Enthalpy of Neutralisation

Q. Enthalpy for the reaction $C+O_2\to C{O}_2$ is

1. Positive
2. Negative
3. Zero
4. Can't say, need thermochemical data

Q. Equal volumes of 1M HCl& 1M $H_{2}S{O}_4$ are neutralized by 1M NaOH solution and x & y KJ/equivalent of heat are liberated respectively. Which of the following relations is correct?

1. x = 2y

2. x = 3y

3. x = 4y

4. x = $\frac{1}{2}$ y

Q.

The enthalpy of neutralization of $HCl$ and $NaOH$ is $-57kJmo{l}^{-1}$. The heat evolved at constant pressure (in kJ) when $0.5mole$ of H2SO4 react with $0.75mole$ of $NaOH$ is equal to

1. $57\times \frac{3}{4}$

2. $57\times 0.5$

3. $57$

4. $57\times 0.25$

Q. The heats of neutralization of four acids A, B, C, D are $-13.7,-9.4,-11.2,-12.4kcal$ respectively, when they are neutrelized by a common base. The acidic character obeys the order :

1. A>B>C>D
2. A>D>C>B
3. D>C>B>A
4. D>B>C>A

Q. Enthalpy of neutralization of $H_{3}P{O}_3$ acid is -106.68 kJ/mol using $NaOH$. If enthalpy of neutralization of $HCl$ by $NaOH$ is -55.84 kJ/mol.
Calculate $△H_{ionization}of{H}_{3}P{O}_3$ into its ions:

1. 50.84 kJ/mol
2. 5 kJ/mol
3. 2.5 kJ/mol
4. None of these

Q. Heat of neutralisation for the given reaction $NaOH+HCl\to NaCl+H_{2}O$ is $57.9kJ/mole$. What will be the heat released when 0.75 moles of $NaOH$ is titrated against 1.25 moles of $HCl$?

1. $22.56$ kJ
2. $47.12$ kJ
3. $43.42$ kJ
4. $28.65$ kJ

Q. $50.0mL$ of $0.10MHCl$ is mixed with $50.0mL$of $0.10MNaOH$. The solution's temperature rises by ${0.6}^{o}C.$ Calculate the enthalpy of neutralization per mole of $HCl$.
Given : density and specific heat of solution is $1gm{L}^{-1}$ and 4.2 $J{g}^{-1\circ }{C}^{-1}$

1. $-50.4kJ/mol$
2. $-54.4kJ/mol$
3. $-57.7kJ/mol$
4. $-63.2kJ/mol$

Q. The heats of neutralization of four acids A, B, C and D are -13.7, -9.4, -11.2 and -12.4 $kcalmo{l}^{-1}$ respectively, when they are neutralized by a common base. The acidic character obeys the order:

1. A > B > C > D
2. A > D > C > B
3. D > C > B > A
4. D > B > C > A

Q. 100 ml of 0.3 M HCI solution is mixed with 100 ml of 0.33 M KOH solution. The amount of heat liberated is:
Consider,
$△H_{neut}=-55.2kJmo{l}^{-1}$

1. 1.66 kJ
2. 1.42 kJ
3. 1.31 kJ
4. 1.94 kJ

Q. Match the following (Assume heat of neutralisation of strong acid with strong base is 13.7 kcal):

$\begin{array}{cccc}& \text{Column - I}& & \text{Column - II}\\ & \text{(Enthalpy change in kcal)}& & \text{(Neutralisation)}\\ \text{(A)}& <13.7\text{kcal}& \text{(p)}& \underset{\left(1mol\right)}{HCl}+\underset{\left(1mol\right)}{NaOH}\\ \text{(B)}& =13.7\text{kcal}& \text{(q)}& \underset{\left(1mol\right)}{HF}+\underset{\left(1mol\right)}{NaOH}\\ \text{(C)}& >13.7\text{kcal}& \text{(r)}& \underset{\left(1mol\right)}{N{H}_{4}OH}+\underset{\left(1mol\right)}{HCl}\\ \text{(D)}& =27.4\text{kcal}& \text{(s)}& \underset{\left(2mol\right)}{NaOH}+\underset{\left(1mol\right)}{H_{2}S{O}_4}\\ & & \text{(t)}& \underset{\left(1mol\right)}{NaOH}+\underset{\left(1mol\right)}{C{H}_{3}COOH}\end{array}$

1. a - r, t
   b - p
   c - q, s
   d - s
2. a - r, t, s
   b - p
   c - q,
   d - s
3. a - r, t, s
   b - p, s
   c - q, s
   d - s
4. a - r, t
   b - p, s
   c - q, s
   d - p

Q.

At a particular temperature $H^{+}\left(aq\right)+O{H}^{-}\left(aq\right)\to H_{2}O\left(l\right);\Delta H=-57.1kJ$. The approximate heat evolved when $400mL$ of $0.2$ $H_{2}S{O}_4$ is mixed with $600mL$ of $0.1m$ $KOH$ solution will be:

1. 3.426kJ

2. 13.7kJ

3. 5.2 kJ

4. 55kJ

Q. Equimolar solutions of HCl and NaOH are neutralized with one another. The enthalpy released in the process is approximately

1. 57.1 kJ/eq.
2. 5.71 kJ/eq.
3. 0.571 kJ/eq.
4. 571 kJ/eq.

