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- Sol. No. 1 2 3 4 5 Volume of KI (ml) 20 18 15 12 10 [KI] K 0.195121951 0.00039 0.175609756 0.0004 0.146341463 0.0005 0.117073171 0.0006 0.097560976 0.0004 Log K Q1) Plot Log K' on y-axis and Log [KI] on x-axis A) Slope = B) Intercept = e) Log K = D) K = Log [KI] -3.40894 -0.70969387 -3.39794 -0.75545136 -3.30103 -0.834632606 -3.22185 -0.931542619 -3.39794 -1.010723865Using the following data O2 (g) SO₂ (g) SO3 (g) Af He/kJ mol-1 0 -296.8 -395.7 AfGe/kJ mol-1 0 -300.2 -371.1 5/JK-1 mol-1 205.1 248.2 256.8 ACO/JK-¹ mol-1 29.4 39.9 50.7 In the following reaction SO₂(g) + O₂(g) → SO3(g) Calculate the enthalpy of reaction, the entropy of reaction, and the Gibbs free energy of the reaction at P=1 atm and T-800 K.the linear trendline equation y= 4.7033x + 0.0045
- The following data are for the system 2A(g) + B(g) → 3C(g) Time (s) 0 10 PA (atm) 1.850 PB (atm) 0.900 Pc (atm) 0.000 0.0850 20 1.500 30 0.600 40 1.100 50 0.435 60 0.920Table 5: Calculating AG Temp "C Temp Kelvin Ка In(Ka) AG=-RTIN(Ka) 22. 1 295.25, 0 0044521 -1.12 18950.34962 35 308 .1S 23236.969dH 0- Ocori4 889 -901 45° 318.18°k 0.0016855 - 8.69 22985.918 55° 328.15°K 0.00 0344201 -1.97 21144.06565 Average AG'= AH°= AS= (Note: the slope of the best fit line is equal to -AS" rather than AS" as stated in the video).•0= AG° + RT * In (K) %3D • -AG° = RT * In (K) %3D • AG° = -RT * In (K) %3D AG° = -0.616 * In (K)... %3D
- 4. Calculate the mass of oxygen (in mg) dissolved in a container of 5.00L of water exposed to a pressure of 1.13atm of air. Assume that the molar fraction of oxygen in the air is 0.21 and Henry's constant for oxygen in water at that temperature is 1.3 x 10-3 M/ atm. al49.4.mg bl.23.5 mg c) 9.87 mg d1.27.3. mg e) 13.7 mgExplain how Matthiessen’s rule is convenient in analyzing the experimental data of potassium below 20 K.Explain the usefulness of the macroscopic, microscopic, and symbolic perspectives inunderstanding chemical systems.
- the speed of particles, thus the Adding ice to food has the effect of likelihood of particle collisions. I.5. At its normal boiling point (337.3 K), methanol (CH3OH) has AvapH = 25.79 kJ/mol, and the densities of its liquid and vapor states at that temperature are 0.7486 g/mL and 0.0.001206 g/mL, respectively. %3D Data from dT (a) Use the Clapeyron equation to determine the value of () for methanol at T = 337.3 K. dP. Report your answer in units of K/bar. (b) Use your result to estimate its boiling point (in K) at a pressure of 2 bars. 3.Using given viscosity values, determine the identity of a liquid which would have a diffusion controlled rate constant kd = 7.51 x 106 m3/s mol at 298K Values: Benzene: 0.601 Ethanol: 1.06 Mercury: 1.55 Methanol: 0.553 Pentane: 0.224 Sulfuric acid: 27 Tetrachloromethane: 0.880 Water: 0.891