Me.

a 60 l cylinder is filled with argon gas to a pressure of 10130.0 kpa at 200°c. how many moles of argon gas does the cylinder contain? (given: r = 8.314 l∙kpa/k∙mol)

To simplify, we need to assume that the gas is an ideal gas so we can use the equation PV=nRT where P is pressure, V is volume, n is the number of moles, R is the universal gas constant and T is the temperature. We can calculate as follows:
PV = nRT
n = PV / RT
n = 10130(60) / 8.314 (200+273.15)
n = 154.51 mol argon gas

Ithink it’s 3 as the answer.

Answerthe half-reaction having the greatest tendency to occur at the anode:     i₂(aq) + 2e⁻  ⇄ 2i⁻  ;   e = +0.53 v======oxidation occurs at the anode. we must therefore find the half-reaction with the greatest tendency to oxidize.the given values of e are reduction potentials (the form of the half-reactions are of reduction).the lower the reduction potential, the higher the potential to oxidize. the half-cell with the lowest reduction potential will have the greatest tendency to oxidize at the anode.the half-reaction having the greatest tendency must be    i₂(aq) + 2e⁻  ⇄ 2i⁻    e = +0.53 vbecause its reduction potential is the lowest out of the three.