Q. Heat of neutralization of strong acid against strong base is constant and is equal to

1. $13.7kcal$
2. $57kJ$
3. $5.7\times {10}^{4}J$
4. All of the above

Q. The enthalpy of neutralisation of strong acid by a strong base is $-57.32kJmo{l}^{-1}$. The enthalpy of formation of water is $-285.84kJmo{l}^{-1}$. The enthalpy of formation of hydroxyl ion is :

1. $+228.52kJmo{l}^{-1}$
2. $-114.26kJmo{l}^{-1}$
3. $-228.52kJmo{l}^{-1}$
4. $+114.2kJmo{l}^{-1}$

Q. The heat of neutralization of HCl by NaOH is -55.9 kJ mol${}^{-1}$. If the heat of neutralization of HCN by NaOH is -12.1 kJ/mol, the energy of dissociation of HCN is:

1. -43.8 kJ
2. 43.8 kJ
3. 68 kJ
4. -68 kJ

Q. Which of the following reactions have maximum heat of neutralisation?

1. $N{H}_{4}OHandC{H}_{3}OOH$
2. $N{H}_{4}OHandHCl$
3. $NaOHandC{H}_{3}OOH$
4. $NaOHandHCl$

Q. Match the following (Assume heat of neutralisation of strong acid with strong base is 13.7 kcal):

$\begin{array}{cccc}& \text{Column - I}& & \text{Column - II}\\ & \text{(Enthalpy change in kcal)}& & \text{(Neutralisation)}\\ \text{(A)}& <13.7\text{kcal}& \text{(p)}& \underset{\left(1mol\right)}{HCl}+\underset{\left(1mol\right)}{NaOH}\\ \text{(B)}& =13.7\text{kcal}& \text{(q)}& \underset{\left(1mol\right)}{HF}+\underset{\left(1mol\right)}{NaOH}\\ \text{(C)}& >13.7\text{kcal}& \text{(r)}& \underset{\left(1mol\right)}{N{H}_{4}OH}+\underset{\left(1mol\right)}{HCl}\\ \text{(D)}& =27.4\text{kcal}& \text{(s)}& \underset{\left(2mol\right)}{NaOH}+\underset{\left(1mol\right)}{H_{2}S{O}_4}\\ & & \text{(t)}& \underset{\left(1mol\right)}{NaOH}+\underset{\left(1mol\right)}{C{H}_{3}COOH}\end{array}$

1. a - r, t
   b - p
   c - q, s
   d - s
2. a - r, t, s
   b - p
   c - q,
   d - s
3. a - r, t, s
   b - p, s
   c - q, s
   d - s
4. a - r, t
   b - p, s
   c - q, s
   d - p

Q. The quantity of heat absorbed or evolved when 1 mole of an acid is neutralised by one mole of a base is called enthalpy of neutralisation.

1. True
2. False

Q. Enthalpy of neutralization of $H_{3}P{O}_3$ acid is -106.68 kJ/mol using $NaOH$. If enthalpy of neutralization of $HCl$ by $NaOH$ is -55.84 kJ/mol.
Calculate $△H_{ionization}of{H}_{3}P{O}_3$ into its ions:

1. 50.84 kJ/mol
2. 5 kJ/mol
3. 2.5 kJ/mol
4. None of these

Q. The heats of neutralization of four acids A, B, C and D are -13.7, -9.4, -11.2 and -12.4 $kcalmo{l}^{-1}$ respectively, when they are neutralized by a common base. The acidic character obeys the order:

1. A > B > C > D
2. A > D > C > B
3. D > C > B > A
4. D > B > C > A

Q. The heat of neutralisation is maximum when

1. Sodium hydroxide is neutralised by acetic acid
2. Ammoniym hydroxide is neutralised by acetic acid
3. Ammonium hydroxide is neutralised by hydrochloric acid
4. Sodium hydroxide is neutralised by hydrochloric acid

Q. When 22.4 litres of $H_2\left(g\right)$ is mixed with 11.2 litres of $C{l}_2\left(g\right)$, each at $S.T.P,$ the moles of $HCl\left(g\right)$ formed is equal to :-

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Q.

If heat of dissociation of $CHC{l}_{2}COOH$ is $0.7kcal/mole$ then $\Delta H$ for the reaction:

$CHC{l}_{2}COOH+KOH\to CHC{l}_{2}COOK+H_{2}O$

1. -13 kcal

2. +13 kcal

3. -14.4 kcal

4. -13.7 kcal

Q. The enthalpy of transition of C(diamond) to C(graphite) is?
Given that the enthalpies of combustion of C(diamond) and C(graphite) are – 393.5 and – 395.4 kJ $mo{l}^{-1}$ respectively)

1. + 1.9 kJ
2. - 1.9 kJ
3. 3.8 kJ
4. - 3.8 kJ

Q.

Which of the following acid will release maximum amount of heat when completely neutralized by strong base NaOH?

1. 1M HCl

2. 1M $HN{O}_3$
3. 1M $HCl{O}_4$
4. 1M $H_{2}S{O}_4$

Q. The enthalpies of neutralisation of $HCl{O}_4$ and $C{l}_{3}C-COOH$ are $-13.5kcal/g-equivalent$ and $-14.7kcal/g-equivalent$respectively when $40gm$of solid NaOH is added to a mix of $1gmol$. $HCl{O}_4$ and $1gmol$. $C{l}_{3}C-COOH$ sodium perchlorate and sodium trichloroacetate are formed in molar ratio of 3 : 1. Then:

1. $△H$ for the reaction of NaOH with the mix. is $6.45kcal$.
2. $△H$ for the reaction of NaOH with the mix. is $13.8kcal$.
3. After reaction the total number of moles of acid remained are 0.5 is $HCl{O}_{4}andC{l}_{3}C-COOH)$
4. After reaction the total weight of moles of acid remained are $147.7g$ is $HCl{O}_{4}andC{l}_{3}C-COOH)$ and $△H$ for the reaction of NaOH with mix. is $-13.8kcal$