CBSE Questions for Class 11 Medical Chemistry Thermodynamics Quiz 12 - MCQExams.com

Choose the reaction in which $$\Delta H$$ is not equal to $$\Delta U$$.
  • $$C\left( graphite \right) +{ O }_{ 2 }\left( g \right) \longrightarrow C{ O }_{ 2 }\left( g \right) $$
  • $${ C }_{ 2 }{ H }_{ 4 }\left( g \right) +{ H }_{ 2 }\left( g \right) \longrightarrow { C }_{ 2 }{ H }_{ 6 }\left( g \right) $$
  • $$2C\left( graphite \right) +{ H }_{ 2 }\left( g \right) \longrightarrow { C }_{ 2 }{ H }_{ 2 }\left( g \right) $$
  • $${ H }_{ 2 }\left( g \right) +{ I }_{ 2 }\left( g \right) \longrightarrow 2HI\left( g \right) $$
  • $${ N }_{ 2 }\left( g \right) +{ O }_{ 2 }\left( g \right) \longrightarrow 2NO\left( g \right) $$
When the total cell emf of a volatic cell is greater than zero, which of the following is true about the reaction quotient $$Q$$ and free energy change $$\triangle G$$ for the cell reaction?
  • $$Q$$ is less than one and $$\triangle G$$ is greater than zero
  • $$Q$$ is greater than one and $$\triangle G$$ is greater than zero
  • $$Q$$ is less than one and $$\triangle G$$ is less than zero
  • $$Q$$ is zero and $$\triangle G$$ is greater than zero
  • $$Q$$ is greater than one and $$\triangle G$$ is less than zero
The enthalpy of combustion for the $$H_{2}$$, cyclohexene and cyclohexane are $$-241, -3800$$ and $$-3920kJ\ mol^{-1}$$, respectively. Heat of hydrogenation of cyclohexene is:
  • $$+121 kJ\ mol^{-1}$$
  • $$-121kJ\ mol^{-1}$$
  • $$+242kJ\ mol^{-1}$$
  • $$-242kJ\ mol^{-1}$$
If $$\Delta H_{f}(H_{2}O)$$ is $$-285.20\ kJ\ mol^{-1}$$, then $$\Delta H_{f}^{\circ}(OH^{-})$$ is:
  • $$-227.90\ kJ\ mol^{-1}$$
  • $$+228.88\ kJ\ mol^{-1}$$
  • $$-343.52\ kJ\ mol^{-1}$$
  • $$+343.52\ kJ\ mol^{-1}$$
The densities of graphite and diamond at $$298K$$ are $$2.25$$ and $$3.31$$ $$g\ { cm }^{ -3 }$$ respectively. If the standard free energy difference is $$1895\ J\ {mol}^{-1}$$, the pressure at which graphite will be transformed into diamond is:
  • $$9.92\times { 10 }^{ 8 }Pa$$
  • $$9.92\times { 10 }^{ 7 }Pa$$
  • $$9.92\times { 10 }^{ 6 }Pa$$
  • None of these
At 298 K the entropy of rhombic sulphur 32.04 J/mol K and that of monoclinic sulphur is 32.68 J/mol K. The heat of their combustion are respectively $$-298246$$ and $$-297948 \,J$$ $$mol^{-1}.$$ $$\Delta \,G $$ for the reaction; $$S_{rhormbic} \rightarrow  S_{monoclinic}$$ will be :
  • 107.28 J
  • 10.728 J
  • 107.28 kJ
  • 10728 J
Given: $$S+\dfrac { 3 }{ 2 } { O }_{ 2 }\longrightarrow S{ O }_{ 3 }+2x$$ $$kcal$$
           $$S{ O }_{ 2 }+\dfrac { 1 }{ 2 } { O }_{ 2 }\longrightarrow S{ O }_{ 3 }+y$$ $$kcal$$

With the help of the above reactions, find out the heat of formation of $$S{ O }_{ 2 }$$.
