A sample of silver with a mass of 88.3 g is heated to a temperature of 100.°C and placed in a calorimeter of water at 22.0° The final temperature of the silver and water is 26.3°C.
Assuming no heat loss, what mass of water was in the container? The specific heat of water
is 4.184 J/gºC and of silver 0.240 J/gºC.
Round to proper sig figs
mwater=___g

The reaction will shift to the right

Sorry i dont understand the question can you rephase it?

Sorry i dont understand the question can you rephase it?

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.