How many grams of O2 must be placed in a 3.33 liter container in order to exert a pressure of 2.46 atm at 27°C?

10.656 g

Explanation:

Given data:

Mass of oxygen = ?

Volume of container = 3.33 L

Pressure of gas = 2.46 atm

Temperature = 27°C

Solution:

The given problem will be solve by using general gas equation,

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

Now we will convert the temperature.

27+273 = 300 K

Now we will put the values in formula.

n = PV/RT

n = 2.46 atm × 3.33 L /  0.0821 atm.L/ mol.K   × 300 K

n = 8.192 atm. L /24.63 atm.L/ mol

n = 0.333 mol

Mass in grams:

Mass = number of moles × molar mass

Mass = 0.333 mol × 32 g/mol

Mass = 10.656 g

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.