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- The value of Q is 1.0*10^-419 g of unknown organic sample was dissolve in 640 mL of Dicloromethane (DCM). The boiling point of benzene was increased by 3.78oC. Determine the molecular weight of the unknown sample? Kb of DCM = 2.42oC/m Bb of benzene = 39.6 oC density of benzene = 1.33 g/mL at 25 °C Round your answer to the nearest whole number, no units required.Convert kPa/sec to uL/min for the following values. -0.0019 kPa/sec -0.0029 kPa/sec -0.0028 kPa/sec -0.0021 kPa/sec -0.0026 kPa/sec -0.0034 kPa/sec
- Chemistry (i) For T = 298K ΔG° = -8.314 x 298 x ln (2.83x10-3) = 14.524 KJ/mol (ii) For T = 308.15K ΔG° = -8.314 x 308.15 x ln (9.619x10-3) = 11.891 KJ/mol (iii) For T = 318.15K ΔG° = -8.314 x 318.15 x ln (3.14x10-2) = 9.147 KJ/mol (iv) For T = 328.15K ΔG° = -8.314 x 328.15 x ln (8.82x10-2) = 6.621 KJ/mol (v) For T = 338.15K ΔG° = -8.314 x 338.15 x ln (2.42x10-1) = 3.990 KJ/mol Based on the measured ΔG° values, is this equilibrium spontaneous at room temperature? Which factor, entropy, or enthalpy, has the greater impact on spontaneity in this case? Explain your answers.Consider the following data. For the acid: H2A Ka = 4.21⋅10−44.21⋅10-4 Calculate the Kb for HA-. Report your answer in scientific notation using 3 sig figs.Ksp values are: 45.76 at -10.0 and 45.75 at 50.0
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