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pH the Power of H

100 ml of 3 m...

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100 ml of 3 mol H2SO4 reacts with 100 ml of 2 NaOH. Enthalpy of neutralisation of reaction is- (1) - 57.1 kJ/mol (2) - 2 * 57.1 kJ/mol (3) - 0.3 * 57.1 kJ/mol (4) - 3 * 57.1 kj/mol (Explain with concept of n-factor and equivalent weight)

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H C l + N a O H ⟶ N a C l + H_{2} O; Δ H = - 57.1 k J m o l^{- 1}

Δ H

is the heat of neutralisation of

H C l

N a O H

solution.If true enter 1 else o

Q. The amount of energy released when 20 ml of 0.5 M NaOH are mixed with 100 ml of 0.1 M HCl is x kJ. The heat of neutralisation (in kJ

m o l^{- 1}

Q. The amount of energy released when

20 m L

0.5 M N a O H

100 m L

0.1 M H C l

x k J

. The heat of neutralisation is : (in

k J m o l^{- 1}

)

A B

A_{2}

B_{2}

are diatomic molecules. If the bond enthalpies of

A_{2}, A B

B_{2}

are in the ratio 1 : 1 : 0.5 respectively and enthalpy of formation of

A B

A_{2}

B_{2}

- 100 {kJ/mol}^{- 1}

. What is the bond enthalpy of

A_{2}

Q. 100 ml 0.5 N

H_{2} S O_{4}

(strong acid) is neutralised with 200 ml 0.2 M

N H_{4} O H

in a constant pressure calorimeter which results in temperature rise of

1.4^{o} C

. If heat capacity of calorimeter content is

1.5 k J /^{o} C

. Which of the following statements is/are correct?
Given:

H C l + N a O H \to N a C l + H_{2} O + 57 k J

C H_{3} C O O H + N H_{4} O H \to C H_{3} C O O N H_{4} + H_{2} O + 48.1 k J

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