Zinc metal reacts with HCl according to the following balanced equation: Zn(s) + 2HCI(aq) ZnCl2(aq) + H2(g) --> When 0.140 grams of Zn(s) is combined with an excess amount of HCI to make 50.0 mL of solution in a coffee-cup calorimeter, all the zinc reacts, raising the temperature of the solution from 21.60°C to 24.60°C. Find AH for this reaction in kJ/mol. Assume the density of the solution is 1.00 g/mL and the specific heat capacity of the solution is 4.184 J/g°C. Use an atomic weight of 65.38 g/mol for Zn Hints: -q(reaction) = q(solution) AH = q/mol of limiting reagent Do not type units with your answer. Type your answer to three significant figures. If this question is on an exam on your scrap paper report your answer to the proper number of significant figures but still type three significant figures online. Your Answer:

Zinc metal reacts with HCl according to the following balanced equation: Zn(s) + 2HCI(aq) ZnCl2(aq) + H2(g) --> When 0.140 grams of Zn(s) is combined with an excess amount of HCI to make 50.0 mL of solution in a coffee-cup calorimeter, all the zinc reacts, raising the temperature of the solution from 21.60°C to 24.60°C. Find AH for this reaction in kJ/mol. Assume the density of the solution is 1.00 g/mL and the specific heat capacity of the solution is 4.184 J/g°C. Use an atomic weight of 65.38 g/mol for Zn Hints: -q(reaction) = q(solution) AH = q/mol of limiting reagent Do not type units with your answer. Type your answer to three significant figures. If this question is on an exam on your scrap paper report your answer to the proper number of significant figures but still type three significant figures online. Your Answer:

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 A student determines the heat of dissolution of solid cobalt(II) sulfate using a coffee-cup calorimeter of negligible heat capacity. When 1.34 g of CoSO4(s) is dissolved in 101.00 g of water, the temperature of the solution increases from 25.00 to 26.69 °C. Based on the student's observation, calculate the enthalpy of dissolution of CoSO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.
A student followed the procedure in this experiment, using 29.5 mL of 1.59 molar HCl and 31.0 mL of 1.59 molar NaOH, with both solutions having an initial temperature of 22.6 oC. After mixing, a maximum temperature of 33.1 oC is measured. The final mass of the mixture was found to be 64.655 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. When entering units, use proper abbreviated units with proper capitalization.
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.)
A student followed the procedure in this experiment, using 50.00 mL of 2.00 molar HCl and 51.00 mL of 2.00 molar NaOH both solutions having an initial temperature of 22.7 oC. After mixing, a maximum temperature of 32.2 oC is measured. The final mass of the mixture was found to be 104.84 grams. For this problem, assume the specific heat of the solution is 4.18 J/g oC. Report all answers with the proper number of significant figures. What is the heat transferred by this reaction, in Joules?
In the following experiment, solid CaCl2 is dissolved in water:CaCl2(s) → Ca2+(aq) + 2Cl-(aq) ΔsolnH = −82.8 kJ mol−1A coffee-cup calorimeter containing 145 mL of H2O is used. The initial temperature of water in the calorimeter is 18.9°C. If 3.04 g of CaCl2 is added to the water, what will be the final temperature of the solution in the calorimeter? Assume the density and specific heat capacity of the solution is the same as water (d=1 g/mL, Cs=4.18 J g-1 °C-1) and that no heat is lost to the calorimeter.
Constants Periodic Table Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s) + 2HC1(aq)→ZnCl2 (aq) + H2 (g) When 0.112 g of Zn(s) is combined with enough HCl to make 515 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.1 C to 241 °C. Part A Find A H 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.) να ΑΣφ AH,xn - kJ/mol Submit Previous Answers Request Answer * Incorrect; Try Again; 25 attempts remaining Next > Provide Feedback P 8:36
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).
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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
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