A pressure cooker contains 5.68 liters of air at a temperature of 394 K. If the absolute pressure of the air in the pressure cooker is 205 pascals, how many moles of air are in the cooker? The cooker contains moles of air.

The question is incomplete. The value for the absolute pressure of air in the pressure cooker is 205 kilopascals I.e. 205, 000 pascals not 205 pascals.

The answer is n= 0.355 mol

Explanation:

The ideal gas equation will be used to solve this question. The ideal gas equation is:

PV=nRT

Where; P = absolute pressure

(atm)

V = Volume (Litres)

n = no. of moles

R = ideal gas constant

(0.0821 L atm/ mol K)

T = absolute temperature

(K)

According to this question, V= 5.68L, P= 205 Kpa, T= 394K

However, the unit of pressure must be converted to atm

1 atm = 101325pa

Hence, 205000 pa will be 205000/101325 atm

= 2.02 atm

Since, n in the equation PV=nRT is being sought for, we make "n" subject of the formula. Thus, n = PV/RT

n = 2.02 × 5.68 / 0.0821 × 394

n = 11.4736 / 32.3474

n = 0.355 mol

Thus, The pressure cooker contains 0.355 moles of air.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

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.