How much heat, in joules and in calories, must be added to a 75.8 g nickel block with a specific heat of 0.445 J/g.°C to increase its temperature from 25°C to its melting temperature of1455°C?4.04.0cal4.Supporting MaterialsPeriodic TableConstants andSupplemental DataFactorsAdditional MaterialsSection 5.1Show My Work (Required) ?What steps or reasoning did you use? Your work counts towards your score.Upioaded File (10 file maximum)You can submit show my work an unlimited number of times.No Files to DisplayO Upload File5:32 PM3/30/2020Type here to searchiphomeendprt scdeletenum+ backspacelock4home00%24%23

Given, Mass of Nickel = 75.8g Specific heat capacity = 0.445 J/g.0C. Initial T = 25 0C Final…

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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...

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1. More than 2000 years ago human cultures figured out a way to produce iron metal from rocks containing iron ores. This iron could be worked by a blacksmith (repeated heating and hammering) to make iron metal pure enough for creating useful tools (even Samurai swords). This direct heating technique was common up until about 200 years ago when people found a better way to obtain iron metal. When hematite, Fe2O3(s), is strongly heated in a blast furnace in the presence of charcoal (carbon), pure iron metal is obtained. Fe2O3() 2 Fe(s) + 3/2 O2 (g) (1) C(s) + O2 (g) → CO2(g) (2) When reaction 1 is coupled to reaction 2, overall chemical equation is Fe2O3() + 3/2 C() 3/2 CO2(g) + 2 Fee) Use the thermodynamic data given below for the following calculations: AG¡ (kJ/mol) | 4H¡ (kJ/mol) | S (J/mol-K) Fe2O3(s) -742.2 -824.2 87.40 Fes) 27.28 CO2(8) -394.36 -393.51 213.74 C (6) 5.74 O2 (2) 205.14 a) Calculate the standard Gibb's free energy change for reaction 1 b) Calculate the standard Gibb’s…
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Use the References to access important values if needed for this question Ethanol, C2H0, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to bum more efficiently in internal combustion engines. The combustion enthalpy of ethanol is 1366.9 kJ/mol The combustion enthalpy of 2-methylpentane, C6H14 is 4.157x103 kJ/mol. Calculate the energy released during the complete combustion of 382 g 2-methylpentane kJ Assuming the same efficiency, would 382 g ethanol provide more, less, or the same quantity of energy as 382 g 2-methylpentane? | Submit Answer Retry Entire Group 8 more group attempts remaining
Part A MISSED THIS? Read Section 7.3 (Pages 267 - 272) ; Watch KCV 7.3, IWE 7.2. Suppose that 28 g of each of the following substances is initially at 29.0 °C. What is the final temperature of each substance upon absorbing 2.45 kJ of heat? gold Express your answer to two significant figures. • View Available Hint(s) T = help Submit Request Answer Part B silver
22. Statement A: The system loses 726 J to the surroundings as heat. The enthalpy change for the system is positive. Statement B: The system absorbs 178 J to the surroundings as heat. According to sign conventions heat is negative. Which of the following conclusions is correct about statements A and B? Group of answer choices Statement A is incorrect, Statement B is correct. Both statements are correct. Both statements are incorrect. Statement A is correct, Statement B is incorrect.
When a 45.0 g sample of an alloy at 100.0 °C is dropped into 100.0 g of water at 25.0 °C, the final temperature is 37.0 °C. What is the specific heat of the alloy? The specific heat of H20(1) is 4.184 J'g-1.°c-1. q = mc AT O A. 0.423 J-g-1.°c-1 O B. 9.88 J-g-1.°C-1 O C. 48.8 J'g-1.°C-1 O D. 1.77 Jg-1.°c-1
1) A 0.416 g sample of KCl is added to 56.5 g of water in a calorimeter. If the temperature decreases by 1.24°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C? _____ J 2) Is the reaction exothermic or endothermic?
Determine the most likely identity of the unknown metal sample. Mass of empty beaker = 50.45 g Mass of beaker and water = 81.26 g Mass of water 30.81 g (represents a calculation rather than a direct measurement) Initial water temperature = 25.5 C Mass of metal = 54.02 g Initial metal temperature = 102.5 C Final water and metal mixture temperature = 36.0 C The specific heat capacity of water is 4184 J/kg C
The specific heat of the metallic element rhodium is 0.240 J/g-K at 25°C. If 586 J of heat is added to an 80.0 g block of rhodium metal that is initially at 25.0°C, what is the expected final temperature of the block? O 32.3°C O 2470°C O 55.5°C O 30.5°C O 26 8°C
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