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...

See similar textbooks

Similar questions

In a coffee cup calorimeter, 50.0 mL of 0.139 M AgNO3 and 50.0 mL of 0.139 M HI are mixed. The following reaction occurs. Ag+ (aq) + I (aq) → Agi(s) If the two solutions are initially at 21.74°C, and if the final temperature is 23.60°C, calculate AH for the reaction in kJ/mol of AgI formed. Assume a mass of 100.0 g for the combined solution and a specific heat capacity of 4.18 J °C-1g-¹. kJ/mol Need Help? Read It Supporting Materials Periodic Table Watch It Constants & Factors. Supplemental Data
In a coffee cup calorimeter, 50.0 mL of 0.130 M AGNO, and 50.0 mL of 0.130M HBr are mixed. The following reaction occurs. Ag*(aq) + Br¯(aq) → AgBr(s) If the two solutions are initially at 23.51°C, and if the final temperature is 24.82°C, calculate AH for the reaction in kJ/mol of AgBr formed. Assume a mass of 100.0 g for the combined solution and a specific heat capacity of 4.18 J°C¯1g=1. 84.2 X kJ/mol
true of false
None
In a coffee cup calorimeter, 50.0 mL of 0.124 M AgNO3 and 50.0 mL of 0.124 M HBr are mixed. The following reaction occurs. Ag*(aq) + Br (aq) → AgBr(s) If the two solutions are initially at 23.92°C, and if the final temperature is 25.17°C, calculate AH for the reaction in kJ/mol of AgBr formed. Assume a mass of 100.0 g for the combined solution and a specific heat capacity of 4.18 J °C-1g-¹. kJ/mol
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.
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
In Part B of the experiment, a student mixes 30.0 mL of 1.1 M HC1(aq) with 30.0 mL of 1.000 M NaOH(aq) in a well-insultated calorimeter and observes that the temperature of the solution increases by 5.75 °C. These are similar conditions as the previous two problems. How many moles of water are formed? number of moles of water = mol
Constants Periodic Table Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s) + 2HCI(aq)→ZnCl2 (aq) + H2 (g) When 0.112 g of Zn(s) is combined with enough HCl to make 51.5 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22,1°C to 24.1 C Part A Find A H,xn 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.) 國 AHxn = kJ/mol Submit Request Answer Provide Feedback Next> P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. | Terms of Use Privacy Pollcy Permissions | Contact Us Vi 1:23
Carbon disulfide burns in air, producing carbon dioxide and sulfur dioxide. CS2 (1) +302(g) → CO,(g) + 250,(9); AH = -1.077 × 10° kJ What is AH for the following equation? CO2 (9) + SO,(g) → - CS ()+0, (9) CS, AH = k]
A calorimeter contains 16.0 mLmL of water at 12.5 ∘C∘C . When 1.40 gg of XX (a substance with a molar mass of 75.0 g/molg/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq)X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 25.0 ∘C∘C . Calculate the enthalpy change, ΔHΔ�, for this reaction per mole of XX. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)J/(g⋅∘C)], that density of water is 1.00 g/mLg/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings. Express the change in enthalpy in kilojoules per mole to three significant figures.
In a coffee cup calorimeter, 3.00 g of NaOH (molar mass 40.00g/mol) was mixed with 75.0 mL of 1.00M HNO3. If the initial temperature of the HNO3 was 31.3°C and the final temperature of the solution was 22.3°C, determine AH for the reaction in kJ/mol. NaOH(s) + HNO3(aq) ===> NaNO3(aq) + H2O) The density and the specific heat capacity of the resulting solution are 1.00 g/ml and 4.18 J/°C.g, respectively. Units do not need to be typed, simply enter the correct number. If the sign of AH is negative put a negative sign (-) in the answer. Answer: