For the questions of the Experiment of Heat and Temperature: The Law of Dulong and Petit, the following data were obtained for the unknown element.specific heat (S) of unknown element (J/g⚫K)Aw of unknown element (g/mol)0.33963.96b) Calculate the atomic heat (C) in J/mol K for the unknown element.1) In this case, your answer should be in decimal notation (for example, 0.123, not 1.23*10^-1) with the correct number of significant figures. Also follow the unit specified ineach question. Do NOT put its unit in your answer because its unit is shown already in the questions.2) It means students shouldn't include any letters or text in the "Numeric answers", because otherwise it'll be marked wrong even if the numbers are correct.Type your answer...

Converting the unit of measurement, C=(0.339g⋅KJ)(63.96molg)C=21.68244mol⋅KJ In three significant…

Answered: For the questions of the Experiment of…

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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Calculate the heat capacity for 50.0 g of water in units of J/oC and calories/oC.
Write all pertinent computations to justify your final answer. Final answersmust be enclosed with a box. Calculate the heat of reaction for the combustion of nitrogen monoxide gas, NO, to form nitrogendioxide, NO2 , as given in the following thermochemical equation: NO(g) + 1/2 O2 → NO2(g) Given:(a) 1/2 N2(g) + 1/2O2(g) → NO(g) ∆Hro = 90.29kJ/mol(b) 1/2N2(g) + O2(g) → NO2(g) ∆Hro = 33.2 kJ/mol
The combustion of butane produces heat according to the equation2C4H10(g) + 13O2(g) --> 8CO2(g) + 10H2O(l) ΔH = -5,314.0 kJ What is the change in heat if 19.53 g C4H10 (58.12g/mol) reacts?(Answer should have one place after the decimal. Watch the sign)
What would the final temperature of a 47.854g sample of a metal be if the sample absorbed 183.2 J of heat and was initially at 22.7 °C? The specific heat capacity of the sample is 0.368 J g 1 °c-1. Your Answer: Answer units
The combustion of butane produces heat according to the equation2C4H10(g) + 13O2(g) --> 8CO2(g) + 10H2O(l) ΔH = -5,314.0 kJ What is the change in heat if 10.44 g C4H10 (58.12g/mol) reacts?(Answer should have one place after the decimal. Watch the sign)
What would the final temperature of a 11.081 g sample of a metal be if the sample absorbed 524.9 J of heat and was initially at 20.8 °C? The specific heat capacity of the sample is 0.158 J g¯¹ °C-¹. Your Answer: Answer units
Coffee cup calorimetry was used to determine the enthalpy of solution of lithium iodide (LiI): A) First, the coffee cup was calibrated. 50.0 mL of water (s=4.184J/g×0 C) was heated to 95.50C and mixed with 50.0 mL of cool water at 22.30 C. The temperature of the contents of the coffee cup stabilized at 49.40 C. Determine the heat capacity of the coffee cup. B) Next, the enthalpy of solution of lithium iodide (LiI) was determined. 0.0g of solid lithium iodide was added to 100mL of water at 23.20 C in the coffee cup, and the temperature increased to 32.10 C. Calculate the enthalpy of the solution of lithium iodide.
When a chemist burns ammonia according to the reaction below she finds that the reaction releases heat. (It is exothermic.) 4NH3(g) + 3O2(g) 2N2(g) + 6H2O(g) The enthalpy of the reaction DH = -1267 kJ. What is the enthalpy change (in kJ) when 3 grams of ammonia are burned?
In a calorimeter, a 75.0 g piece of metal at 98.6 *C is submerged in 100.0 g of water, that is initially at 21.8 *C. When the metal and water reach thermal equilibrium, the temperature is 26.2 *C. What was the heat capacity of the metal (3 sig figs)?
2 NO(g) N2(g) + O2(g) H = -180.7 kJ 2 NO(g) + O2(g) 2 NO2(g) H = -113.1 kJ 2 N2O(g) 2 N2(g) + O2(g) H = -163.2 kJ Use Hess's law to calculate H for the reaction below.3 NO(g) N2O(g) + NO2(g)H = _____k J
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic (b) Calculate the amount of heat transferred when 55.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 12.0 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 450.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K
What would the final temperature of a 33.851 g sample of a metal be if the sample absorbed 682.9 J of heat and was initially at 22.5 °C? The specific heat capacity of the sample is 0.255 J g-1 °C-1, Your Answer: Answer units

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