Have a query? Ask a Tutor!!

Access to best educators and exclusive paper discussions

Can’t find what you’re looking for?

Our tutors are from top schools around the world, and they are waiting for you 24/7, anytime, anywhere.

Homework- One to One Solutions
Understand concepts to solve better
Get your doubts solved instantly

Chemistry-

General

Easy

Question

Metals are refined by using different methods. Which of the following metals are refined by electrolytic refining?
i)Ag
ii)Cu
iii)Na
iv)Al.

(i) , (ii) and (iv)
(i) and (iii)
(ii) and (iii)
(iii) and (iv)

The correct answer is: (i) , (ii) and (iv)

This method is used for Cu, Ag, Zn, Sn, Pb, Al, Ni and Cr

Related Questions to study

Galvanization is a method of protecting iron from rusting by coating with a thin layer of

Galvanization is a method of protecting iron from rusting by coating with a thin layer of

Chemistry-General

Corrosion or rusting can be prevented by

Corrosion or rusting can be prevented by

Chemistry-General

An element reacts with oxygen to give a compound with a high melting point. This compound is also soluble in water. The element is likely to be:

An element reacts with oxygen to give a compound with a high melting point. This compound is also soluble in water. The element is likely to be:

Chemistry-General

parallel

Which of the following metals is protected by a layer of its own oxide?

Which of the following metals is protected by a layer of its own oxide?

Chemistry-General

The correct decreasing order of the metals in the activity series is:

The correct decreasing order of the metals in the activity series is:

Chemistry-General

The order of reactivity with oxygen is in the order

The order of reactivity with oxygen is in the order

Chemistry-General

parallel

H₂SO₄ acts as dehydrating agent in its reaction with

H₂SO₄ acts as dehydrating agent in its reaction with

Chemistry-General

When an aluminium strip is kept immersed in freshly prepared ferrous sulphate solution taken in a test tube, the change observed is that

When an aluminium strip is kept immersed in freshly prepared ferrous sulphate solution taken in a test tube, the change observed is that

Chemistry-General

A student puts one big iron nail in four test tubes containing solutions of zinc sulphate, aluminium sulphate, copper sulphate and iron sulphate. A reddish brown coating was observed only on the surface of iron nail which was put in the solution of:

A student puts one big iron nail in four test tubes containing solutions of zinc sulphate, aluminium sulphate, copper sulphate and iron sulphate. A reddish brown coating was observed only on the surface of iron nail which was put in the solution of:

Chemistry-General

parallel

The correct order of decreasing reactivity of Zn, Cu, Fe and Al is:

The correct order of decreasing reactivity of Zn, Cu, Fe and Al is:

Chemistry-General

Generally non-metals are not lustrous. Which of the following non-metal is lustrous?

Generally non-metals are not lustrous. Which of the following non-metal is lustrous?

Chemistry-General

Statement–1: $P C l subscript 5 end subscript open parentheses g close parentheses rightwards harpoon over leftwards harpoon P C l subscript 3 end subscript open parentheses g close parentheses plus C l subscript 2 end subscript open parentheses g close parentheses$ . If more Cl₂ is added the equilibrium constant will decrease.
Statement–1 : Addition of inert gas to the equilibrium mixture at constant volume does not alter the equilibrium.

Statement–1: $P C l subscript 5 end subscript open parentheses g close parentheses rightwards harpoon over leftwards harpoon P C l subscript 3 end subscript open parentheses g close parentheses plus C l subscript 2 end subscript open parentheses g close parentheses$ . If more Cl₂ is added the equilibrium constant will decrease.
Statement–1 : Addition of inert gas to the equilibrium mixture at constant volume does not alter the equilibrium.

Chemistry-General

parallel

Statement–1: For $N subscript 2 end subscript open parentheses g close parentheses plus 3 H subscript 2 end subscript open parentheses g close parentheses rightwards harpoon over leftwards harpoon 2 N H subscript 3 end subscript open parentheses g close parentheses$ the equilibrium constant is ‘K’ then for $fraction numerator 1 over denominator 2 end fraction N subscript 2 end subscript open parentheses g close parentheses plus fraction numerator 3 over denominator 2 end fraction H subscript 2 end subscript open parentheses g close parentheses rightwards harpoon over leftwards harpoon N H subscript 3 end subscript open parentheses g close parentheses$ the equilibrium constant will be $square root of K$
Statement–2 : If concentration are changed to half the equilibrium constant will be halved.

Statement–1: For $N subscript 2 end subscript open parentheses g close parentheses plus 3 H subscript 2 end subscript open parentheses g close parentheses rightwards harpoon over leftwards harpoon 2 N H subscript 3 end subscript open parentheses g close parentheses$ the equilibrium constant is ‘K’ then for $fraction numerator 1 over denominator 2 end fraction N subscript 2 end subscript open parentheses g close parentheses plus fraction numerator 3 over denominator 2 end fraction H subscript 2 end subscript open parentheses g close parentheses rightwards harpoon over leftwards harpoon N H subscript 3 end subscript open parentheses g close parentheses$ the equilibrium constant will be $square root of K$
Statement–2 : If concentration are changed to half the equilibrium constant will be halved.

