If i have 4 moles of a gas ata pressure of 5.2 atm and a volume of 15 liters, what is the temperature?

273.51 K

Explanation:

The Ideal gas law given by the combination of Boyle's law, Charles's law, Avogadro's law, and Gay-Lussac's law is given as follows:-

PV=nRT

Where,

P =   the pressure of the gas

V  =  the volume it occupies

n  = the number of moles of gas present in the sample

R =  the universal gas constant, equal to  0.0821  atm L /mol K

T  = the absolute temperature of the gas

∴ T = PV/nR = 5.2 *15/0.0821 * 4 = 273.5 K

explanation:

the largest database of organic compounds lists about 10 million substances, which include compounds originating from living organisms and those synthesized by chemists. the number of potential organic compounds has been estimated at 1060—an astronomically high number. the existence of so many organic molecules is a consequence of the ability of carbon atoms to form up to four strong bonds to other carbon atoms, resulting in chains and rings of many different sizes, shapes, and complexities. the simplest organic compounds contain only the elements carbon and hydrogen, and are called hydrocarbons. even though they are composed of only two types of atoms, there is a wide variety of hydrocarbons because they may consist of varying lengths of chains, branched chains, and rings of carbon atoms, or combinations of these structures. in addition, hydrocarbons may differ in the types of carbon-carbon bonds present in their molecules. many hydrocarbons are found in plants, animals, and their fossils; other hydrocarbons have been prepared in the laboratory. we use hydrocarbons every day, mainly as fuels, such as natural gas, acetylene, propane, butane, and the principal components of gasoline, diesel fuel, and heating oil. the familiar plastics polyethylene, polypropylene, and polystyrene are also hydrocarbons. we can distinguish several types of hydrocarbons by differences in the bonding between carbon atoms. this leads to differences in geometries and in the hybridization of the carbon orbitals.