Please give me right answer The following information is given for copper atlatm:AHvap(2567 °C)= 305boiling point = 2567 °CkJ/molAHfus(1083 °C) = 13.0melting point1083 °C%3DkJ/molspecific heat solid=0.385 J/g°Cspecific heat liquid0.494 J/g°CWhat is AH in kJ for the process of freezing a 21.1g sample of liquid copper at its normal meltingpoint of 1083 °C.kJ

Boiling point of copper= 2567 °C ∆HVap = 305 KJ/molMelting point of copper = 1083…

The following information is given for copper at 1atm: AHvap(2567 °C) = 305 %3D boiling point 2567 °C %3D kJ/mol AHfus(1083 °C) = 13.0 melting point = 1083 °C kJ/mol specific heat solid= 0.385 J/g°C specific heat liquid 0.494 J/g°C What is AH in kJ for the process of freezing a 21.1 g sample of liquid copper at its normal melting point of 1083 °C. kJ

The following information is given for copper at 1atm: AHvap(2567 °C) = 305 %3D boiling point 2567 °C %3D kJ/mol AHfus(1083 °C) = 13.0 melting point = 1083 °C kJ/mol specific heat solid= 0.385 J/g°C specific heat liquid 0.494 J/g°C What is AH in kJ for the process of freezing a 21.1 g sample of liquid copper at its normal melting point of 1083 °C. kJ

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section4.5: Energy And Enthalpy

Problem 4.6PSP

See similar textbooks

Similar questions

The following information is given for lead at 1 atm: boiling point = 1.740×103 °C Hvap(1.740×103 °C) = 858.2 J/g melting point = 328.0 °C Hfus(328.0 °C) = 23.00 J/g specific heat solid = 0.1300 J/g°C specific heat liquid = 0.1380 J/g°C A 29.30 g sample of liquid lead at 496.0 °C is poured into a mold and allowed to cool to 26.0 °C. How many kJ of energy are released in this process. Report the answer as a positive number. __________ kJ
To vaporize 100.0 g carbon tetrachloride at its normal boiling point, 349.9 K, and P =1 atm, 19.5 kJ of heat is required. Calculate DHvap for CCl4 and compare it with DU for the same process.
After the sinking of RMS Titanic, US operated the International Ice patrolwith the purpose of monitoring the presence and movements of icebergsin the Atlantic and Arctic oceans. Once, they observed a unique tabulariceberg in a form of a rectangle (250 km x 50 km x 300 m). How manyyears would it take to melt the iceberg solely by heat from the sun if theice absorbs a mean of 98 J/m2-s, 12.5 hrs per day? Note: the exposed area for heating is 250 km x 50 km and the density is 920 kg/m3.
a copper container of mass 500 g and contains 1 litre of water at293 K. Prove that the quantity of heat which can be obtained will be ableto raise the temperature of the water in the container to a boiling pointif there are no heat losses. Assume that the specific heat capacity ofcopper is 390 J/(kg K), the specific heat capacity of water is 4.2 kJ/(kg K)and 1 litre of water has a mass of 1 kg.
A 41.90 g sample of solid bismuth is initially at 248.00°C. If the sample is heated at constant pressure ( = 1 atm), _____________ kJ of heat are needed to raise the temperature of the sample to 629.00°C. tb=1627 C Hvap=822.9 j/g tm=271 C Hfus=52.60 specific heat solid= 0.1260 j/g specfifc heat liquid= 0.1510 j/g
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.
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.
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?
A pure solid has two crystal forms: α and β, and is under transformation from α to β at 1 atm and 25 oC. At 1 atm and 25 oC, the molar enthalpy (or heat) of transformation is ∆Hmo(α à β) = - 0.57 kJ/mol. The internal energy change at 1 atm and 25 oC is ∆Umo(α à β) = - 0.43 kJ/mol. Which of the following statements is TRUE for the density between these two crystal forms? The dentistry of solid α is equal to the dentistry of solid β. The dentistry of solid α is less than the dentistry of solid β. The dentistry of solid α is greater than the dentistry of solid β. Insufficient information to find the density relation between the two types of solid.
The pressures deep within the Earth are much greater than those on the surface, and to make use of thermochemical data in geochemical assessments you need to take the differences into account. (a) Given that the enthalpy of combustion of graphite is -393.5 kJ mol-1 and that of diamond is -395.41 kJ mol-1, calculate the standard enthalpy of the C(s, graphite) → C(s, diamond) transition. (b) The densities of graphite and diamond are 2.250 g cm-3 and 3.510 g cm-3 , respectively. Calculate the internal energy of the transition when the sample is under a pressure of 150 kbar.
Liquid ammonia (boiling point = –33.4°C) can be used as a refrigerant and heat transfer fluid. The amount of energy needed to heat 25.0 g of NH3(l) from –65.0°C to –12.0°C is to be calculated.
Calculate the heat required to bring 10.0 g CCl2F2 from -29.8 °C as a liquid to the gas phase at 10.0 °C. (molar mass = 120.91 g/mol) Cs (gas) = 0.074 kJ/mol·K ΔHvap = 20.1 kJ/mol ΔHfus = 4.14 kJ/mol