Useful Data and Formulae: Cp water = 4.2 kJ kg-1 K-1 Specific volume of water at 35°C = 0.001006 m³ kg-1 Cp steam = 2.0 kJ kg-1 K-1. Enthalpy of vaporization of water at 100°C = 2257 kJ kg-1 Molar mass of water = 18.01 Density of steam at 175°C = 4.66 kg m3. Standard free energies of formation: Substance HCl(g) O2(g) Cl2(g) H2O(g) AG (kJ mol-1) -95.299 -228.59 QUESTION 1 (a) Write the thermochemical equation for the formation of 1 mole of solid sodium bicarbonate, NaHCO3(s), from its elements. (b) Use the following information to calculate the standard enthalpy of formation of NaHCO 3(s): (i) AH, of CO2(g) = - 393.51 kJ mol-1 (ii) AH, of NaOH(s) = -425.61 kJ mol-1 (iii) NaOH() +CO2(g) → NaHCO3{s) AH = -127.5 kJ mol¬

Useful Data and Formulae: Cp water = 4.2 kJ kg-1 K-1 Specific volume of water at 35°C = 0.001006 m³ kg-1 Cp steam = 2.0 kJ kg-1 K-1. Enthalpy of vaporization of water at 100°C = 2257 kJ kg-1 Molar mass of water = 18.01 Density of steam at 175°C = 4.66 kg m3. Standard free energies of formation: Substance HCl(g) O2(g) Cl2(g) H2O(g) AG (kJ mol-1) -95.299 -228.59 QUESTION 1 (a) Write the thermochemical equation for the formation of 1 mole of solid sodium bicarbonate, NaHCO3(s), from its elements. (b) Use the following information to calculate the standard enthalpy of formation of NaHCO 3(s): (i) AH, of CO2(g) = - 393.51 kJ mol-1 (ii) AH, of NaOH(s) = -425.61 kJ mol-1 (iii) NaOH() +CO2(g) → NaHCO3{s) AH = -127.5 kJ mol¬

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter9: Liquids, Solids, And Materials

Section: Chapter Questions

Problem 98QRT

See similar textbooks

Similar questions

Suppose 50.0 g of superheated Na(s) melts at 500 K and 1 bar pressure. Find the ΔSsys, ΔSsurr, and \ΔSuniv in J/K and round the answer to the hundredths place. Thermodynamic Data for Sodium Property Value Tfus 371 K ΔfusH0 at T_{fus}Tfus 2.60 kJ/mol Cp,m0(l) at 298 K 32.7 J K-1 mol-1 Cp,m0(s) at 298 K 28.2 J K-1 mol-1 Assume heat capacities are independent of temperature.
For SO2 melting and boiling points are 198 K and 263 K respectively. Cp values for solid phase are 1.255 J/mol-K at 15 K and 84.185 J/mol-K for greater than 15 K. Cp values for liquid phase is 24.937 J/mol-K. For gas phase Cp = 49.769 + 4.56*10 TJ/mol-k where T is in K. Enthalpy of freezing and condensation processes are -7.402 kJ/mol and-24.937 kJ/mol respectively. Determine specific entropy of SO2 at 400 K. Image of question attached.
normal boiling point of C2Cl3F3 (MW=187.4) is 47.6oC. The specific heats for the liquid and gas are 0.91 J/gK and 0.67 J/gK, respectively. Calculate the heat required to convert 25.0 g of C2Cl3F3 from a liquid at 5.00oC to a gas at 82.00oC if ΔvapH = 27.49 kJ/mol.
What is the enthalpy change for heating ice from 266 K to steam at 378 K? Assume Cp = 37.7 J K-1 mol-1 for ice and steam and Cp = 75.3 J K-1 mol-1, delvapHo373 = 40.656 J mol-1, and delfusHo273 = 6008 J mol-1 Notes:answer in KJ/mol.
Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°CSpecific heat capacity (liquid): 2.161 J/g°CSpecific heat capacity (gas): 1.291 J/g°C How much heat is involved in taking 165.2 g of acetone from 14.7°C to 52.1°C?
If a particular liquid has a normal boiling point of 338.0 K and a vapor pressure of 75.0 mmHg at 285.0 K, determine ∆Hvap for the liquid.
The vapor pressure of 1-chlorotetradecane at several temperatures are tabulated below. T (ºC) P∗ mm Hg 98.5 1 131.8 5 148.2 10 166.2 20 199.8 60 215.5 100 Use the calculated values for ln(P∗)ln(P∗) to estimate the vapor pressure at 185°C.
The melting point of sodium is 370.6 K at 1 atm pressure. Under these conditions, the molar volumes of solid and liquid sodium are 24.18 and 24.78 cm3 mol-1, respectively. The standard enthalpy of fusion of sodium at 370.6 K is 3.05 kJ mol-1. Calculate the melting point of sodium at 135 atm pressure.Answer should be 371.6 K
The enthalpy of fusion of water is 6.01 kJ/mol. Sunlightstriking Earth’s surface supplies 168 W per square meter(1 W = 1 watt = 1 J/s). (a) Assuming that melting of iceis due only to energy input from the Sun, calculate howmany grams of ice could be melted from a 1.00 squaremeter patch of ice over a 12-h day. (b) The specific heatcapacity of ice is 2.032 J/g °C. If the initial temperature ofa 1.00 square meter patch of ice is -5.0 °C, what is its finaltemperature after being in sunlight for 12 h, assuming nophase changes and assuming that sunlight penetrates uniformlyto a depth of 1.00 cm?
Substance W (MW = 122.00 g/mol) melts at -10.0 oC and boils at 110.0 oC. How muchenergy is needed to heat a solid 12.54 g sample from -10.0 oC to 20 oC? Potentially usefulinformation: Hfusion = 12.3 kJ/mol, specific heat = 6.45 J/g oC and Hvap = 49.7 kJ/mol.
Determine the amount of heat, in kJ, required to heat 100.0 g of liquid Ca at 851C to 951C.Melting Point = 851C Boiling Point = 1487CMolar Heat CapacitiesC = 26.2 J/molCC = 31.0 J/molCΔH = 9.33 kJ/molΔH = 162 kJ/mol
Polymer PXX has a glass transition temperature of 49°C. What is the typical appearance and mechanical behaviour of this polymer PXX?