Home
Class 12
CHEMISTRY
Cl(2) and F(2) are added to a solution c...

`Cl_(2)` and `F_(2)` are added to a solution containing `1M` each M of `Cl^(c-)` and `Br^(c-)` . What reaction will occur ?

Text Solution

AI Generated Solution

To solve the problem of what reactions occur when \( Cl_2 \) and \( F_2 \) are added to a solution containing \( 1M \) each of \( Cl^- \) and \( Br^- \), we will follow these steps: ### Step 1: Identify the species present In the solution, we have: - Chloride ions (\( Cl^- \)) - Bromide ions (\( Br^- \)) - Chlorine gas (\( Cl_2 \)) - Fluorine gas (\( F_2 \)) ...
Promotional Banner

Topper's Solved these Questions

  • NCERT BASED EXERCISE

    CENGAGE CHEMISTRY ENGLISH|Exercise Short Answer Type Questions(Electrochmical Cell)|12 Videos

  • NCERT BASED EXERCISE

    CENGAGE CHEMISTRY ENGLISH|Exercise Electrolysis, Batteries , and Rusting|20 Videos

  • NCERT BASED EXERCISE

    CENGAGE CHEMISTRY ENGLISH|Exercise NCERT Exercise|104 Videos

  • GRIGNARD REAGENTS AND ORGANOMETALLIC REAGENTS

    CENGAGE CHEMISTRY ENGLISH|Exercise Exercises Archives (Linked Comprehension)|1 Videos

  • NUCLEAR CHEMISTRY

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|13 Videos

Similar Questions

Explore conceptually related problems

Cl_(2) and Br_(c-) are added to a solution containing 1M each of Cl^(c-) and Br^(c-) . What reaction will occur ?

Br_(2) and I_(2) are added to a solution containing 1M each of Br^(c-) and I^(c-) . What reaction will occur ?

I2 and Br2 are added to a solution containing Br– and I– ions. What reaction will occur if, I_(2) + 2e^(-) rarr 2I^(-) , E^(0) = + 0.54V and Br_(2) + 2e^(-) rarr 2Br^(-) , E^(0) = +1.09 V?

When chlorine (Cl_(2)) water in excess is added to a salt solution containing chloroform, chloroform layer turns pale yellow.Salt contains:

C_(2)F_(3)Cl_(3) is named as :-

If in solution containing Cl^(-) & Br^(-) ions, AgNO_(3) is added then initial precipitate of which colour will be formed ?

Write the reactions of F_(2) and Cl_(2) with water.

In 500 ml capacity vessel CO and Cl_(2) are mixed to form COCl_(2) . At equilibrium, it contains 0.2 moles of COCl_(2) and 0.1 mole of each of CO and Cl_(2) , The equilibrium constant K_(C) for the reaction CO(g)+Cl(g)hArrCOCl_(2)(g) is

PCl_(5),PCl_(3)andCl_(2) are at equilibrium at 500 K with concentration 2.1 M PCl_(3) , 2.1 M Cl_(2) and 1.9 M PCl_(5) . The equilibrium constant for the given reaction is PCl_(5(g))hArrPCl_(3(g))+Cl_(2(g))

Silver ions are added to a solution with [Br^(-)]=[Cl^(-)]=[CO_(3)^(2-)]=[AsO_(4)^(3-)] =0.1M. Which compound will precipitate with lowest [Ag^(+)] ?