Chemistry-General

If the composition of the system does not change with time, the system is said to be in chemical equilibrium. It is the state in which net reaction of a system is zero. In another words we can say that in reversible reactions, a stage is reached when the rate of transformation of reactants into products equals to the rate of transformation of products into reactants. At this stage, the composition of reactants and products does not change with time. This does not mean that the reaction has ceased, as both reverse and forward reactions are still taking place but with equal rate. Such equilibria are called dynamic equilirbria.
Let us consider a reaction of the type
A (g) + B(g) $Error converting from MathML to accessible text.$ C(g) + D(g)
$Error converting from MathML to accessible text.$
where Kc is equilibrium constant which is equal to the ratio of the concentrations of the product to reactants
$Error converting from MathML to accessible text.$
where KP is the equilibrium constant which is equal to the ratio of partial pressure of products to reactants. The relation between KP and KC is as follows.
KP = Kc(RT)^Dⁿ
20.For the reaction
NH2COONH4(s) $Error converting from MathML to accessible text.$ 2 NH3(g) + CO2(g)
The equilibrium constant KP = 2.9 × 10-5 atm3. The total pressure of gases at equilibrium when mole of reactant was heated will be

If the composition of the system does not change with time, the system is said to be in chemical equilibrium. It is the state in which net reaction of a system is zero. In another words we can say that in reversible reactions, a stage is reached when the rate of transformation of reactants into products equals to the rate of transformation of products into reactants. At this stage, the composition of reactants and products does not change with time. This does not mean that the reaction has ceased, as both reverse and forward reactions are still taking place but with equal rate. Such equilibria are called dynamic equilirbria.
Let us consider a reaction of the type
A (g) + B(g) $Error converting from MathML to accessible text.$ C(g) + D(g)
$Error converting from MathML to accessible text.$
where Kc is equilibrium constant which is equal to the ratio of the concentrations of the product to reactants
$Error converting from MathML to accessible text.$
where KP is the equilibrium constant which is equal to the ratio of partial pressure of products to reactants. The relation between KP and KC is as follows.
KP = Kc(RT)^Dⁿ
20.For the reaction
NH2COONH4(s) $Error converting from MathML to accessible text.$ 2 NH3(g) + CO2(g)
The equilibrium constant KP = 2.9 × 10-5 atm3. The total pressure of gases at equilibrium when mole of reactant was heated will be

Chemistry-General

If the composition of the system does not change with time, the system is said to be in chemical equilibrium. It is the state in which net reaction of a system is zero. In another words we can say that in reversible reactions, a stage is reached when the rate of transformation of reactants into products equals to the rate of transformation of products into reactants. At this stage, the composition of reactants and products does not change with time. This does not mean that the reaction has ceased, as both reverse and forward reactions are still taking place but with equal rate. Such equilibria are called dynamic equilirbria.
Let us consider a reaction of the type
A (g) + B(g) $Error converting from MathML to accessible text.$ C(g) + D(g)
$Error converting from MathML to accessible text.$
where Kc is equilibrium constant which is equal to the ratio of the concentrations of the product to reactants
$Error converting from MathML to accessible text.$
where KP is the equilibrium constant which is equal to the ratio of partial pressure of products to reactants. The relation between KP and KC is as follows.
KP = Kc(RT)^Dⁿ
The equilibrium constant for the reaction 2 SO2(g) + O2(g) $Error converting from MathML to accessible text.$ 2 SO3(g) at 1000 K is 3.5. What would the partial pressure of oxygen gas if there are equal moles of SO2 and SO3 ?

If the composition of the system does not change with time, the system is said to be in chemical equilibrium. It is the state in which net reaction of a system is zero. In another words we can say that in reversible reactions, a stage is reached when the rate of transformation of reactants into products equals to the rate of transformation of products into reactants. At this stage, the composition of reactants and products does not change with time. This does not mean that the reaction has ceased, as both reverse and forward reactions are still taking place but with equal rate. Such equilibria are called dynamic equilirbria.
Let us consider a reaction of the type
A (g) + B(g) $Error converting from MathML to accessible text.$ C(g) + D(g)
$Error converting from MathML to accessible text.$
where Kc is equilibrium constant which is equal to the ratio of the concentrations of the product to reactants
$Error converting from MathML to accessible text.$
where KP is the equilibrium constant which is equal to the ratio of partial pressure of products to reactants. The relation between KP and KC is as follows.
KP = Kc(RT)^Dⁿ
The equilibrium constant for the reaction 2 SO2(g) + O2(g) $Error converting from MathML to accessible text.$ 2 SO3(g) at 1000 K is 3.5. What would the partial pressure of oxygen gas if there are equal moles of SO2 and SO3 ?

Chemistry-General

parallel

card img

With Turito Academy.

card img

With Turito Foundation.

card img

Get an Expert Advice From Turito.

Turito Academy

card img

With Turito Academy.

Test Prep

card img

With Turito Foundation.