH3), hydrogen fluoride (HF), water (H2O), and sodium sulfide (Na2S) which have stronger intermolecular forces due to hydrogen bonding or ionic interactions.
The boiling point in degree Celsius are given below:Na: 883K: 774Si: 2355Ne: -246Silicon has the highest boiling point among the elements given.
In liquid ammonia one hydrogen atom from an adjacent molecule can form an intermolecular hydrogen bond with the nitrogen atom of the central ammonia molecule. With an average of only one intermolecular bond per ammonia molecule, less thermal energy is required to break the liquid ammonia into individual gas phase molecules. Therefore a lower boiling temperature results. In the case of liquid water, one hydrogen atom from each of two adjacent water molecules can form an intermolecular hydrogen bond with each lone pair on the oxygen atom of the central water molecule. As such, a greater amount of thermal energy is required to break the extensive hydrogen bonding network and a higher boiling temperature results.
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.
1/2 n2 + 3/2 h2 = nh3 sorry about the lower case they wouldn't let me summit it with caps N2 + 3 H2 => 2 NH3
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.
Among the options provided, nitrogen gas (N2) should have the lowest boiling point. Nitrogen is a diatomic molecule with weak van der Waals forces between its molecules, leading to a relatively low boiling point compared to ammonia (NH3), hydrogen fluoride (HF), water (H2O), and sodium sulfide (Na2S) which have stronger intermolecular forces due to hydrogen bonding or ionic interactions.
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
a) O2 would have a higher boiling point than N2 since it experiences London dispersion forces in addition to its higher molecular weight. b) SO2 would have a higher boiling point than CO2 due to its ability to form stronger dipole-dipole interactions and London dispersion forces. c) HF would have a higher boiling point than HI due to hydrogen bonding, which is stronger than the dipole-dipole interactions present in HI.
The freezing point of a substance with a molecular weight of N2 is -210.01 degrees Celsius.
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