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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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If 75.4 J of energy is absorbed by 0.25 mol of CCl4 at constant pressure, what is the change in temperature? The specific heat of CCl4 is 0.861 J/g·°C. |
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- 5.00 g of potassium hydroxide (molar mass = 56.1 g/mol) dissolves in 100.0 g of water and the temperature of the solution increases by 1.60oC. Calculate ΔH for the reaction in kJ/mol of KOH .The specific heat capacity of the solution is 4.18 J/goC ( Hint: the mass of the solution is 105g) (Hint #2: is this + or -?) Your answer should be in kJ/mol and have 3 sig figsarrow_forward[2] When 1.045 g of CaO is added to 50.0 ml of water at 22.0 °C in a coffee-cup calorimeter, the temperature of the water increases to 29.3 °C. Assume that the specific heat and density of the solution is 4.184 J/g-°C and 1.00g/ml, respectively. The heat capacity of the calorimeter is 18.0 J/°C. Calculate AH for the reaction. CaO(s) + H2O(1) –→ Ca(OH)2(aq); AH =arrow_forwardAn electrical heater adds 25.3 kJ of heat to a constant-volume calorimeter. The temperature of the calorimeter rises by 4.55 °C. When 1.75 g of methanol is burned in the same calorimeter, the temperature increases by 7.14 °C. Calculate the molar energy of combustion of methanol. kJ/molarrow_forward
- The heat capacity of an object indicates how much energy that object can absorb for a given increase in that object's temperature. In a system in which two objects of different temperatures come into contact with one another, the warmer object will cool and the cooler object will warm up until the system is at a single equilibrium temperature. Note the difference between the terms molar heat capacity, which has units of J/(mol-K). and specific heat, which has units of J/(g-K). Remember to use 3 significant figures for all answers unless stated otherwise in the problem. Common issues with this problem involve entering units incorrectly into the answer field. Please check this help website for a refresher on how to enter units in Mastering Chemistry: http://help.pearsoncmg.com/mastering/student/standalone/TopicsStudent/acceptable units list.htm The margin of error is 2%. Part A A volume of 75.0 mL of H₂O is initially at room temperature (22.0 °C). A chilled steel rod at 2.00 °C is placed…arrow_forward3.76 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate AH, in kJ/mol, for the dissolution of MgSO4. (The specific heat of water is 4.184 J/g °C and the density of the water is 1.00 g/ mL). You can assume that the specific heat of the solution is the same as that of water.arrow_forwardCalculate the heat required to raise the temperature of a 50.0 g of water from 25.0 °C to 39.0 °C. (The specific heat capacity of water is 4.184 J·g–1·°C–1). A) 2.93 kJ B) 4.18 kJ C) 5.23 kJ D) 8.16 kJ 0.163 kJarrow_forward
- Energy in the amount of 5.0 J is added to 0.50 g pieces of aluminum, copper, and magnesium that are initially kept at 22 °C. The molar heat capacities of these metals are 24.3 J/(mol·°C), 24.5 J/(mol·°C), and 24.9 J/(mol·°C), respectively. Which piece of metal will have the highest temperature and what is that temperature?arrow_forwardWhen a 6.00 g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 3.74 kJ · K¯¹, the temperature decreases by 0.400 K. Calculate the molar heat of solution of KSCN. ΔΗsoln = kJ/molarrow_forward
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