The following information was obtained when carrying out an experiment to determine the enthalpy (δh) of neutralization reaction between hcl and naoh. 100 ml of 2.00 m hcl solution was added to 95.00 ml of 2.00 m solution of naoh. the final temperature reached was 35.40 °c and the initial temperature at mixing was 22.15 °c. the density of the mixture was 1.04 g/ml and its specific heat capacity was 3.89 j/g-°c. how many moles of hcl were used to neutralize the naoh in the reaction?

The correct answer should be "electrons orbit the nucleus in circular motions exactly as shown on the classic bohr model."

257 grams h2o i think

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.