Predict the product(s) using a balanced equation and state whether the following

Question

1. Predict the product(s) using a balanced equation and state whether the following is a redox reaction:
   Phosphorus trichloride + chlorine => a. PCl3 + Cl => PCl4; redox reaction b. PCl3 + Cl2 => PCl5; redox reaction c. PCl3 + Cl2 => PCl5; not a redox reaction d. PCl3 + 2Cl => PCl5; redox reaction e. PCl3 + 2Cl => PCl5; not a redox reaction

Predict the product(s) using a balanced equation and state whether the following is a redox reaction:
Phosphorus trichloride + chlorine => a. PCl3 + Cl => PCl4; redox reaction b. PCl3 + Cl2 => PCl5; redox reaction c. PCl3 + Cl2 => PCl5; not a redox reaction d. PCl3 + 2Cl => PCl5; redox reaction e. PCl3 + 2Cl => PCl5; not a redox reaction Predict the product(s) using a balanced equation and state whether the following is a redox reaction:
Phosphorus trichloride + chlorine => PCl3 + Cl => PCl4; redox reaction PCl3 + Cl2 => PCl5; redox reaction PCl3 + Cl2 => PCl5; not a redox reaction PCl3 + 2Cl => PCl5; redox reaction PCl3 + 2Cl => PCl5; not a redox reaction a. PCl3 + Cl => PCl4; redox reaction b. PCl3 + Cl2 => PCl5; redox reaction c. PCl3 + Cl2 => PCl5; not a redox reaction d. PCl3 + 2Cl => PCl5; redox reaction e. PCl3 + 2Cl => PCl5; not a redox reaction

Explanation / Answer

The answer is:

b. PCl3 + Cl2 => PCl5; redox reaction


Note:

(1) chlorine exists as a molecule under standard conditions => Cl2

(2) Oxidation state of P increases from +3 (in PCl3) to +5 (in PCl5) while that of Cl decreases from 0 (in Cl2) to -1 (in PCl5) => redox reaction

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