$-\left[\Delta G_{f}^{\circ} \mathrm{CaCO}_{3}(s)+2 \Delta G_{f}^{\circ} H^{+}(a q)\right]$ strategies to Crack Exam in limited time period. Specific heat of $L i(\mathrm{s}), N a(\mathrm{s}), K(s), R b(s)$ and $C s(s)$ at $398 K$ are $3.57,1.23,0.756,0.363$ and $0.242 \mathrm{Jg}^{-1} \mathrm{K}^{-1}$ respectively. of water vaporised $=\frac{10}{18}=0.56$ Download eSaral App for Video Lectures, Complete Revision, Study Material and much more...Sol. so $\mathrm{NO}(g)$ is unstable. $20.0 \mathrm{g}$ 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. SHOW SOLUTION This question bank is designed, keeping NCERT in mind and the questions are updated with respect to … Q. Thermodynamics is the study of energy transformations. Download eSaral App for Video Lectures, Complete Revision, Study Material and much more...Sol. Power $\left.=\frac{\text { energy }}{\text { time }} \text { and } 1 W=1 \quad J s^{-1}\right)$ Closed system : (iii) Cane of tomato soup, (iv) Ice cube tray filled with water, (vii) Helium filled balloon. $\Delta S_{1}=-\frac{\Delta H_{v}}{T_{b}}=-\frac{9714.6 \mathrm{cal} \mathrm{mol}^{-1}}{373 \mathrm{K}}$ $\operatorname{SiH}_{4}(g)+2 O_{2}(g) \rightarrow \operatorname{Si} O_{2}(s)+2 H_{2} O(l)$ What type of system would it be ? You are on page 1 of 14. Download eSaral App for Video Lectures, Complete Revision, Study Material and much more...Sol. $H_{2}(g)+\frac{1}{2} O_{2}(g) \rightarrow H_{2} O(l) ; \Delta_{r} H^{\circ}=-286.0 k J m o l^{-1}$ $\Delta G=\Delta H-T \Delta S$ Reaction of combustion of octane: SHOW SOLUTION $\Delta H-92.38 k J=-92380 J, R=8.314 J K^{-1} \mathrm{mol}^{-1}$ (i) Write the relationship between $\Delta H$ and $\Delta U$ for the process at constant pressure and temperature. (iii) $\quad \Delta S=-v e$ because gas is changing to less disorder solid. \[ \Delta_{f} H^{o}=-92.8 k J m o l^{-1} \] Now, $q=53.28 \mathrm{JK}^{-1} \times \Delta T$ Enthalpy of combustion of octane, Heat transferred $=$ Heat capacity $\times \Delta T$, $=\left(8.93 \mathrm{kJ} K^{-1}\right) \times(6.73 \mathrm{K})=60.0989 \mathrm{kJ}$, Molar mass of octane $\left(C_{8} H_{18}\right)=(8 \times 12)+(18 \times 1)=114$, $\therefore$ Internal energy change $(\Delta E)$ during combustion of one mole of, octane $=\frac{60.0989}{1.250} \times 114=5481.02 k J \mathrm{mol}^{-1}$, $C_{8} H_{18}(l)+\frac{25}{2} O_{2}(g) \rightarrow 8 C O_{2}(g)+9 H_{2} O(l)$, $\Delta n_{g}=8-\frac{25}{2}=-\frac{9}{2}$, $\Rightarrow$ Enthalpy change, $\Delta H=\Delta E+\Delta n_{g} R T$, $=\left(5481.02 \times 10^{3}\right)+(-4.5 \times 8.314 \times 300.78)$, $=\left(5481.02 \times 10^{3}\right)-11253.08 \mathrm{J} \mathrm{mol}^{-1}$, $=5492273.082 \mathrm{Jmol}^{-1}=5492.27 \mathrm{kJ} \mathrm{mol}^{-1}$, Q. SHOW SOLUTION The carefully crafted questions and answers provide students with a comprehensive understanding of the chapters involved. $B_{O=O}=\frac{2102}{5}=420.4 \mathrm{kJ} \mathrm{mol}^{-1}$, standard enthalpy change $\Delta H_{r}^{\circ}=-2.05 \times 10^{3} k J / m o l_{r x n}$ and bond energies of $C-C, C-H, C=O$ and $O-H$ are 347 $414,741$ and 464 respectively calculate the energy of oxygen. We won’t spam you. Express the change in internal energy of a system when What is meant by average bond enthalpy ? (ii) Work is done by the system? Calculate the standard enthalpy of formation of $C H_{3} O H(l)$ from the following data: (ii) Calculation of $w$ Compare it with entropy decrease when a liquid sample is converted into a solid. [NCERT] $=270.2-17.22-522.72=-269.72 J K^{-1} \mathrm{mol}^{-1}$, gaseous propane $\left(C_{3} H_{8}\right)$ at $298 K$, $3 C(\text { graphite })+4 H_{2}(g) \rightarrow C_{3} H_{8}(g)$, Given that $S_{m}^{\circ} C(\text { graphite })=5.74 J K^{-1} m o l^{-1}$, $\mathrm{S}_{\mathrm{mH}_{2}(\mathrm{g})}^{\circ} 130.68 \mathrm{JK}^{-1} \mathrm{mol}^{-1}, \mathrm{S}_{\mathrm{mC}_{3} \mathrm{H}_{8}(\mathrm{g})}^{\circ}=270.2 \mathrm{JK}^{-1}$, $S_{m C_{3} H_{8}(g)}-\left[3 \times S_{m}^{\circ} C_{(g r a p h i t e)}+4 \times S_{m H_{2}(g)}^{\circ}\right]$, $=270.2-[(3 \times 5.74)-(4 \times 130.68)] J K^{-1} \mathrm{mol}^{-1}$, $=270.2-17.22-522.72=-269.72 J K^{-1} \mathrm{mol}^{-1}$, Q. As heat is taken out, the system must be having thermally conducting walls. Multiply eqn. 2000 AP CHEMISTRY FREE RESPONSE QUESTIONS. are $30.56 \mathrm{kJ} \mathrm{mol}^{-1}$ and $66.0 \mathrm{JK}^{-1} \mathrm{mol}^{-1}$ respectively. $\therefore \quad \Delta H=+22.2 k_{0} J$ (i) $\frac{1}{2} N_{2}(g)+\frac{1}{2} O_{2}(g) \rightarrow N O(g) ; \Delta_{r} H^{\circ}=90 k J \operatorname{mol}^{-1}$ Which of the following are open close or nearly isolated system ? Internal energy change is measure at constant volume. Calculate the enthalpy change when $10.32 g$ of phosphorus reacts with an excess of bromine. $\therefore$ The enthalpy of polymerization $\left(\Delta H_{\text {poly }}\right)$ must be negative. Predict the sign of entropy change for each of the following changes of state: What will be sign of for backward reaction? 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