The first step in the industrial recovery of zinc from zinc sulfide ore is roasting. That is the conversion of ZnS to ZnO by heating: 2ZnS (s) + 30₂(g) → 2ZnO(s) + 2SO₂ (g) kJ mol Calculate the heat (in kJ) associated with roasting 2.00 grams of zinc sulfide. Be sure your answer has the correct number of significant digits. kJ 0x10 ΔΗ= - 879

The first step in the industrial recovery of zinc from zinc sulfide ore is roasting. That is the conversion of ZnS to ZnO by heating: 2ZnS (s) + 30₂(g) → 2ZnO(s) + 2SO₂ (g) kJ mol Calculate the heat (in kJ) associated with roasting 2.00 grams of zinc sulfide. Be sure your answer has the correct number of significant digits. kJ 0x10 ΔΗ= - 879

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

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 2.30 kg of water at 35.8 °C. During the reaction 74.9 kJ of heat flows out of the bath and into the flask. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions 1 is 4.18 J.g •K`1 ▪ Be sure your answer has the correct number of significant digits.
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 9.70 kg of water at 38.3 °C. During the reaction 51.2 kJ of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18 J-g K. Be sure your answer has the correct number of significant digits. °C
A 0.2415 g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 3024 The temperature increases by 1.978 °C. Part 1 of 2 kJ Calculate the heat associated with the burning of Mg in Be sure your answer has the correct number of significant digits. g Part 2 of 2 kJ g ☐ x10 ☑ Calculate the heat associated with the burning of Mg in kJ mol Be sure your answer has the correct number of significant digits. KJ mol x10 ☑
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
A chemist carefully measures the amount of heat needed to raise the temperature of a 1.10kg sample of a pure substance from −6.3°C to 10.7°C . The experiment shows that 8.40kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.
Express the quantity in the unit indicated and designate whether this heat is gained or lost by the substance a. The quantity of heat in calories when 162.5 grams of water undergoes a temperature decrease from 45.84 C to 40.00 C. b. The quantity of heat in Kilojoules when 43.5 Kg of chloroform ,CHCl3 has its temperature changed from 16.8 C to 22.3 C ( sp ht of CHCl3 = 0.971 KJ/kg- C)
A chemist carefully measures the amount of heat needed to raise the temperature of a 500.0 mg sample of a pure substance from 21.7 °C to 37.6 °C. The experiment shows that 14.7 J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits. 圖 -K dh
A series of equal-mass samples of the five materials listed in the table are brought from room temperature to 100. °C. Which sample required the least amount of energy (J) to reach the final temperature? Material Specific heat (J/g•°C) Al (aluminum) 0.903 Pyrex glass 0.75 Fe (iron) 0.449 Pb (lead) 0.128 water; H2O (l) 4.18
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 4.70 kg of water at 39.2 °C. During the reaction 120. kJ of heat flows out of the bath and into the flask. -1x-1 Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18 J•g answer has the correct number of significant digits. ·K Be sure your
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 9.50kg of water at 38.9°C. During the reaction 83.3kJ of heat flows out of the bath and into the flask. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18J·g−1·K−1. Be sure your answer has the correct number of significant digits.
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction.A student heats 62.45 grams of platinum to 99.18 °C and then drops it into a cup containing 84.71 grams of water at 23.23 °C. She measures the final temperature to be 25.02 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.66 J/°C.Assuming that no heat is lost to the surroundings calculate the specific heat of platinum.
How much heat is given off to the surroundings when 6 g of aluminum reacts according to the following equation? Express your answer correctly rounded to two decimal places.2 Al + Fe2O3 Al2O3 + 2 Fe ΔH°rxn = -849 kJ. kJIf all of the heat generated by the reaction was absorbed by one liter of room temperature water, what would be the highest temperature the water could reach? Express your answer correctly rounded to two decimal places. °CWhile writing this question, I had to take into account that the final temperature reachable in the previous question could not exceed the boiling point of water. Given this information, what is the highest whole number amount of aluminum that could have been used for this question? Enter only a number for your answer. g