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STATEMENT 1 when a copper wire is placed...

STATEMENT 1 when a copper wire is placed in a solution of `AgNO_(3)` the solution blue colour and
STATEMENT 2 `E_(RP)^(@) "of" Cu^(+2)//Cu` is lesser than `E_(Ag^(+)//Ag)^(@)`

A

Statement 1 is ture , Statement 2 is true Statement 2 is correct explanation for Statement 6

B

Statement 1 is true Statement 2 is ture Statement 2 is NOT a correct explantion for Statement 6

C

Statement 1 is true statement 2 is ture

D

Statement 1 is false Statement 2 is true

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The correct Answer is:
A
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When a copper wire is placed in a solution of AgNO_(3) , the solution acquires blue colour. This is due to

(a) When a bright silver object is placed in the solution of gold chloride, it acquires a golden tings but nothing happens when it is placed in solution of copper chloride. Explain this behaviour of silver. [Given : E_(Cu^(2+//)Cu)^(@)=+0.34 V, E_(Ag^(+//)Ag)^(@) =+0.80 V, E_(Au^(3+//)Au)^(@) =+1.40V ] (b) Consider the figure given above and answer the following questions : (i) What is the direction of flow of electrons? (ii) Which is anode and which is cathode? (iii) What will happen if the salt bridge is removed ? (iv) How will concentration of Zn^(2+) and Ag^(+) ions be affected when the cell functions ? (v) How will concentration of these ions be affected when the cell becomes dead ?

STATEMENT - 1 : A dark blue colour is obtained on adding excess of dilute NH_(4)OH solution in aqueous soluiton of copper sulphate. and STATEMENT - 2 : Dark blue colour is due to the formation of [Cu(NH_(3))_(4)]^(2+) complex ion.

Can a solution of 1 M ZnSO_(4) be stored in a vessel made of copper ? Given that E_(Zn^(+2)//Zn)^(@) =-0.76V and E_(Cu^(+2)//Cu)^(@)=0.34 V

Can we use a copper vessel to store 1 M AgNO_(3) solution? Given E_(Cu^(2+)//Cu)^(Theta)=0.34V" "E_(Ag^(+)//Ag)^(Theta)=0.80

When CU reacts with AgNO_(3) solution , the reaction takes place is f:

STATEMENT-1: Copper is dissolved at anode and deposited at cathode when Cu electrodes are used and electrolyte is 1 M CuSO_4 (aq) solution. STATEMENT-2: SOP of Cu is less than SOP of water and SRP of Cu is greater than SRP of water.

Why blue colour of CuSO_(4) solution gets discharged when zinc rod is dipped in it ? Given, E_(Cu^(+2)//Cu)^(@)=0.34 V and E_(Zn^(+2)//Zn)^(@)=-0.76V

A: Copper rod turns colourless solution of zinc sulphate to blue. R: Zinc reduce Cu^(2+) " ions to " Cu^(+)

Is it possible to store: (i) Copper sulphate solution in a zinc vessel? (ii) Copper sulphate solution in a silver vessel? (iii) Copper sulphate solution in a gold vessel? Given: E_(Cu^(2+)| Cu )^(0) = + 0.34 volt and E_(Ag^(2+)| Ag )^(0) = 0.80 volt and E_(Au^(2+)| Au )^(0) = +1.50 volt