Reducing Natu...

Reducing Nature (Group 2)

Trending Questions

Define metals and non-metals based on electron loss or gain.

Q. On electrolysis of aqueous sodium sulphate using platinum electrodes, the product formed at cathode and anode are respectively:

$H_{2}, O_{2}$
$N a, S O_{2}$
$N a, O_{2}$
$O_{2}, S O_{2}$

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Q. Which of the following statements is not true regarding alkali metals

The alkali metals have high chemical reactivity
The alkali metals exhibit only +1 oxidation state
The alkali metals die slove in liquid ammonia to give blue coloured solutions
Since the alkali metals have good tendency to lose s – electron, they behave as strong oxidizing agents

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A metal gives two chlorides ‘A’ and ‘B’. ‘A’ gives black precipitate with $N H_{4} O H$ and ‘B’ gives white. With KI ‘B’ gives a red precipitate soluble in excess of $K I$ . ‘A’ and ‘B’ are respectively :

$H g C l_{2}$ and $H g_{2} C l_{2}$
None of these
$H g_{2} C l_{2}$ and $H g C l_{2}$
$H g C l_{2}$ and $H g C l$

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Consider the cell:

Z n | Z n^{2 +} (a q) (1.0 M) | | C u^{2 +} (a q) (1.0 M) | | C u

The standard reduction potential are

0.350

V for

C u^{2 +} (a q) + 2 e^{-} \to C u

and

- 0.763

V for

Z n^{2 +} (a q) + 2 e^{-} \to Z n

The cell reaction is:

$Z n + C u^{3 +} \to Z n^{+} + C u^{2 +}$
$Z n^{2 +} + C u^{3 +} \to Z n^{2 +} + C u^{2 +}$
$Z n + C u^{+} \to Z n^{2 +} + C u$
$Z n + C u^{2 +} \to Z n^{2 +} + C u$

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Q. A substance that reacts with water to produce marsh gas (methane) is:

$C a C_{2}$
$A l_{4} C_{3}$
none of these
$A l_{2} C_{3}$

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Q. Given a reaction:

4 N H_{3} (g) + 5 O_{2} (g) \to 4 N O (g) + 6 H_{2} O (g)

When

1

mole of ammonia and

1

mole of

O_{2}

are made to react to completion :

$1.0$ mole of $H_{2} O$ is produced
$1.0$ mole of $N O$ will be produced
all the oxygen will be consumed
all the ammonia will be consumed

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Q. Magnesium ribbon burns in an atmosphere of both nitrogen and

N_{2} O

. Explain.

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B e

is placed above

M g

in the second group.

B e

dust, therefore when added to

M g C l_{2}

solution will

have no effect
lead to dissolution of Be
precipitate Mg metal
precipitate MgO

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Q. Oxygen and hydrogen gas are produced at the anode and cathode respectively, during the electrolysis of fairly concentrated aqueous solution of:

$A g N O_{3}$
$H_{2} S O_{4}$
$K_{2} S O_{4}$
$N a O H$

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Q. Mg burns in

C O_{2}

to form

MgO +C
MgO + CO
Mgo

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Q. Which of the following has no reaction with water?

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Q. (A) + dil.

H_{2} S O_{4} △ ⟶ g a s

(B). Gas (B) turns

K_{2} C r_{2} O_{7} / H^{+}

solution green.
Aqueous solution of (A) +

B a C l_{2} ⟶ w h i t e p p t (C)

Filtrate after removing (C) +

B r_{2}

water

⟶ w h i t e p p t (C)

. Here (A), (B) and (C) are
(A)

S O_{3}^{2 -} + S O_{4}^{2 -}

(B)

S O_{2}

and (C)

B a S O_{4}

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Q. A solution of sodium sulphate in water is electrolysed using inert electrodes. The products at the cathode and anode are respectively
(IIT-JEE, 1987)

$H_{2}, O_{2}$
$O_{2}, H_{2}$
$O_{2}, N a$
$O_{2}, S O_{3}$

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Q. Magnesium burns in air to give:

$M g O$ and $M g N$
$M g O_{2}$ and $M g_{3} N_{2}$
$M g O$ and $M g_{3} N_{2}$
$M g_{2} O$ and $M g_{3} N_{2}$

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Q. How much thermal energy released when 36.0 g of Al reacts with excess of

F e_{2} O_{3}

568 kJ
639 kJ
$1.14 \times 10^{3} k J$
$1.27 \times 10^{3} k J$

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Why Zinc oxide can be reduced to metal by heating with carbon but chromium oxide cannot be reduced by heating with carbon

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Q. Which of one of the following burns in the air giving a gaseous oxide? (at room temp.)

Sodium
Helium
Hydrogen
Sulphur

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Metals are good because they are electron .

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WEAK REDUCTANT(in aqs solution)alkali metal is what

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Q. When magnesium burns in air, it forms both an oxide and nitride.
If true enter 1, else enter 0.

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Q. In the electrolysis of aqueous sodium chloride solution which of the half-cell reaction will occur at the anode?

$N a_{(a q)}^{+} + e^{-} \to N a_{(s)}; E_{c e l l}^{o} = - 2.71$ V
$2 H_{2} O_{(l)} \to O_{2 (g)} + 4 H_{(a q)}^{+} + 4 e^{-}; E_{c e l l}^{o} = 1.23$ V
$H_{a q}^{+} + e^{-} \to \frac{1}{2} H_{2 (g)}; E_{c e l l}^{o} = 0.00$ V
$C l_{(a q)}^{-} \to \frac{1}{2} C l_{2 (g)} + e^{-}; E_{c e l l}^{o} = 1.36$ V

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Q. The electrode potential of oxidation half-cell is:

decreases with decreased concentration of ions in the cells
none of these
decreases with increased concentration of ions in the cells
is independent of the concentration of ions in the cell

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Q. Assertion :Alkali metals dissolve in liquid ammonia to give deep blue colour. Reason: Blue colour of the solution is due to the formation of ammoniated electron

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
Assertion is correct but Reason is incorrect
Both Assertion and Reason are incorrect

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