The heat capacity of gold (Au, 197 g mol-¹), is 25.0 J mol-¹ K-1. Calculate theenergy needed to heat 26.9 g of gold from 18.7 °C to 51.8 °C.O a. 2.23 x 104 JO b. 4.06 x 107 JO c. 4.39 x 106 JO d. 1.05 x10³ JO e. 1.13 x 10² J Using the data in the table below, which is the weakest base?AcidKaHCO34.7 x 10-11HOBr2.3 × 10-⁹CH3COOH1.7 x 10-5HF6.8 x 10-4HCIO3.0 × 10-8O a. CO3²O b. OBrO c. CH3COO™O d. FO e. Clo

Given that For goldmolar mass =197 gmolCp=25 Jmol K m =26.9 g T1 =18.7 CT2 =51.8 CAccording to…

Answered: The heat capacity of gold (Au, 197 g…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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One mol of an ideal gas is taken througha three-step cyclic process.The gas is subjected successively to an isothermal expansion at 600 K from 5 to 3 bar (path a to b), a constant-pressure cooling(b to c), and a constant-volume heating (c to a). All processes are reversible. ̄CV= 21.686J mol−1K−1and ̄Cp= 30J mol−1K−1. Calculate Q, W, ∆Uand∆Hfor each step and for the entire process. Drawthe cycle on the PV diagram.
This table displays the vapor pressure of nitrogen at several different temperatures. Use the data to determine the heat of vaporization and normal boiling point of nitrogen. Temperature (K) Pressure (torr) 65 130.5 70 289.5 75 570.8 80 1028 85 1718
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Whenever a substance is heated, its enthalpy increases, as suggested by the relation, ∆?=Cp∆?. However, the molar heat capacity itself is a function of temperature, and for N2 this function can be modeled as ?p(?)=? + ?? + c / T2 where a= 28.58 J/mol·K, b= 0.00377 J/mol·K2, and c= –5.0 x 104J·K/mol. (a) What does this formula for heat capacity predict for the value of ?p(?)at 300K? (b) Now, compute the enthalpy change associated with heating 0.62 moles of N2 from 300 to 600 K using the formula for ?p (?), and report the answer in J. (c) What is the difference between this value and one computed using the constant value for Cp at 300 K from part (a)? Report the absolute value of the difference in J.
Calculate AH for the change of state of 1.000 mol of helium from a volume of 5.000 L and a temperature of 298.15 K to a volume of 10.000 L and a temperature of 373.15 K. Assume that CP,m = 5R/2 and assume that the gas is ideal. Table A.6 Molar Heat Capacities Gases Cp,m = a + bT + cT-2 (Applicable between 298 K and 2000 K) Substance a/J K-l mol¬! b x 10°/J K-2 mol¬ c x 10-$/J K mol¬1 27.3 H2 O2 N2 CO 3.3 0.50 30.0 4.18 -1.67 28.6 3.8 4.1 8.79 10.3 -0.50 28.4 -0.46 CO2 H2O CH4 44.2 -8.62 30.5 23.6 47.86 -1.8
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Methane in a piston-cylinder assembly undergoes an adiabatic compression from an initial state (0.5 bar, 0.05 m³/mol) to a final state (10 bar, 3×10-³ m³/mol). Use the van der Waals equation of state to calculate the amount of work done on the system, in J/mol. Note that if ideal gas, the heat capacity of methane is given by Cp = 1.702 +9.081 × 10-³ T-2.164 x 10-6 T², where T is in K. R
2-Steam initially at 10 bar and 0.25 dryness fraction (i.e quality=85%.). Expands down to P₂= 3.5 bar According to the hyperbolic law. PV=Constant, Determine. 1. The final of the steam. 2- The change of temperature of the steam. 3. The work done kg during the change. 4 The change in internal energy. 5- The amount of heat supplied

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The heat capacity of gold (Au, 197 g mol-¹), is 25.0 J mol-1¹ K-¹. Calculate the energy needed to heat 26.9 g of gold from 18.7 °C to 51.8 °C. O a. 2.23 x 104 J O b. 4.06 x 107 J O c. 4.39 x 106 J O d. 1.05 × 10³ J O e. 1.13 x 10² J