Thus $A l_{2} O_{3}$ cannot be reduced by $C$, (ii) Let us now calculate the $\Delta G$ value for reduction of $P b O$, $2 P b O \longrightarrow 2 P b+O_{2} ; \Delta+120 k J$, $C+O_{2} \longrightarrow C O_{2} ; \Delta G=-380 k J$, On adding, $2 P b O+C \longrightarrow 2 P b+C O_{2}$, Hence $P b O$ can bereduced by carbon because $\Delta \mathrm{G}$ of couple reaction is $-v e$. (iv) the system in equilibrium state or moving from one equilibrium state to another equilibrium state. In the following questions two or more options may be correct. ( } i v)$, (i) $\quad \mathrm{CH}_{3} \mathrm{OH}(l)+\frac{3}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O}(l)$, $\Delta_{r} H^{\circ}=-726 \mathrm{kJmol}^{-1}$, $C_{(G r a p h i t e)}+2 H_{2}(g)+\frac{1}{2} O_{2}(g) \longrightarrow C H_{3} O H(l)$, $\Delta_{r} H^{\circ}=-239 k J m o l^{-1}$. In the following questions more than one correlation is possible between options of both columns. In what way is it different from bond enthalpy of diatomic molecule ? In adiabatic expansion of an ideal gas always: (a) Increase in temperature (b) ∆H = 0 (c) q = 0 (d) W = 0 Answer: (c) q = 0. (iv) burning carbon in oxygen to give carbon dioxide. NCERT Solutions for Class 11 Chemistry Chapter 6 - Thermodynamics. Explain whether the following properties are extensive or intensive. Go Back to Chemistry Home Page Physics Maths Biology. Enthalpy of combustion of carbon to carbon dioxide is – 393.5 J mol-1 .Calculate the heat released upon formation of 35.2 g of C02 from carbon and oxygen gas. Answer: The combustion equation is: C (s) + 0 2 (g) —–> C0 2 (g); AcH = – 393.5 KJ mol -1. Under what conditions will the reaction occur spontaneously? (i) ΔS (system) decreases but ΔS (surroundings) remains the same. Give suitable examples. Q2: Which law of thermodynamics evaluate thermodynamic parameters? What will be the direction of the reaction at this temperature and below this temperature and why? Extensive properties depend on the quantity of matter but intensive properties do not. B negative . During complete combustion of one mole of butane, 2658 kJ of heat is released. Explain. Question 1. of water vaporised $=\frac{10}{18}=0.56$, $\therefore W=-p_{e x} \Delta V \quad\left(\Delta V=\frac{n R T}{P_{e x t}}\right)$, $=-p_{e x} \frac{n R T}{P_{e x t}}=-n R T$, $=-0.56 \times 8.314 \times 10^{-3} \times 373.15=-1.737 k J$, $\Delta U=\Delta H-P \Delta V=\Delta H-n R T$, Calculate the bond enthalpy of $H C l .$ Given that the bond enthalpies of $H_{2}$ and $C l_{2}$ are $430 \mathrm{kJ} \mathrm{mol}^{-1}$ and $242 \mathrm{kJ} \mathrm{mol}^{-1}$ respectively and $\Delta \mathrm{H}_{f}^{\circ}$ for $H C l s-95 k J m o l^{-1}$, $\Delta H_{\text {Reaction}}=\Sigma \Delta H^{\circ}$ $f$ (Products) $-\Sigma \Delta H^{\circ}$ f $(\text {Reactants})$, Calculate $\Delta S$ when 1 mole of steam at $100^{\circ} \mathrm{C}$ is converted into ice at $0^{\circ} \mathrm{C}$. Laws of thermodynamics apply only when a system is in equilibrium or moves from one equilibrium state to another equilibrium state. Standard vaporization enthalpy of benzene at boiling point is $30.8 \mathrm{kJ} \mathrm{mol}^{-1} ;$ for how long would a $100 \mathrm{W}$ electric heater have to operate in order to vaporize a $100 \mathrm{g}$ sample at the temperature? How many times is molar heat capacity than specific heat capacity of water ? It is suggested to check these marks wise questions to be able to tackle any question in the examinations. $20.0 \mathrm{g}$ of ammonium nitrate $\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)$ is dissolved in $125 \mathrm{g}$ of water in a coffee-cup calorimeter. Enthalpy. 1800-212-7858 / 9372462318. What is meant by average bond enthalpy ? Why? It is denoted by G and is given by the equation . Calculate the temperature at which the Gibbs energy change for the reaction will be zero. Clarify concepts to prepare for Organic Chemistry. Is there any enthalpy change in a cyclic process ? At the same time, you must have a basic understanding of all the chapters. where v indicates constant volume. 