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

The cylinder is nit on the verge of exploding.

Explanation:

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:

PV  = nRT

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 Latm/ K. mol x 298.15 K

⇔ P= 217.58 atm

Pressure limit = 500 atm .

sorry idk the answer well to you i have a explaination

explanation: a formula which shows the arrangement of atoms in the molecule of a compound

the volume increases