  • $$\left( 2x-y \right) $$
  • $$\left( x+y \right) $$
  • $$\left( 2x+y \right) $$
  • $$\left( { 2x }/{ y } \right) $$
A particular reaction at $${27}^{o}C$$ for which $$\Delta H > 0$$ and $$\Delta S> 0$$ is found to be non-spontaneous. The reaction may proceed spontaneously if:
  • the temperature is decreased
  • the temperature is kept constant
  • the temperature is increased
  • it is carried in open vessel at $${27}^{o}C$$
Although the dissolution of ammonium chloride in water is an endothermic reaction, even then it is spontaneous because:
  • $$\Delta H$$ is positive, $$\Delta S$$ is -ve
  • $$\Delta H$$ is +ve, $$\Delta S$$ is zero
  • $$\Delta H$$ is positive, $$T\Delta S< \Delta H$$
  • $$\Delta H$$ is +ve, $$\Delta S$$ is positive and $$\Delta H< T\Delta S$$
A piece of metal weighing $$100$$ g is heated to $$80^o$$ C and dropped into $$1$$ kg of cold water in an insulated container at $$15^o$$ C. If the final temperature of the water in the container is $$15.69^o$$ C, the specific heat of the metal in $$J/g^o$$.C is:
  • $$0.38$$
  • $$0.24$$
  • $$0.45$$
  • $$0.13$$
The enthalpy of hydrogenation of benzene is $$-49.8\ kcal/mol$$ while its resonance energy is $$36.0\ kcal/mol$$. The enthalpy of formation of benzene is:
  • $$-4.6\ kcal$$
  • $$-28.6\ kcal/mol$$
  • $$-85.8\ kcal/mol$$
  • $$-13.8\ kcal/mol$$
The molar heat capacities of Iodine vapour and solid are $$7.8$$ and $$14\ cal/mol$$ respective enthalpy of sublimation of iodine is $$6096\ cal/mol$$ at $$200^{\circ}C$$, then what is $$\Delta H$$ the value  at $$250^{\circ}C$$ in cal/mol.
  • $$5360$$
  • $$4740$$
  • $$6406$$
  • none of these
The enthalpy of combustion of methane, graphite and dihydrogen at $$298K$$ are $$-890.3$$ $$kJ{ mol }^{ -1 },-393.5$$ $$kJ{ mol }^{ -1 },-285.8$$ $$kJ { mol }^{ -1 }$$ respectively. Enthalpy of formation of $${CH}_{4(g)}$$ will be:
  • $$-74.8kJ { mol }^{ -1 }$$
  • $$-52.27kJ { mol }^{ -1 }$$
  • $$+74.8kJ{ mol }^{ -1 }$$
  • $$+52.26kJ{ mol }^{ -1 }$$
Water is brought to boil under the pressure of $$1.0\ atm$$. When an electric current of $$0.50\ A$$ from a $$12\ V$$ supply is passed for $$300\ s$$ through resistance in thermal contact with it is found that $$0.798\ g$$ of water is vapourised. Calculate the molar internal energy change at boiling point $$(373.15\ K)$$.
  • $$37.5kJ\ { mol }^{ -1 }$$
  • $$3.75kJ\ { mol }^{ -1 }$$
  • $$42.6kJ\ { mol }^{ -1 }$$
  • $$4.26kJ\ { mol }^{ -1 }$$
Calculate $$\Delta H^0_{f}$$ for $$ UBr_4$$ from $$\Delta G^0$$ of reaction and the $$S^0$$ values.$$ U(s)+2Br_2(l)\rightarrow UBr_4(s) ; \, \Delta G^0=-788.6 KJ; \, S^0(J/K-mol) 50.3 , 152.3 , 242.6$$
  • -822.1 KJ/mol
  • -841.2 KJ/mol
  • -775.6 KJ/mol
  • -804.3 KJ/mol
For the reaction, $${ C }_{ 3 }{ H }_{ 8 }\left( g \right) +5{ O }_{ 2 }\left( g \right) \longrightarrow 3C{ O }_{ 2 }\left( g \right) +4{ H }_{ 2 }O\left( l \right) $$ at constant temperature, $$\Delta H-\Delta E$$ is:
  • $$+3 RT$$
  • $$-RT$$
  • $$+RT$$
  • $$-3RT$$
If for $$H_{2}(g) + \dfrac {1}{2} O_{2}(g) \rightarrow H_{2}O(g); \triangle H_{1}$$ is the enthalpy of reaction and for $$H_{2}(g) + \dfrac {1}{2}O_{2}(g) \rightarrow H_{2}O(l); \triangle H_{2}$$ is enthalpy of reaction then:
  • $$\triangle H_{1} > \triangle H_{2}$$
  • $$\triangle H_{1} = \triangle H_{2}$$
  • $$\triangle H_{1} < \triangle H_{2}$$
  • $$\triangle H_{1} + \triangle H_{2} = 0$$
Ellingham's diagram represents
  • Change of $$\Delta G$$ with temperature
  • Change of $$\Delta H$$ with temperature
  • Change of $$\Delta G$$ with pressure
  • Change of $$\left( \Delta G-T\Delta S \right) $$ with temperature
$$1$$ mole of ice at $$0^{\circ}C$$ and $$4.6$$ mm Hg pressure is converted to water vapour at a constant temperature and pressure. Find $$\Delta H$$ if the latent heat of fusion of ice is $$80$$ Cal/gm and latent heat of vaporization of liquid water at $$0^{\circ}C$$ is $$596$$ Cal per gram and the volume of ice in comparison to that of water (vapour) is neglected.
