Use the following information to answer the next questionFructose is a sugar molecule that has the chemical formula C6H12O6(S). A studentburned 1.30 g of fructose to heat 236 g of water according to the reaction below.C6H12O6(S) +6 O₂(g) →6 CO2(g) + 6 H₂O(g)The initial temperature of the water was 21.3 °C and after the sugar reacted thetemperature was 41.1 °C.From the information above, determine the molar enthalpy of combustion forfructose.Your answer

we have to calculate the molar enthalpy for combustion of fructose using the given information

4. Use the following information to answer the next question Fructose is a sugar molecule that has the chemical formula C6H12O6(S). A student burned 1.30 g of fructose to heat 236 g of water according to the reaction below. C6H12O6(S) +6 O₂(g) →6 CO₂(g) + 6 H₂O(g) The initial temperature of the water was 21.3 °C and after the sugar reacted the temperature was 41.1 °C. From the information above, determine the molar enthalpy of combustion for fructose.

4. Use the following information to answer the next question Fructose is a sugar molecule that has the chemical formula C6H12O6(S). A student burned 1.30 g of fructose to heat 236 g of water according to the reaction below. C6H12O6(S) +6 O₂(g) →6 CO₂(g) + 6 H₂O(g) The initial temperature of the water was 21.3 °C and after the sugar reacted the temperature was 41.1 °C. From the information above, determine the molar enthalpy of combustion for fructose.

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

Section: Chapter Questions

Problem 106QRT

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You have two samples of different metals, metal A and metal B, each having the same mass. You heat both metals to 95C and then place each one into separate beakers containing the same quantity of water at 25C. a You measure the temperatures of the water in the two beakers when each metal has cooled by 10C and find that the temperature of the water with metal A is higher than the temperature of the water with metal B. Which metal has the greater specific heat? Explain. b After waiting a period of time, the temperature of the water in each beaker rises to a maximum value. In which beaker does the water temperature rise to the higher value, the one with metal A or the one with metal B? Explain.
Sulfur dioxide gas reacts with oxygen, O2(g), to produce SO3(g). This reaction releases 99.0 kJ of heat (at constant pressure) for each mole of sulfur dioxide that reacts. Write the thermochemical equation for the reaction of 2 mol of sulfur dioxide, and then also for the decomposition of 3 mol of sulfur trioxide gas into oxygen gas and sulfur dioxide gas. Do you need any other information to answer either question?
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).
The temperature of the cooling water as it leaves the hot engine of an automobile is 240 F. After it passes through the radiator it has a temperature of 175 F. Calculate the amount of heat transferred from the engine to the surroundings by one gallon of water with a specific heat of 4.184 J/g oC.
Consider the following specific heats of metals. Metal Specific Heat copper 0.385 J/(gC) magnesium 1.02 J/(gC) Mercury 0.138 J/(gC) Silver 0.237 J/(gC) Four 25-g samples, one of each metal, and four insulated containers with identical water volumes, all start out at room temperature. Now suppose you add exactly the same quantity of heat to each metal sample. Then you place the hot metal samples in different containers of water (that all have the same volume of water). Which of the answers below is true? a The water with the copper will be the hottest. b The water with the magnesium will be the hottest. c The water with the mercury will be the hottest. d The water with the silver will be the hottest. e The temperature of the water will be the same in all the cups.
A 15.5-g piece of chromium, heated to 100.0 C, is dropped into 55.5 g of water at 16.5 C. The final temperature of the metal and the water is 18.9 C. What is the specific heat capacity of chromium? (Assume no energy is lost to the container or to the surrounding air.)
You drink 350 mL of diet soda that is at a temperature of 5 C. (a) How much energy will your body expend to raise the temperature of this liquid to body temperature (37 C)? Assume that the density and specific heat capacity of diet soda are the same as for water. (b) Compare the value in part (a) with the caloric content of the beverage. (The label says that it has a caloric content of 1 Calorie.) What is the net energy change in your body resulting from drinking this beverage? (1 Calorie = 1000 kcal = 4184 J.) (c) Carry out a comparison similar to that in part (b) for a nondiet beverage whose label indicates a caloric content of 240 Calories.
A sample of sucrose, C12H22O11, is contaminated by sodium chloride. When the contaminated sample is burned in a bomb calorimeter, sodium chloride does not burn. What is the percentage of sucrose in the sample if a temperature increase of 1.67C is observed when 3.000 g of the sample are burned in the calorimeter? Sucrose gives off 5.64103kJ/mol when burned. The heat capacity of the calorimeter and water is 22.51 kJ/C.
Three 45-g ice cubes at 0 C are dropped into 5.00 102 mL of tea to make iced tea. The tea was initially at 20.0 C; when thermal equilibrium was reached, the final temperature was 0 C. How much of the ice melted, and how much remained floating in the beverage? Assume the specific heat capacity of tea is the same as that of pure water.
Copper is used in building the integrated circuits, chips, and printed circuit boards for computers. When 228 J of heat are absorbed by 125 g of copper at 22.38C, the temperature rises to 27.12C. What is the specific heat of copper?
A 500-mL bottle of water at room temperature and a 2-L bottle of water at the same temperature were placed in a refrigerator. After 30 minutes, the 500-mL bottle of water had cooled to the temperature of the refrigerator. An hour later, the 2-L of water had cooled to the same temperature. When asked which sample of water lost the most heat, one student replied that both bottles lost the same amount of heat because they started at the same temperature and finished at the same temperature. A second student thought that the 2-L bottle of water lost more heat because there was more water. A third student believed that the 500-mL bottle of water lost more heat because it cooled more quickly. A fourth student thought that it was not possible to tell because we do not know the initial temperature and the final temperature of the water. Indicate which of these answers is correct and describe the error in each of the other answers.
Alloys When a 58.8-g piece of hot alloy is placed in125 g of cold water in a calorimeter, the temperature ofthe alloy decreases by 106.1°C, while the temperature ofthe water increases by 10.5°C. What is the specific heat ofthe alloy?

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