When the pressure in a certain gas cylinder with a volume of 4.50 l reaches 500 atm, the cylinder is likely to explode. if this cylinder contains 40.0 moles of argon at 25.0oc is it on the verge of exploding?

The cylinder is nit on the verge of exploding.

Explanation:

Given:  

Temperature = 25.0 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (25.0 + 273.15) K = 298.15 K  

Volume = 4.50 L

Moles = 40.0 mol

Using ideal gas equation as:

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

P × 4.50 L = 40.0 mol × 0.0821 L.atm/K.mol × 298.15 K  

⇒P = 217.58 atm

Pressure limit = 500 atm

Hence, the cylinder is nit on the verge of exploding.

the answer to this question is 3.

it forms an anion that has a larger radius. anions have a negative charge and are larger than the original atom.