1; 2; 3 » Question No : 1 In a thermal decomposition reaction, sign of ∆ H may be... A positive . (iv) pressure, volume, temperature, amount. On the basis of these reactions find out which of the algebric relations given in options (i) to (iv) is correct? $\Delta_{r} G^{\circ}=\Delta_{f} G^{\circ}\left(S i O_{2}\right)+2 \Delta_{f} G^{\circ}\left(H_{2} O\right)-\left[\Delta_{f} G^{\circ}\left(S i H_{4}\right)\right]+$, $2 \Delta_{f} G^{\circ}\left(O_{2}\right)$. One mole of acetone requires less heat to vapourise than 1 mol of water. $20.0 \mathrm{g}$ of ammonium nitrate $\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)$ is dissolved in $125 \mathrm{g}$ of water in a coffee cup calorimeter, the temperature falls from $296.5 \mathrm{Kto} 286.4 \mathrm{K} .$ Find the value of $q$ for the calorimeter. (a) Throwing a stone from the ground to roof. Show mathematically that ΔG is a measure of free energy. (ii) Both A and R are true but R is not the correct explanation of A. (ii), (ii) $C_{( \text {graphite) } }+O_{2}(g) \rightarrow C O_{2}(g) ; \Delta_{r} H^{\circ}=-393 \mathrm{kJ} \mathrm{mol}^{-1}$, (iii) $\times 2: 2 H_{2}(g)+O_{2}(g) \rightarrow 2 H_{2} O(l) ; \Delta_{r} H^{o}=-572 k J m o r^{1}$, (iv) $\quad C(g)+2 H_{2}(g)+2 O_{2}(g) \longrightarrow C O_{2}(g)+2 H_{2}^{\circ} O$, $\Delta_{r} H^{\circ}=-965 \mathrm{kJmol}^{-1}$, Subtract eq. (iv) the feasibility of a chemical reaction. Important Questions for 12th Chemistry; Important Questions for 12th Physics; Keep in Touch . (iii) A partition is removed to allow two gases to mix. Thermodynamics Questions with Solutions to help you to revise complete Syllabus and Score More marks in your Class 11 Examinations. CBSE Important Questions for Class 11 Chemistry, Kerala Board Class 11th Model Question Paper, NCERT Important Questions for Class 11 Chemistry, NCERT Solutions for Class 8 Sanskrit Chapter 11 सावित्री बाई फुले, NCERT Solutions for Class 12th Macroeconomics : Chapter 6 – Open Economy Macroeconomics, Class 11 Important Questions for Chemistry - Equilibrium. (i) interrelation of various forms of energy and their transformation from one form to another. Question 11. Dec 19,2020 - Test: First Law Of Thermodynamics | 20 Questions MCQ Test has questions of Class 11 preparation. Assertion (A) : Spontaneous process is an irreversible process and may be reversed by some external agency. Is it possible to decide spontaneity of a reaction from given diagram. Free Question Bank for NEET Chemistry Thermodynamics. The temperature falls from $296.5 \mathrm{Kto} 286.4 \mathrm{K.Find}$ out the value of $q$ for calorimeter and its contents. (iv) because graphite has more disorder than diamond. The enthalpy of vaporisation of liquid diethyl ether $\left[\left(C_{2} H_{5}\right)_{2} O\right]$ is $26.0 \mathrm{kJ} \mathrm{mol}^{-1}$ at its boiling point $\left(35^{\circ} \mathrm{C}\right)$. Our social links. }}{T_{b}}=\frac{\left(26000 \mathrm{J} \mathrm{mol}^{-1}\right)}{(308 \mathrm{K})}=84.4 \mathrm{JK}^{-1} \mathrm{mol}^{-1} \mathrm{since}$. Although heat is a path function but heat absorbed by the system under certain specific conditions is independent of path. Class 11 Detailed Chapter Notes - Thermodynamics, Class 11, Chemistry | EduRev Notes Summary and Exercise are very important for perfect preparation. CBSE Class 11 Chapter 6 Thermodynamics Chemistry Marks Wise Question with Solutions. $T=\frac{\Delta H}{\Delta S}=\frac{-10000 J m o l^{-1}}{-33.3 J K^{-1} m o l^{-1}}=300.3 \mathrm{K}$, (i) For spontaneity from left to right, $\Delta G$ should be $-v e$ for the given reaction. Calculate $\Delta_{f} H^{\circ}$ for chloride ion from the following data: $\frac{1}{2} H_{2}(g)+\frac{1}{2} C l_{2}(g) \rightarrow H C l(g) \Delta_{f} H^{\circ}=-92.8 k J m o l^{-1}$, $H C l(g)+H_{2} O \rightarrow H_{3} O^{+}(a q)+C l^{-}(a q)$, $\Delta_{d i s s} H^{\circ}=-75.2 k J m o l^{-1}$, \[ \Delta_{f} H^{o}=-92.8 k J m o l^{-1} \], (ii) $\quad H C l(g)+H_{2} O \rightarrow H_{3} O^{+}(a q)+C l(a q)$, \[ =\Delta_{d i s s} H^{o}=-75.2 k J m o l^{-1} \], $\frac{1}{2} H_{2}(g)+\frac{1}{2} C l_{2}(g)+H_{2} O \rightarrow H_{3} O^{+}(a q)+C l^{-}(a q)$, $\Delta H^{\circ}=-168.0 \mathrm{kJ} \mathrm{mol}^{-1}$, $\Delta H=\Delta_{f} H^{o}\left(H_{3} O^{+}\right)+\Delta_{f} H^{o}\left(C l^{-}\right)$, $-\left[\frac{1}{2} \Delta_{f} H^{o}\left(H_{2}\right)+\frac{1}{2} \Delta_{f} H^{o}\left(C l_{2}\right)\right]$, The enthalpy of formation of $H_{3} O^{+}(a q)$ in dilute solution may be, taken as zero i.e., $\Delta_{f} H\left[H_{3} O^{+}(a q)\right]=0$, $-168.0=0+\Delta_{f} H^{\circ}\left(\mathrm{C} l^{-}\right)-\left[\frac{1}{2} \times 0+\frac{1}{2} \times 0\right]$, $\Delta_{f} H^{o}\left(C l^{-}\right)=-168 k J m o l^{-1}$. 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