alpy: Heat of Neutralızation Prelaboratory Questions Name Laboratory Section 1. The The temperature 18.2°C. How much heat (in ) has been absorbed by the metal? of a 15.0 g sample of a metal (specific heat 0.040 J/g-°C) is raised by 2. A calorimeter and its contents have a heat capacity of 70 J/°C. A reaction occurs in this calorimeter at atmospheric pressure. The temperature of the system rises 10.5°C when one mole of product is formed. Calculate the heat change for this reaction. o 3. If 100 g of a solution (specific heat of 0.32 J/g-°C) undergoes a reaction in which 74.84 J of heat is released, what is the temperature change (AT) of this solution? Does the tem- perature of the solution increase or decrease? 4 30.0 g of a substance (molar mass: 46 g/mol) required 262J of heat to raise its temperature from 32.0 to 37.4°C. What is the specific heat per gram and per mole of this substance? (continued on next page) 125

alpy: Heat of Neutralızation Prelaboratory Questions Name Laboratory Section 1. The The temperature 18.2°C. How much heat (in ) has been absorbed by the metal? of a 15.0 g sample of a metal (specific heat 0.040 J/g-°C) is raised by 2. A calorimeter and its contents have a heat capacity of 70 J/°C. A reaction occurs in this calorimeter at atmospheric pressure. The temperature of the system rises 10.5°C when one mole of product is formed. Calculate the heat change for this reaction. o 3. If 100 g of a solution (specific heat of 0.32 J/g-°C) undergoes a reaction in which 74.84 J of heat is released, what is the temperature change (AT) of this solution? Does the tem- perature of the solution increase or decrease? 4 30.0 g of a substance (molar mass: 46 g/mol) required 262J of heat to raise its temperature from 32.0 to 37.4°C. What is the specific heat per gram and per mole of this substance? (continued on next page) 125

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter10: Energy

Section: Chapter Questions

Problem 44QAP: When ethanol (grain alcohol, is burned in oxygen, approximately 1360 kJ of heat energy is released...

See similar textbooks

Similar questions

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 reaction of 50 mL of acid and 50 mL of base described in Example 5.5 increased the temperature of the solution by 6.9 degrees C. How much would the temperature have increased if loo mL of acid and 100 mL of base had been used in the same calorimeter starting at the same temperature of 22.0 C? Explain your answer.
When hydrazine reacts with oxygen, nitrogen gas and steam are formed. (a) Write a thermochemical equation for the reaction. (b) How much heat is evolved or absorbed if 1.683 L of steam at 125C and 772 mm Hg are obtained?
Equal masses of liquid A, initially at 100C, and liquid B, initially at 50C, are combined in an insulated container. The final temperature of the mixture is 80C. All the heat flow occurs between the two liquids. The two liquids do not react with each other. Is the specific heat of liquid A larger than, equal to, or smaller than the specific heat of liquid B?
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.
Carbon tetrachloride, CCl4, is a liquid used as an industrial solvent and in the preparation of fluorocarbons. What is the heat of vaporization of carbon tetrachloride? CCl4(l)CCl4(g);H=? Use standard enthalpies of formation (Table 6.2).
How much heat is produced by combustion of 125 g of methanol under standard state conditions?
A7.50-gpiece of iron at 100.0C is dropped into 25.0g of water at 22.0C. Assuming that the heat lost by the iron equals the heat gained by the water,determine thefinal temperature of the iron/watersystem. Assume a heat capacity of water at 4.18 J/g.K and of iron at 0.452J/g.K.
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?
9.45 What happens to the temperature of a material as it undergoes an endothermic phase change? If heat is added, how can the temperature behave in this manner?
A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g water at 23.5C. After the metal cools, the final temperature of metal and water mixture is 25.0C. If the specific heat capacity of nickel is 0.444 J/C g, what mass of nickel was originally heated? Assume no heat loss to the surroundings.
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?