28. The reaction of 50 mL of acid and 50 mL of base described in Example 5.5 increased the temperature of thesolution by 6.9 degrees C. How much would the temperature have increased if 100 mL of acid and 100 mL of basehad been used in the same calorimeter starting at the same temperature of 22.0 °C? Explain your answer. For context, here is Example 5.5:Example 5.5Heat Produced by an Exothermic ReactionWhen 50.0 mL of 1.00 M HCI(aq) and 50.0 mL of 1.00 M NAOH(aq), both at 22.0 °C, are added to a coffeecup calorimeter, the temperature of the mixture reaches a maximum of 28.9 °C. What is the approximateamount of heat produced by this reaction?HСC(ag) + NaOН(ад) —NaCl(aq) + H2O(1)SolutionTo visualize what is going on, imagine that you could combine the two solutions so quickly that no reactiontook place while they mixed; then after mixing, the reaction took place. At the instant of mixing, you have100.0 mL of a mixture of HCl and NaOH at 22.0 °C. The HCl and NaOH then react until the solutiontemperature reaches 28.9 °C.The heat given off by the reaction is equal to that taken in by the solution. Therefore:9 reaction =-9 solution(It is important to remember that this relationship only holds if the calorimeter does not absorb any heatfrom the reaction, and there is no heat exchange between the calorimeter and the outside environment.)Next, we know that the heat absorbed by the solution depends on its specific heat, mass, and temperaturechange:9 solution = (c Xmx AT)olutionTo proceed with this calculation, we need to make a few more reasonable assumptions or approximations.Since the solution is aqueous, we can proceed as if it were water in terms of its specific heat and massvalues. The density of water is approximately 1.0 g/mL, so 100.0 mL has a mass of about 1.0 x 102 g (twosignificant figures). The specific heat of water is approximately 4.184 J/g °C, so we use that for the specificheat of the solution. Substituting these values gives:9 solution = (4.184 J/g °C)(1.0x 10 g)(28.9 °C- 22.0 °C) = 2.9 x 10 JFinally, since we are trying to find the heat of the reaction, we have:9reaction - solution =-2.9x 10 JThe negative sign indicates that the reaction is exothermic. It produces 2.9 kJ of heat.Check Your LearningWhen 100 mL of 0.200 M NaCl(ag) and 100 mL of 0.200 M AGNO3(aq), both at 21.9°C, are mixed ina coffee cup calorimeter, the temperature increases to 23.5 °C as solid AgCl forms. How much heat isproduced by this precipitation reaction? What assumptions did you make to determine your value?Answer: 1.34 x 10 J; assume no heat is absorbed by the calorimeter, no heat is exchanged between thecalorimeter and its surroundings, and that the specific heat and mass of the solution are the same as those forwater

Given: Volume of acid used = 50 mL Volume of base used = 50 mL And change in temperature of solution…

28. 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 100 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.

28. 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 100 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.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Simple Calorimetry. A piece of solid aluminum at 15.0°C is immersed in 12.3 g of nitrogen gas which is initially at 51.1°C and the system is allowed to equilibrate. Given that the specific heat of solid aluminum is 0.908 J/K/g and the specific heat of nitrogen gas is 1.0 J/K/g, what is the mass of the piece of solid aluminum if the final temperature is 34.7°C?
A 1.261 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 25.39 °C to 28.44 °C. The heat capacity (calorimeter constant) of the calorimeter is 27.69 kJ/ °C, what is the heat of combustion per gram of the material? heat of combustion: kJ/g
In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.00 mL of 1.00 M HCl are mixed. Both solutions were originally at 24.6 C. After the reaction, the final temperature is 31.3 C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87, calculate the change in enthalpy of neutralization per mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.
6 8 7. Consider the following reaction: 2 CH;OH (g) → 2 CH4() O2 (g), AH = + 252.8 kJ a) Is this reaction exothermic or endothermic? b) Calculate the amount of heat transferred when 26.0 g of CH3OH(g) is decomposed by this reaction at constant pressure. Express the heat to three significant digits with the appropriate units. c) For a given sample of CH;OH, the enthalpy change during the reaction is 82.9 kJ. What mass of methane gas is produced? Express the mass to three significant digits with the appropriate units. d) How many kilojoules of heat are released when 38.8 g CH4(g) reacts completely with 02(g) to form CH,OH(g) at constant pressure?
2. A calorimeter contains 100.0 g of water at 39.8 °C. A 12.78 g object at 100.0 ºC is placed inside the calorimeter. When equilibrium has been reached, the new temperature of the water and metal object is 40.6 °C. What is the specific heat of the metal?
5. When 1.00g of NaCl (MM 58.44 g/mol) is dissolved in 50.00g of water, the temperature drops by 0.319°C. This temperature change is only detectable by the most sensitive thermometers. If this process takes place in a very well insulated calorimeter, no calorimeter constant is needed. a. Calculate the enthalpy change per gram of NaCl. b. Calculate the enthalpy change per mole of NaCl.
A chemical reaction takes place in an open flask. The reaction releases 355 kJ of heat and does 25 kJ of work on the surroundings. Is the reaction endothermic or exothermic? Calculate ΔH for the reaction. Calculate ΔU for the reaction.
4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6
To measure the enthalpy of an acid-base reaction, a student places the thermometer in the hydrochloric acid solution, and then, without rinsing with DI water, places it in the sodium hydroxide solution prior to adding the hydrochloric acid solution to the calorimeter. How would this affect the calculated enthalpy of the reaction, be too high, too low, or unaffected? Why?
A 3.915 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 23.51 °C to 27.32 °C. The heat capacity (calorimeter constant) of the calorimeter is 26.61 kJ/ °C, what is the heat of combustion per gram of the material? heat of combustion: kJ/g
12. When 30.0 mL of 1.00 M HCl(aq) and 45.0 mL of 1.00 M NaOH(aq), both at 21.0 °C, are added to a coffee cup calorimeter, the temperature of the mixture reaches a maximum of 24.0° What is the amount of heat produced by this reaction? The mixture has a specific heat of 4.184 J/g °C and density of 1g/mL. Show work and write your answers in 4 significant figures. Box in your final answer. HCl(aq) + NaOH(aq) --> NaCl(aq) + H₂O(1)
22. A 44.97−g sample of water at 72.2°C is added to a sample of water at 25.7°C in a constant-pressure calorimeter. If the final temperature of the combined water is 38.4°C and the heat capacity of the calorimeter is 26.3 J/°C, calculate the mass of the water originally in the calorimeter.