Part A Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s) + 2HC1(aq)→ZnCl2 (aq) + H2 (9) Find A, H for this reaction as written. (Use 1.0 g mL-1 for the density of the solution and 4.184 J g¬1 °C-1 as the specific heat capacity.) Express your answer in kilojoules per mole to two significant figures. When 0.124 g of Zn(s) is combined with enough HCl to make 52.7 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.4 °C to 24.4 °C. A,H = kJ mol-1

Part A Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s) + 2HC1(aq)→ZnCl2 (aq) + H2 (9) Find A, H for this reaction as written. (Use 1.0 g mL-1 for the density of the solution and 4.184 J g¬1 °C-1 as the specific heat capacity.) Express your answer in kilojoules per mole to two significant figures. When 0.124 g of Zn(s) is combined with enough HCl to make 52.7 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.4 °C to 24.4 °C. A,H = kJ mol-1

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.94PAE

See similar textbooks

Similar questions

Peanuts and peanut oil are organic materials and bum in air. How many burning peanuts does it take to provide the energy to boil a cup of water (250 mL of water)? To solve this problem, we assume each peanut, with an average mass of 0.73 g, is 49% peanut oil and 21% starch; the remainder is noncombustible We further assume peanut oil is palmitic acid, C16H32O2, with an enthalpy of formation of 848.4 kJ/mol. Starch is a long chain of C6H10O5 units, each unit having an enthalpy of formation of 960 kJ.
The enthalpy of vaporization for water is 40.65 kJ mol-1. As a design engineer for a project in a desert climate, you are exploring the option of using evaporative cooling. (a) If the air has an average volumetric heat capacity of 0.00130 J cm-3 K-1, what is the minimum mass of water that would need to evaporate in order to cool a 5 m? 5 m room with a 3 m ceiling by 5°F using this method? (b) Is this a spontaneous or nonspontaneous process?
SHOW CLEAR SOLUTION: To a test tube containing 10.0 ml of 0.50 M HCl solution in a calorimeter, 0.05482 g of solid MgO (MW = 40.30 g/mol) at the same temperature was added. A change in temperature of 6.2°C was recorded. In a separate experiment, the heat capacity of the calorimeter was determined to be 0.293 kJ/°C. D. Calculate the experimental ΔHrxn (in kJ/mol) for the reaction between MgO andHCl.E. If the theoretical ΔHrxn of the reaction between MgO and HCl is -1349 kJ/mol, calculate the %error.
Give handwritten answer A coffee cup calorimeter is prepared, containing 100.000 g of water (specific heat capacity = 4.184 J/g K) at initial temperature 80.000 C. A salt weighing 7.308 g is quickly added. The salt has a molar mass of 178.051 g/mol. The final temperature of the solution is 51.028 C. Assume no heat loss to the surroundings. Assume the specific heat capacity of the solution is equal to that of pure water, and that the mass of the solution is equal to the mass of the solid plus the mass of water in the calorimeter. What is the molar heat of solution for the salt, in kJ/mol?
In a calorimetry experiment similar to the one performed today, a student used 50.0 ml of 1.0 m NaOH and 5.0 ml of 1.0 m HCL each initially at 22.5ºC. The max temp observed after mixing was 28.0º C. What is the heat of reaction in units of kJ ?
Part B Consider the reaction C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l)C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l) in which 10.0 gg of sucrose, C12H22O11C12H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/∘CkJ/∘C. The temperature increase inside the calorimeter was found to be 22.0 ∘C∘C. Calculate the change in internal energy, ΔEΔEDelta E, for this reaction per mole of sucrose. Express the change in internal energy in kilojoules per mole to three significant figures.
You are camping and need to cook all your food using your camp stove which runs off of propane.If you wanted to warm up your giant mug (67.628 fluid ounces) of morning coffee from 10°C to 80°C,what mass of propane would you have to use?The ΔHcomb for propane is -2219.2 kJ/mol, the density of coffee is 1.0002 g/mL, and the specific heatcapacity of coffee is equal to that of water.1 fluid ounce = 0.0295735 L
Given the following information: Chemical Reaction: 2 C10H10 (l) + 25 O2 (g) → 20 CO2 (g) + 10 H2O(l) ∆H = 10,314 KJ/mol The standard heat of formation (KJ/mol) at 298.15 oC : CO2 = -393.5 ; H2O(l) = -285.8 What is the standard enthalpy of formation of C10H10?
In this experiment you will place a sample of your salt in water in a constant pressure calorimeter with a heat capacity of 29.4 J/℃. You will determine the enthalpy change for the dissociation of your salt, Delta Hdiss. A sample of 4.368 grams of the salt SrCl2 was placed in 35.5 g water, the initial temperature was 20.00℃ and the final temperature was 27.086365℃. If the heat capacity of the calorimeter, C (cal) is 29.4 J/ g℃, what is the correct sig fig answer for the heat of calorimeter? q (calorimeter) = C (cal) x delta t q (calorimeter) = (29.4 J/℃) x (27.086365℃ – 20.00℃) q (calorimeter) = (29.4 J/℃) x (7.086365℃) q (calorimeter) = 208.339131 J a. 208.3 J b. 208.34 J c. none of these d. 208.3391 J e. 208 J f. 208.339131 J g. 2.0 x 10^2 J h. 2.1 x 10^2 J
A 21.42g sample of an unknown metal was heated to 99.5ºC, and the added to 50.00g of water contained in a foam coffee cup. The initial temperature of the water was 20.5ºC, and the final temperature of the metal and water was 25.1ºC. The calorimeter constant for the coffee-cup calorimeter was 13.5 J/ºC. What was the specific heat of the metal? * the answer is 0.64 J/gºC, but I need to know how to get there
You will find the final temperature when 5.00 grams of aluminum at 425℃ is placed in 50.0 grams of water at 19.5℃. Aluminum has a specific heat capacity of 0.900 J/g ℃. And water has a specific heat capacity of 4.184 J/g℃. (So that we do not have 8 points on one question I have broken this down into a few steps). First what is the calculator answer for the value of m Cs (mass times specific heat capacity) for the hot aluminum? Select one: a. 45 J/℃ b. none of these c. 209.2 J/℃ d. 25.104 J/℃ e. 3.6 J/℃ f. 16.736 J/℃ g. 4.5 J/℃ h. 20.92 J/℃ i. 5.4 J/℃
: Determine the molar enthalpy change for reaction 2 NH4Cl(aq) + NaOH(aq) ® NaCl(aq) + NH3(aq) + H2O(l) DH2 = Using the solution procedure similar to that of the sample problem shown on page 2, calculate the molar heat of enthalpy, in kJ/mol NH4Cl, of reaction 2 given the following procedure and data information. Measure 50.0 mL of 2.00 M NaOH into the coffee cup calorimeter Measure 50.0 mL of 2.00 M NH4Cl into a glass beaker Collect the initial temperature of both solutions Add the 50.0 mL of 2.00 M NaOH into the coffee cup calorimeter all at once Use the thermometer to gently and continuously stir the mixture in order to disperse the heat evenly thorough the solution Continue to monitor the temperature until it maxes out. Record the highest temperature. Assume all solutions have a density = 1.03 g/mL and a heat capacity = 4.18 J/g×°C Temperature data: Temperature of the solutions before mixing: 21.3 °C…