What amount of heat (in kJ) is required to convert 21.3 g of an unknown liquid (MM = 83.21 g/mol) at 19.2 °C to a gas at 93.5 °C? (specific heat capacity of liquid = 1.58 J/g-°C; specific heat capacity of gas = 0.932 J/g °C; AHvap = 22.5 kJ/mol; normal boiling point, Tb = 57.3°C)

Heat capacities are usually given in terms of polynomial functions of temperature. Heat capacity of potassium permanganate in terms of temperature is given by:  Cp =4.6895+6.231x10-3T+1.187x10-6T2  Where T is expressed in  degree F and CP=BTU(lb-mol-degree F) Modify the formula so that the resulting expression has the asssociated units of J/(g-mol-K) and T is in K.

Boiling Point Elevation/Freezing Point DepressionT = m KWhere: T = T(solution) - T(pure solvent) * m = (# moles solute / Kg solvent) Kb = boiling point elevation constant. Kf = freezing point depression constant. Kb and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow. Solvent Formula Kb (°C / m) Kf (°C / m) Water H2O 0.512 -1.86 Ethanol CH3CH2OH 1.22 -1.99 Chloroform CHCl3 3.67   Benzene C6H6 2.53 -5.12 Diethyl ether CH3CH2OCH2CH3 2.02   *Please note that ΔT as defined above will be a negative number for freezing point depression. Therefore, Kf must also be given as a negative number.

Suppose 1.000 mol argon (assumed to be an ideal gas) is confined in a strong, rigid container of volume 22.41 L at 273.15 K. The system is heated until 3.000 kJ (3000 J) of heat has been added. The molar heat capacity of the gas does not change during the heating and equals 12.47 J K-1 mol-1. (a) Calculate the original pressure inside the vessel (in atmospheres). (b) Determine q for the system during the heating process. (c) Determine w for the system during the heating process. (d) Compute the temperature of the gas after the heating, in degrees Celsius. Assume the container has zero heat сараcity. (e) Compute the pressure (in atmospheres) inside the ves- sel after the heating. (f) Compute AU of the gas during the heating process. (g) Compute AH of the gas during the heating process. (h) The correct answer to part (g) exceeds 3.000 kJ. The increase in enthalpy (which at one time was mislead- ingly called the “heat content") in this system exceeds the amount of heat actually added. Why…

17D.3. A sample of iron metal is cooled by 1000. g of water. The temperature of the water is raised from 23.0 °C to 30.1 °C. Before contact with the water, the temperature of the iron was 40.9 °C. What was the mass of the iron sample? The specific heat capacity of iron is 0.449 J/g⋅°C.(Assume the final temperature of the iron and water are the same.)

You have a calorimeter with 100 g of water at 22.6ᵒC and a 50.0 g piece of copper that you have heated to 98.7ᵒC. You place the copper in the water and wait for the temperature of the water to stop rising. What will be the highest temperature of the water? (Specific heats: water = 4.184 J/gᵒC, copper = 0.385 J/gᵒC )

How did this arrive from that value? Because when I tried to solve it manually, the value I get is 20.83...

What is the final temperature of a 200.00 gram sample of water (c = 4.18 J/g°C) that absorbs 5,000 Joules of heat energy after starting with a temperature of 20°C?