Constants Periodic TableZinc metal reacts with hydrochloric acid accordingto the following balanced equation.Zn(s) + 2HC1(aq)→ZnCl2 (aq) + H2 (g)When 0.112 g of Zn(s) is combined with enoughHCl to make 515 mL of solution in a coffee-cupcalorimeter, all of the zinc reacts, raising thetemperature of the solution from 22.1 C to 241°C.Part AFind A H for this reaction as written. (Use 1.0 g/mL for the density of the solution and 4.18 J/g. C asthe specific heat capacity.)να ΑΣφAH,xn -kJ/molSubmitPrevious Answers Request Answer* Incorrect; Try Again; 25 attempts remainingNext >Provide FeedbackP 8:36

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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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2 ·als NaOH, H ethanol heat
When 200.0 mL of 0.862 M HCI is mixed with 200.0 mL of 0.431 M Ba(OH)2 in a coffee cup calorimeter, the temperature of the solution increases from 21.35°C to 27.05°C. Given the specific heat of solution of 4.18 J g1 °C-l and assuming the density of each solution to be 1.00 g/mL, what is the heat of reaction in kJ per mole of HCl? The neutralization reaction is: 2 HCI(aq) + Ba(0H)2(aq) → BaCl2(aq) + 2 H20(1) Select one: -55.3 kJ/mol HCI -9.53 kJ/mol HCI O - 110.6 kJ/mol HCI O 110.6 kJ/mol HCl 55.3 kJ/mol HCI O 9.53 kJ/mol HCI ВАCK Question 5 of 6 NEXT étv A
A student transferred 50.0 ml 1.00 M HCl into a coffee-cup calorimeter, which had a temperature of 25.5 °C. He then added this to 50.0 ml 1.00 M NaOH which also had a temperature of 25.5 °C and stirred the mixture quickly. The resulting solution was found to have a temperature of 32.5 °C. The calorimeter constant for the coffee-cup calorimeter used was 15.0 J/°C. Calculate the heat of reaction. Please include the full solution.
A student followed the procedure in this experiment, using 29.5 mL of 1.66 molar HCl and 31.5 mL of 1.66 molar NaOH, with both solutions having an initial temperature of 22.1 oC. After mixing, a maximum temperature of 30.7 oC is measured. The final mass of the mixture was found to be 63.194 grams. For this problem, assume the specific heat of the solution is 4.18 J/g oC. What is the heat transferred by this reaction, in Joules? Give your answer in in decimal format.
Zinc metal reacts with hydrochloric acid according to the following balanced equation.Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g)When 0.111 g of Zn(s) is combined with enough HCl to make 53.8 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.0 ∘C to 24.0 ∘C.Find ΔHrxn for this reaction as written. (Use 1.0 g/mL for the density of the solution and 4.18 J/g⋅∘C as the specific heat capacity.)
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4. When 1.00 L of 1.05 M Ba(NO3)2 solution is mixed with 1.00 L of 1.10 M NazSO4 solution at 25.0°C in a coffee-cup calorimeter. The reaction is Ba(NOs)2(aq) + NazSO4(aq) → BaSO4(s) + 2NANO:(aq). The final temperature of the mixture increases to 28.1°C. Calculate the enthalpy change per mole for this process. (Assuming C=4.18 J °C' g' and density of the final solution is 1.05 g/ml).
Zinc metal reacts with hydrochloric acid according to the balanced equation:Zn(s) + 2 HCl(aq) ----------> ZnCl2(aq) + H2(g)When 0.103 g of Zn(s) is combined with enough HCl to make 50.0 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.5 °C to 23.7 °C. Find ∆Hrxn for this reaction as written. (Use 1.0 g/mL for the density of the solution and 4.18 J/g . °C as the specific heat capacity.)
25.00 mL of 0.200 M sulfuric acid was added to 25.00 mL of 0.200 M NAOH, in a constant volume calorimeter. The density of the resulting solution is 1.225 g/mL and its specific heat is 5.321 J/g-°C. As the reaction took place, the temperature of the solution rose from 22.0 °C to 31.3 °C. What is AH (in units of kJ/mol) for the reaction, per mole of water formed? This is a limiting reactant problem and your choice of limiting reactant must be justified through stoichiometric calculations. 21.
Solid calcium chloride dissolves in water according to the equation below.CaCl2 (s) ➝ Ca+2 (aq) + 2 Cl – (aq) ΔHº = –81.3 kJ/mol8.00 grams of solid CaCl2 dissolves in 45.0 grams of water initially at a temperature of 20.00 ºC in a perfect calorimeter. Calculate the final temperature of the solution in the calorimeter.[You may assume that no heat escapes the calorimeter and that all solutions have the same specific heat capacity as pure water (4.184 J/g·ºC)]Tfinal = Answer ºC
The addition of hydroiodic acid to a silver nitrate solution precipitates silver iodide according to the reaction: AGNO3 (aq) + HI(aq) → AgI(s) + HNO3 (aq) When 50.0 mL of 5.00x10-2 M AgNO3 is combined with 50.0 mL of 5.00x10-2 M HI in a coffee-cup calorimeter, the temperature changes from 22.40 °C to 22.91 °C. Part A Calculate AHrxn for the reaction as written. Use 1.00 g/mL as the density of the solution and Cs = 4.18 J/(g·°C) as the specific heat capacity of the solution. Express the energy to two significant figures and include the appropriate units. HẢ Units Value ΔΗΚΗ rxn
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 0.79 g of KOH(s) are dissolved in 104.10 g of water, the temperature of the solution increases from 24.69 to 26.63 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.58 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of KOH(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. kJ/mol AH dissolution = BrookaCom Cengage Leaming Thermometer Cardboard or Styrofoam lid Nested Styrofoam cups Reaction occurs in solution.

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