  • 14.53 Kcal/mol
  • 12.16 Kcal/mol
  • 10.22 Kcal/mol
  • 15.62 Kcal/mol
$$100\ ml\ 0.5 N\ H_{2}SO_{4}$$ (strong acid) is neutralised with $$200\ ml\ 0.2\ M\ NH_{4}OH$$ in a constant pressure Calorimeter which results in temperature rise of $$1.4^{\circ}C$$. If heat capacity of Calorimeter content is $$1.5\ kJ/^{\circ}C$$. Which statement is/ are correct:

Given: $$HCl + NaOH\rightarrow NaCl + H_{2}O + 57\ kJ$$
$$CH_{3}COOH + NH_{4}OH \rightarrow CH_{3}COONH_{4} + H_{2}O + 48.1\ kJ$$
  • enthalpy of neutralisation of $$HCl$$ v/s $$NH_{4}OH$$ is $$-52.5\ kJ/mol$$
  • enthalpy of dissociation (ionization) of $$NH_{4}OH$$ is $$4.5\ kJ/ mol$$
  • enthalpy of dissociation of $$CH_{3}COOH$$ is $$4.6\ kJ/mol$$
  • $$\triangle H$$ for $$2H_{2}O(l)\rightarrow 2H^{+}(aq.) + 2OH^{-}(aq.)$$ is $$114\ kJ$$
Fruend and Long were 2 scientists interested in adsorption.
Once in a discussion Fruend asked "I can see adsorption is spontaneous, but why it is always exothermic?"
Long said"_________________"
Choose Long's answer :
  • $$\triangle$$G > 0 & $$\triangle$$ S < 0 $$\Rightarrow$$ $$\triangle$$H < 0
  • $$\triangle$$G < 0 & $$\triangle$$ S < 0 $$\Rightarrow$$ $$\triangle$$H < 0
  • $$\triangle$$G > 0 & $$\triangle$$ S > 0 $$\Rightarrow$$ $$\triangle$$H > 0
  • $$\triangle$$G , 0 & $$\triangle$$ S > 0 $$\Rightarrow$$ $$\triangle$$H > 0
Calculate the heat needed to raise the temperature of $$20g$$ iron from $${25}^{o}C$$ to $${500}^{o}C$$, if specific heat capacity of iron is $$0.45J{K}^{-1}$$ $${g}^{-1}$$.
  • $$6732J$$
  • $$225J$$
  • $$15.66J$$
  • $$2250J$$
For the reaction taking place at certain temperature $$NH_{2}COONH_{4}(s)\rightleftharpoons 2NH_{3}(g)$$ if equilibrium pressure is $$3X$$ bar then $$\Delta G^{\circ}$$ would be:
  • $$-RT\ ln\ 9 -3RT\ ln\ X$$
  • $$RT\ ln\ 4 -3RT\ ln\ X$$
  • $$-3RT\ ln\ 4X$$
  • none of these
A monoatomic ideal gas undergoes a process in which the ratio of $$P$$ to $$V$$ at any instant is constant and equals to $$1$$. What is the molar heat capacity of the gas?
  • $$4R/2$$
  • $$3R/2$$
  • $$5R/2$$
  • $$0$$
Which statement is correct?
