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Chemistry-

General

Easy

Question

Which favours the backward reaction in a chemical equilibrium?

Increasing the concentration of one of the reactants
Removal of at least one of the products at regular intervals
Increasing the concentration of one or more of the products
None of the above

The correct answer is: Increasing the concentration of one or more of the products

An increase in the concentration of products always brings in backward reaction.

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In $K subscript p end subscript equals K subscript c end subscript open square brackets R T close square brackets to the power of increment n end exponent comma increment n$ may have:

In $K subscript p end subscript equals K subscript c end subscript open square brackets R T close square brackets to the power of increment n end exponent comma increment n$ may have:

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The $left square bracket H to the power of plus end exponent right square bracket$ ion concentration in $0.001 blank M$ acetic acid is $1.34 cross times 10 to the power of negative 4 end exponent g blank i o n divided by l i t r e.$ The $open square brackets H to the power of plus end exponent close square brackets$ ion concentration of $0.164 g blank o f blank C H subscript 3 end subscript C O O N a$ is added to a $l i t r e$ of $0.001 blank M C H subscript 3 end subscript C O O H$ will be:

The $left square bracket H to the power of plus end exponent right square bracket$ ion concentration in $0.001 blank M$ acetic acid is $1.34 cross times 10 to the power of negative 4 end exponent g blank i o n divided by l i t r e.$ The $open square brackets H to the power of plus end exponent close square brackets$ ion concentration of $0.164 g blank o f blank C H subscript 3 end subscript C O O N a$ is added to a $l i t r e$ of $0.001 blank M C H subscript 3 end subscript C O O H$ will be:

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Which of the following is a buffer?

Which of the following is a buffer?

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$M g to the power of 2 plus end exponent$ is … than $A l to the power of 3 plus end exponent$ .

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The equilibrium constant $K subscript c end subscript$ for $A open parentheses g close parentheses rightwards harpoon over leftwards harpoon B open parentheses g close parentheses$ is 1.1, Gas $B$ will have molar concentration greater than 1 if :

The equilibrium constant $K subscript c end subscript$ for $A open parentheses g close parentheses rightwards harpoon over leftwards harpoon B open parentheses g close parentheses$ is 1.1, Gas $B$ will have molar concentration greater than 1 if :

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The solubility product of $B a S O subscript 4 end subscript$ is $1.5 cross times 10 to the power of negative 9 end exponent$ . The precipitation in a 0.01 M $B a to the power of 2 plus end exponent$ solution will start, on adding $H subscript 2 end subscript S O subscript 4 end subscript$ of concentration

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An aqueous solution contains $N i to the power of 2 plus end exponent comma C o to the power of 2 plus end exponent blank a n d blank P b to the power of 2 plus end exponent$ ions at equal concentrations. The solubility product of $N i S comma P b S blank a n d blank C o S$ in water at $25 ℃$ are $1.4 cross times 10 to the power of negative 24 end exponent comma 3.4 cross times 10 to the power of negative 28 end exponent a n d blank 3 cross times 10 to the power of negative 26 end exponent$ , respectively. Indicate which of these ions will be precipitated first and last when sulphide concentration is progressively increased from zero?

An aqueous solution contains $N i to the power of 2 plus end exponent comma C o to the power of 2 plus end exponent blank a n d blank P b to the power of 2 plus end exponent$ ions at equal concentrations. The solubility product of $N i S comma P b S blank a n d blank C o S$ in water at $25 ℃$ are $1.4 cross times 10 to the power of negative 24 end exponent comma 3.4 cross times 10 to the power of negative 28 end exponent a n d blank 3 cross times 10 to the power of negative 26 end exponent$ , respectively. Indicate which of these ions will be precipitated first and last when sulphide concentration is progressively increased from zero?

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0.005 M acid solution has 5 pH. The percentage ionisation of acid is

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At 90 $℃$ , pure water has $H subscript 3 end subscript O to the power of plus end exponent$ ion concentration of $10 to the power of negative 6 end exponent m o l divided by L to the power of negative 1 end exponent$ . The $K subscript w end subscript a t blank 90 ℃$ is

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Final pressure is higher than initial pressure of a container filled with an ideal gas at constant temperature. What will be the value of equilibrium constant?

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The reaction, $2 S O subscript 2 end subscript open parentheses g close parentheses plus O subscript 2 end subscript left parenthesis g right parenthesis rightwards harpoon over leftwards harpoon 2 S O subscript 3 end subscript left parenthesis g right parenthesis$ is carried out in a $1 blank d m to the power of 3 end exponent$ vessel and $2 blank d m to the power of 3 end exponent$ vessel respectively. The ratio of the reaction velocities will be

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In which of the following reactions is $K subscript p end subscript less than K subscript c end subscript$ ?

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What mole of $C a open parentheses O H close parentheses subscript 2 end subscript$ is dissolved in 250 mL aqueous solution to given a solution of $p H$ 10.65, assuming full dissociation?

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