Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Calculate the mass of methanol when burned in oxygen (assuming complete combustion), required to give a heat output of 2200 kJ. Take the molar mass of methanol to be 32 g mol^-1arrow_forwardThere are two steps in the usual industrial preparation of acrylic acid, the immediate precursor of several useful plastics. In the first step, calcium carbide and water react to form acetylene and calcium hydroxide: CaC,(s) + 2 H,O(g9) → C,H,(9) + Ca(OH),(s) AH=-414. kJ In the second step, acetylene, carbon dioxide and water react to form acrylic acid: 6 C,H,(9) + 3 CO,(g) + 4 H,O(g) → 5 CH, CHCO,H(9) AH=132. kJ Calculate the net change in enthalpy for the formation of one mole of acrylic acid from calcium carbide, water and carbon dioxide from these reactions. Round your answer to the nearest kJ.arrow_forwardA 148 g sample of an unknown metal at 74.0 oC is placed in a beaker containing 80.0 g of H2O at 25 oC. The final temperature of the metal sample and water is 32 oC. cH2O(l) = 4.184 j/ g oC SHOW ALL WORK (a) What is the specific heat (c) of the metal? (b) 5 common metals have the following specific heat capacities (c) [given in units of J/g oC] : Aluminum: 0.921 Copper: 0.377 Gold: 0.126 Iron: 0.461 Nickel: 0.502 Your sample is most likely to be which metal?arrow_forward
- A student has a coffee-cup calorimeter with 50.0 g of water at 21.5oC. They introduce 15.525 g of magnesium metal initially at 100.0oC. The final temperature of the calorimeter came to 27.2oC. What is the sensible heat change of magnesium, q magnesium , in joules?arrow_forwardA coffee cup calorimeter contains 156.56 g of water at 22.50 °C. A 66.065 g piece of iron is heated to 101.17 °C. The piece of iron is added to the coffee cup caloriemter and the contents reach thermal equilibrium at 25.68 °C. The specific heat capacity of iron is 0.449 and the specific heat capacity of water is 4.184 How much heat, q, is lost by the piece of iron? Fire = How much heat, q, is gained by the water? qwater = Ccalorimeter = The difference between the heat lost by the piece of iron and the heat gained by the water is due to heat transfer to the styrofoam and the heat required to raise the temperature of the calorimeter. What is the heat capacity of the styrofoam calorimeter in joules per kelvin (*)? What would be the final temperature of the system if all of the heat lost by the iron was absorbed by the water? Tinal J = J °Carrow_forwardAn experiment is performed in the chemical lab, 405 J of heat is absorbed by a system and 285 J of work is done by the system. What is the change in internal energy for the process?arrow_forward
- 2. In studying the energy generated by a person, you may view the person roughly as a constant pressur calorimeter using sugar (i.e., sucrose, C₁2H₂2O11) to generate power. The reaction of table sugar in calorimeter is given by + Ch. 9 Sl....pdf C12H22O11(s)+120₂(g) →12CO₂(g)+11H₂O+heat. C. a. What is the heat released by consuming one mole of sugar (C₁2H22O11) in this b. Calculate the enthalpy of combustion per sugar utilization. mole Does the result of your calculation make I wi (540 Karak 14 11 M de 2009 1 AP fik Tour of 1 way? 20arrow_forwardDuring a certain chemical reaction 255 J of heat is absorbed by the system and 275 J of work is done on the surroundings. Calculate the change in internal energy of the system. Do not type units with your answer. Your Answer:arrow_forwardA system does 501 kJ of work and loses 216 kJ of heat to the surroundings. What is the change in internal energy, AE, of the system? Note that internal energy is symbolized as AU in some sources. AE = kJarrow_forward
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