  • $$\left (\dfrac {dH}{dT}\right )_{P} < \left (\dfrac {dE}{dT}\right )_{V}$$
  • $$\left (\dfrac {dH}{dT}\right )_{P} + \left (\dfrac {dE}{dT}\right )_{V} = R$$
  • $$\left (\dfrac {dE}{dV}\right )_{T}$$ of ideal gas is zero
  • All of these
Calculate the hear needed to raise the temperature of $$20g$$ from $${25}^{o}C$$ to $${500}^{o}C$$, if specific heat capacity of iron is $$0.45J{K}^{-1}$$ $${g}^{-1}$$.
  • $$4274J$$
  • $$225J$$
  • $$15.66J$$
  • $$2250J$$
A solid material supplied with heat at a constant rate. The temperature of material is changing with heat input as shown in figure. What does slope DE represents?
770029_61e11a6e2e494229bed77b340bcce338.png
  • latent heat of liquid
  • latent heat of vapour
  • heat capacity of vapour
  • inverse of heat capacity of vapour
The Gibb's energy for the decomposition of $${Al}_{2}{O}_{3}$$ at $${500}^{o}C$$ is as follows:

$$\cfrac { 2 }{ 3 } { Al }_{ 2 }{ O }_{ 3 }\longrightarrow  \dfrac{ 4}{ 3}Al+{ O }_{ 2 }\ ;$$    $$\Delta G=+960\ kJ$$.

The potential difference needed for the electrolytic reduction of aluminium oxide ($${Al}_{2}{O}_{3}$$) at $${500}^{o}C$$ is at least:
  • $$4.5V$$
  • $$3.0V$$
  • $$2.5V$$
  • $$5.0V$$
$$H_2(g) + Cl_2 (g)  = 2HCl (g)$$;
$$\Delta{H}$$(298K) $$= -22.06 $$kcal. For this reaction, $$\Delta{U}$$ is equal to:
  • $$-22.06 + 2\times 10^{-3} \times 298 \times 2 kcal$$
  • $$-22.06 + 2 \times 298\ kcal$$
  • $$-22.06 - 2 \times 298 \times 4\ kcal$$
  • $$-22.06\ kcal$$
Calculate the heat needed to raise the temperature of $$20\ g$$ iron from $$25^{\circ}C$$ to $$500^{\circ}C$$, if specific heat capacity of iron is $$0.45\ JK^{-1}g^{-1}$$.
  • $$15.66\ J$$
  • $$4275\ J$$
  • $$225\ J$$
  • $$2250\ J$$
$$9.2g$$ of toulene $${C}_{2}{H}_{8}(l)$$ is completely burnt in air. The difference in heat change at constant pressure and constant volume at $${27}^{o}C$$ is
  • $$-2.5kJ$$
  • $$+2.5kJ$$
  • Zero
  • $$-0.50kJ$$
A vessel contains $$100$$ litres of a liquid X. Heat is supplied to the liquid in such a fashion that, heat given equals change in enthalpy. The volume of the liquid increases by $$2$$ litres. If the external pressure is one atm, and $$202.6$$ Joules of heat were supplied, then $$[$$U $$-$$ total internal energy$$]$$ :
  • $$\Delta U = 0, \Delta H=0$$
  • $$\Delta U = +202.6J, \Delta H = +202.6$$J
  • $$\Delta U = -202.6J, \Delta H = -202.6$$J
  • $$\Delta U = 0, \Delta H = +202.6J$$
$$H^{+}(aq) + NaOH (aq) \to Na^{+} + H_{2}O(l)\ \triangle H_{1} = -1390\ cals$$
$$HCN(aq) + NaOH(aq) \rightarrow Na^{+} + CN^- + H_{2}O(l)\ \triangle H_{2} = -2900\ cals$$.

What is $$\triangle H$$ value for $$HCN (aq) \to H^{+}(aq) + CN^{-}(aq)$$?
  • $$11400\ cals$$
  • $$10790\ cals$$
  • $$12500\ cals$$
  • $$9800\ cals$$
Ethyl chloride $$\left( { C }_{ 2 }{ H }_{ 5 }Cl \right) $$, is prepared by reaction of ethylene with hydrogen chloride :
$${ C }_{ 2 }{ H }_{ 4 }\left( g \right) +HCl\left( g \right) \longrightarrow { C }_{ 2 }{ H }_{ 5 }Cl\left( g \right) ; \triangle H=-72.3kJ/mol$$
What is the value of $$\triangle U$$ (in kJ), if $$70\ g$$ of ethylene and $$73\ g$$ of $$HCL$$ are allowed to react at $$300\ K$$?
