The vaporization of compound A is described by the following chemical equation. A(1) A(8) A rap(72.39...
Be sure to answer all parts. The molar heats of fusion and vaporization of a certain substance are 2.89 kJ/mol and 8.84 kJ/mol, and its melting point and boiling point are -177°C and -141°C, respectively. Calculate the entropy changes for fusion (solid to liquid) and vaporization (liquid to gas). ASfus J/K mol AS vap = J/K mol
From AHⓇ and AS 11. Hydrogen reacts with nitrogen to form ammonia (NH) according to the reaction 3H:(g) +Nz() 5 2NH,(g) The value of Alºis -92.38 kJ/mol, and that of AS is -198.2 J/mol K. Determine AG at 25°C. a. +5.897 x 109 kJ/mol d. -16,66 kJ/mol b. +297.8 kJ/mol +49.5 kJ/mol c.-33.32 kJ/mol Free Energy, Entropy, Enthalpy 12. A reaction with a low enthalpy of reaction value is not spontaneous at low temperature but becomes spontaneous at high temperature....
Liquid nitrogen has a measured enthalpy of vaporization ( ΔH^o vap) = 2.79 kJ/mol and entropy of vaporization ( Δ S^ovap) = 36.1 J/K mol. Calculate the boiling point of liquid nitrogen, in oC using this information. (Use 273.15 K = 0 oC for the temperature conversion. Report your answer with three significant figures.) Tvap = ????? °C I got 196^oC but it is incorrect.
Entropy and Change of State The standard enthalpy of vaporization for CHFCI2 is 242.17 J/g at its normal boiling point of 8.92°C. Calculate the standard entropy of vaporization (AS°vap) of CHFC12(1). Answer to the nearest 0.1 J K-1 mol-1. cf Zumdahl Chemical Principles 8th ed. sec. 10.4 pp 362-5. Submit Answer Tries 0/5
The heat of vaporization of benzene (C6H6) is 30.77 kJ/mol at it's boiling point (80 C). As a liquid, it has a heat capacity of 134.8 J/mol*K, and as a gas it has a heat capacity of 82.4 J/mol*K. Calculate the enthalpy change of heating 245g of benzene from 50 C to 100 C.
Calculate the change in entropy (in J/K) that occurs when a sample containing 2.00 moles of water is heated from 10.00°C to 300.0 °C at 1 atm pressure. Molar Heat Capacity H2O(1) = 75.3 JK' moi? H2O(g) = 36.4 JK' mol Enthalpy of Vaporization at 100 °C = 40.7 kJ mol .-1 -1 Answer:
rams of ethanol (C2HSOH) from-120.0 C to 85.0 4. How much energy is needed to convert 25.0 g °C? 25 points molar heat capacity (solid) = 1 1 1 .46 J/mol*K molar heat capacity(liquid) 112.4 J/mol*K molar heat capacity(gas)- 78.28 J/mol*K heat of fusion 4.9 KJ/mol heat of vaporization = 38.56 KJ/mol melting point--114.1 C boiling point-783 C
The normal molar vaporization enthalpy (∆H_Vap ^ °) of methanol is worth 37.4 kJmol ^ (- 1), and its normal molar vaporization entropy (∆S_Vap ^ °) 110.9 JK ^ (- 1) mol ^ (- 1). Calculate: The vapor pressure of methanol, at 298 K (R = 8.3144 J K -1 mol -1). The approximate normal boiling point. The boiling point for an external pressure of 0.1 atm. Applying the Clausius-Clapeyron equation, estimate the cooking temperature in a pressure cooker whose...
5. Calculate the heat (in kJ) required to transform 70.80 g of bromine from a solid at a temperature of -7.2 °C to a gas at 92 °C. Report your answer to one decimal place. Data: Molar mass of bromine, Br 2 = 159.808 g/mol Melting point = -7.2 °C Boiling point = 59°C. Enthalpy of fus ion = 10.57 kJ/mol Enthalpy of vaporization = 29.96 kJ/mol. Molar heat capacity of the liquid phase = 75.7 J/mol • K Molar...
A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by the reaction ATP(aq) + H,O(1) ADP(aq) + HPO- (aq) for which AG = -30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of AG xn in a biological cell in which [ATP] = 5.0 mm, (ADP) = 0.10 mM, and (HPO 1 - 5.0 mM. AG...