None 4. A 23.4 g piece of ice at -12.1 °C is placed into a container with 5.62 g of steam at 102.4 °C. What is the niwe10.8temperature once the ice and steam achieve thermal equilibrium?Cice 2.11 J/gK Cwater = 4.18 J/gK=Csteam = 2.08 J/gk AHfus 6.02 kJ/mol=AHvap 40.7 kJ/mol anser Aestaduadear to Isvome no fungewied ni egner seg eritritivallwow -05-16 grimal jugui tser to noltonul 8 26 9 29agreed at wala colomexbos antog gnitioniter & inoltulobugil sislupils mont gaiandawanmet ozish the tort bilozidwintog gailiod sa

Step 1: Calculate the energy required to heat the ice to 0°C.Mass of ice: 23.4 gInitial temperature:…

Answered: 4. A 23.4 g piece of ice at -12.1 °C is…

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 109AE: A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g...

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Similar questions

A student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at room temperature (22.5C) to vapor at 59.0C.To do this, one must use Tables 8.1 and 8.2 for information on the specific heat, boiling point, and heat of vaporization of bromine. In addition, the following step-wise process must be followed. (a) Calculate H for: Br2(l,22.5C)Br2(l,59.0C) (b) Calculate H for: Br2(l,59.0C)Br2(g,59.0C) (c) Using Hess's law, calculate H for: Br2(l,22.5C)Br2(g,59.0C)
Which evolves more heatâ€”freezing 100.0 g of benzene or 100.0 g of bromine?
When steam condenses to liquid water, 2.26 kJ of heat is released per gram. The heat from 168 g of steam is used to heat a room containing 6.44 104 g of air (20 ft 12 ft 8 ft). The specific heat of air at normal pressure is 1.015 J/(gC). What is the change in air temperature, assuming the heat from the steam is all absorbed by air?
9.49 Hvap=31.3 kJ/mol for acetone. If 1.40 kg of water were vaporized to steam in a boiler, how much acetone (in kg) would need to be vaporized to use the same amount of heat?
The addition of 3.15 g of Ba(OH)28H2O to a solution of 1.52 g of NH4SCN in loo g of water in a calorimeter caused the temperature to fall by 3.1 C. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat absorbed by the reaction, which can be represented by the following equation: Ba(OH)28H2O(s)+2NH4SCN(aq)Ba(SCN)2(aq)+2NH3(aq)+10H2O(l)
The enthalpy change when 1 mol methane (CH4) is burned is 890 kJ. It takes 44.0 kJ to vaporize 1 mol water. What mass of methane must be burned to provide the heat needed to vaporize 1.00 g water?
9.38 The energy densities of various types of coal are listed below: Anthracite 35 kJ/g Subbituminous 31 kJ/g Bituminous 28 kJ/g Lignite 26 kJ/g An unknown sample of one of these coals is burned in an apparatus with a calorimeter constant of 1.3 kJ/°C. When a 0.367-g sample is used, the temperature change is 8.75°C. Which type of coal is the sample?
How much will the temperature of a cup (180 g) of coffee at 95 C be reduced when a 45 g silver spoon (specific heat 0.24 J/g C) at 25 C is placed in the coffee and the two are allowed to reach the same temperature? Assume that the coffee has the same density and specific heat as water.
An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g)+3O2(g)2H2O(l)+2SO2(g);H=1124kJ The density of sulfur dioxide at 25C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/(mol C). (a) How much heat would be evolved in producing 1.00 L of SO2 at 25C and 1.00 atm? (b) Suppose heat from this reaction is used to heat 1.00 L of the SO2 from 25C to 500C for its use in the next step of the process. What percentage of the heat evolved is required for this?
9.47 If 14.8 kJ of heat is given off when 1.6 g of HCl condenses from vapor to liquid, what is Hcond for this substance?
9.68 What are some features of petroleum that make it such an attractive fuel?
The enthalpy of combustion of CH4(g) when H2O(l) is formed is 891 kJ/mol and the enthalpy of combustion of CH4(g) when H2O(g) is formed is 803 kJ/mol. Use these data and Hesss law to determine the enthalpy of vaporization for water.

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