  • $$-69.8$$
  • $$-180.75$$
  • $$-174.5$$
  • $$-139.6$$
For a certain reaction the change in enthalpy and change in entropy are 40.63 kJ $$mol^{-1}$$ and 100 $$JK^{-1}$$. What is the value of $$\Delta$$ at $$27^0C$$ and indicate whether the reaction is spontaneous or not
  • $$+10630 J\, mol^{-1}$$; spontaneous
  • $$+10630 J\, mol^{-1}$$; non spontaneous
  • $$-7990\, J\, mol^{-1}$$; spontaneous
  • $$+7900\, J\,mol^{-1}$$; spontaneous
Stearic acid $$\left[ C{ H }_{ 3 }\ { \left( C{ H }_{ 2 } \right)  }_{ 16 }\ C{ O }_{ 2 }H \right]$$ is a fatty acid, the part of fat that stores most of the energy. $$1.0\ g$$ of stearic acid was burned in a bomb calorimeter. The bomb had a heat capacity of $$652\ J/ C$$. If the temperature of $$500\ g $$ water $$\left( c=4.18J/g\ C \right)$$ rose from $$25.0$$ to $$39.3 C$$, how much heat was released when the strearic acid burned? $$[Given\ { C }_{ p }\left( { H }_{ 0 }O \right) =4.18\ { J }/{ g }\ C]$$
  • $$39.21\ kJ$$
  • $$29.91\ kJ$$
  • $$108\ kJ$$
  • $$9.32\ kJ$$
For which of the following reaction $$\triangle H \neq \triangle U$$:
  • $$H_2(g) + Cl_2(g)\rightarrow 2HCl(g)$$
  • $$N_2(g) + 3H_2(g)\rightarrow 2NH_3(g)$$
  • $$NH_4HS_{(s)}\rightarrow NH_3(g) + H_2S(g)$$
  • $$CaCO_3(s)\rightarrow CaCO(s) + CO_2(g)$$
For Pt, $${H}_{2}$$($${p}_{1}atm$$) $$\left| { H }^{ \oplus}\left( 1M \right)  \right| { H }_{ 2 }\left( { p }_{ 2 }\ atm \right)$$ , Pt (where, $${p}_{1}$$ and $${p}_{2}$$ are pressures) cell reaction will be spontaneous if?
  • $${p}_{1}={p}_{2}$$
  • $${p}_{1}> {p}_{2}$$
  • $${p}_{2}> {p}_{1}$$
  • $${p}_{1}=1atm$$
For a certain reaction the change in enthalpy and change in entropy are $$40.63\ kJ\ ,ol\ KJ^{-1}$$. What is the value of $$\triangle G$$ at $$27^{\circ}C$$ and indicate whether the reaction is spontaneous.
  • $$+10630\ J\ mol^{-1}$$; spontaneous
  • $$+10630\ J\ mol^{-1}$$; non spontaneous
  • $$-7990\ J\ mol^{-1}$$; spontaneous
  • $$+7900\ J\ mol^{-1}$$; spontaneous
For $$Ag, \overline {C_{P}} (JK^{-1}mol^{-1})$$ is given by $$24 + 0.006\ T$$. If temperature of $$3\ mol$$ of silver is raised from $$27^{\circ}C$$ to its melting point $$927^{\circ}C$$ under $$1$$ atm pressure then $$\triangle H$$ is equal to:
  • $$52\ kJ$$
  • $$76.95\ kJ$$
  • $$89.62\ kJ$$
  • $$38.62\ kJ$$
What is free energy change $$\left( \Delta G \right) $$ when $$1.0$$ mole of water at $${ 100 }^{ o }C$$ and $$1$$ atm pressure is converted into steam at $${ 100 }^{ o }C$$ and $$2\ atm$$ pressure?
  • $$0\ cal$$
  • $$540\ cal$$
  • $$515.4\ cal$$
  • $$None\ of\ these$$
The heat capacity of a bomb calorimeter is $$300\ J/K$$. When $$0.16\ gm$$ of methane was burnt in this calorimeter the temperature rose by $$3^{\circ}C$$. The value of $$\triangle U$$ per mole will be
  • $$100\ kJ$$
  • $$90\ kJ$$
  • $$900\ kJ$$
  • $$48\ kJ$$
$$NX$$ is produced by the following step of reactions:
$$M+{ X }_{ 2 }\longrightarrow M{ X }_{ 2 }$$
$$3M{ X }_{ 2 }+{ X }_{ 2 }\longrightarrow { M }_{ 3 }{ X }_{ 8 }$$
$${ M }_{ 3 }{ X }_{ 8 }+{ N }_{ 2 }{ CO }_{ 3 }\longrightarrow NX+{ CO }_{ 2 }+{ M }_{ 3 }{ O }_{ 4 }$$
How much $$M$$ (metal) is consumed to produce $$206gm$$ of $$NX$$?
(Take atomic weight of $$M=56,N=23,X=80$$)
  • $$42gm$$
  • $$336gm$$
  • $$\cfrac { 14 }{ 3 } gm$$
  • $$\cfrac { 7 }{ 4 } gm$$
The heat change during the reaction $$24g\ C$$ and $$128g\ S$$ following the change: 

$$C + S_{2} \rightarrow CS_{2}; \triangle H = 22K\ cal$$.
  • $$22\ K\ cal$$
  • $$11\ K\ cal$$
  • $$44\ K\ cal$$
  • $$32\ K\ cal$$
$$100ml$$ of $${O}_{2}$$ gas diffuses in $$10$$ seconds. $$100ml$$ of gas $$x$$ diffuses in $$t$$ seconds. Gas $$x$$ and time $$t$$ can be respectively:
  • $${H}_{2}, 2.5$$ seconds
  • $${SO}_{2}$$, $$16$$ seconds
  • $$CO$$,$$10$$ seconds
  • $$He$$, $$4$$ seconds
For a given reaction, $$\Delta H = 35.5 kJ mol^{-1}$$ and $$\Delta S = 83.6 kJ mol^{-1}$$. The reaction is spontaneous at: (Assume that $$\Delta H $$ and $$\Delta S$$ do not vary with temperature)
  • T > 425 K
  • all temperatures
  • T > 298 K
  • T < 425 K
On the basis of the following thermochemical data
$${ H }_{ 2 }{ O }_{ (g) }\longrightarrow { H }_{ (aq) }^{ + }+{ OH }_{ (aq) }^{ - };\Delta H=57.32kJ\quad $$
$${H}_{2(g)}+\cfrac{1}{2}{O}_{2(g)}\longrightarrow{ H }_{ 2 }{ O }_{ (l) };\Delta H=-286.2kJ$$
The value of enthalpy of formation of $${OH}^{-}$$ ion at $${ 25 }^{ o }C$$ is:
  • $$+288.88kJ$$
  • $$-343.52kJ$$
  • $$-22.88kJ$$
  • $$-228.88kJ$$
Heat of reaction for the equation, $$A(s) + B(g) \rightarrow 2C(g)$$ is $$40\ kJ$$ at $$300\ K$$ at constant volume. Hence, heat of reaction at constant pressure and at $$300\ K$$ is___________.
  • $$42.5\ kJ$$
  • $$37.5\ kJ$$
  • $$40.0\ kJ$$
  • $$30.0\ kJ$$
If an electron is moving in an orbit with total energy $$U = -\dfrac {e^{2}}{r} r$$ is radius of the orbit then find the speed of the electron.
  • $$\dfrac {e}{\sqrt {mr}}$$
  • $$e\dfrac {e}{\sqrt {mr}}$$
  • $$\dfrac {e}{r}\sqrt {\dfrac {2}{m}}$$
  • $$\dfrac {2e}{\sqrt {mr}}$$
$${E}^{o}$$ of an electrode half reaction is related to $$\Delta { G }^{ o }$$ by the equation, $${ E }^{ o }=-\Delta { G }^{ o }/nF$$. If the amount of $${Ag}^{+}$$ in the half reaction, $${ Ag }^{ + }+{ e }^{ - }\longrightarrow Ag$$ is tripled then:
  • $$n$$ is tripled
  • $$\Delta { G }^{ o }$$ reduces to one third
  • $${E}^{o}$$ reduces to one third
  • None of the above
0:0:1


Answered Not Answered Not Visited Correct : 0 Incorrect : 0

Practice Class 11 Medical Chemistry Quiz Questions and Answers