A 2.50 g sample of powdered zinc is added to 100.0 mL of a 2.00 M aqueous solution of hydrobromic acid in a calorimeter. The total heat capacity of the calorimeter and solution is 448 J/K. The observed increase in temperature is 21.1 K at a constant pressure of one bar. Calculate the standard enthalpy of reaction using these data. Zn(s) + 2 HBr(aq) → ZNB., (aq) + H, (g) kJ/mol AHan =

A 2.50 g sample of powdered zinc is added to 100.0 mL of a 2.00 M aqueous solution of hydrobromic acid in a calorimeter. The total heat capacity of the calorimeter and solution is 448 J/K. The observed increase in temperature is 21.1 K at a constant pressure of one bar. Calculate the standard enthalpy of reaction using these data. Zn(s) + 2 HBr(aq) → ZNB., (aq) + H, (g) kJ/mol AHan =

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

Related questions

Q: When 50.0 mL of 1.60 M of HCl(aq) is combined with 50.0 mL of 1.70 M of NaOH(aq) in a coffee-cup…

A: The amount of heat required to raise the temperature of the sample is given by: q = mc∆Tq is the…

Q: A scientist measures the standard enthalpy change for the following reaction to be -661.2 kJ : ...…

A: P4H10(s) + 6H2O (l)------> 4H3PO4(aq) ∆Hof( P4H10 )= -3009.94 kJ/mol ∆Hof(H2O)= -285.82 kJ/mol…

Q: A 100.0 g piece of metal at 100°C is placed in contact with 50.0 g of water (s = 4.184 J g–1 °C–1)…

Q: Consider 100.0 mL of 1.00 M HCI (aq) that reacts with 50.0 mL of 5.00 M NaOH, in a coffee - cup…

A: The objective of this question is to calculate the molar heat of reaction (ΔHrxn) for the…

Q: A student dissolves 12.4 g of sodium hydroxide (NaOH) in 200. g of water in a well-insulated open…

A: The reaction is Exothermic.

Q: Part A Given the following heat capacity data, calculate AH of CO2 (g) at 753 K. The standard…

A: The standard enthalpy of formation is the change in enthalpy calculated at the standard state…

Q: When 50.0 mL of 1.20 M of HCl(aq) is combined with 50.0 mL of 1.30 M of NaOH(aq) in a coffee-cup…

Q: A 2.50 g sample of powdered zinc is added to 100.0 mL of a 2.00 M aqueous solution of hydrobromic…

Q: A generic solid, X, has a molar mass of 76.0 g/mol. In a constant‑pressure calorimeter, 37.7 g of X…

A: Solution:-

Q: A scientist measures the standard enthalpy change for the following reaction to be 2885.4 kJ:…

A: 6CO2 (g) + 6 H2O (l) ---> C6H12O6 (s) + 6 O2 (g) ∆Hrxn = 2885.4 KJ/mol ∆H°f H2O = ?

Q: An electrical heater adds 21.9 kJ of heat to a constant-volume calorimeter. The temperature of the…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 664.0 mg sample…

A: To find the molar heat capacity, we need to use the formula which contains mol, specific heat and ∆T…

Q: A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of 0.300 M HCl in a calorimeter.…

Q: Measurements show that the energy of a mixture of gaseous reactants increases by 369. kJ during a…

A: We have to calculate the change in enthalpy and nature of reaction.

Q: A 0.00757 mol sample of an organic compound was burned in oxygen in a bomb calorimeter. The…

Q: A piece of metal weighing 5.10 gg at a temperature of 48.5 ∘C∘C was placed in a calorimeter in…

Q: 8.000 g of Compound X with molecular formula C4H are burned in a constant-pressure calorimeter…

A: Mass of water = 10 kg Mass of C4H8 = 8g Temperature rise = 8.755°C

Q: An electrical heater adds 23.7 kJ of heat to a constant - volume calorimeter. The temperature of the…

A: The objective of the question is to calculate the molar energy of combustion of methanol using the…

Q: A 61.0 mL sample of 1.0 M NaOH is mixed with 48.0 mL of 1.0 M H2SO4 in a large Styrofoam coffee cup;…

A: Reaction - NaOH + H2SO4 --> Na2SO4 + H2OMoles of NaOH = (Molarity x volume in Liters) of NaOH…

Q: A student using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when…

A: Given: Temperature of the solution with calorimeter decreased = 1.10 K Mass of KNO3 added = 1.00 g.…

Q: When a solid dissolves in water, the solution may become hotter or colder. The dissolution enthalpy…

Q: Measurements show that the enthalpy of a mixture of gaseous reactants increases by 338. kJ during a…

A: Enthalpy change(∆H) = 338 KJ Work (W) = +135 KJ (positive because work done on the system)

Q: Measurements show that the energy of a mixture of gaseous reactants increases by 231. kJ during a…

Q: Measurements show that the energy of a mixture of gaseous reactants decreases by 308.kJ during a…

Q: 50.0 mL of 2.03 M NaOH(aq) is mixed with 50.0 mL of 2.20 M HCl in a Styrofoam calorimeter.…

Q: ICI is a corrosive colourless gas that dissolves readily in water. Aqueous HCL reacts with NaOH to…

Q: A quantity of 2.00 ×102 mL of 0.715 M HCl is mixed with 2.00 × 102 mL of 0.358 M Ba(OH)2 in a…

A: Molarity - ratio of number of moles of solute to the volume of solution in litres. Formula is,…

Q: A system absorbs 1.66E2 kJ of heat and the surroundings do 1.032E2 kJ of work on the system. What is…

A: We have to predict the change in internal energy of system.

Q: Measurements show that the energy of a mixture of gaseous reactants increases by 243.kJ during a…

A: Given:Change in energy Where the positive sign indicates energy is increasedWhere the positive sign…

Q: A scientist measures the standard enthalpy change for the following reaction to be 6.7 kJ : CO(g) +…

Q: A 2.50 g sample of powdered zinc is added to 100.0 mL of a 2.00 M aqueous solution of hydrobromic…

A: Given weight of Zn = 2.50 g [HBr] = 2M Volume of HBr = 100mL= 0.1 L No. Of moles of HBr = 2 x 0.1 =…

Q: When 50.0 mL of 1.24 M of HCI(aq) is combined with 50.0 mL of 1.32 M of NaOH(aq) in a coffee-cup…

Q: When 18.5 g of HgO(s) is decomposed to form Hg(l) and O2(g), 7.75 kJ of heat is absorbed at…

A: From standard sources, we get:- Molar mass of HgO = 216.59 g/mol Amount of HgO consumed = 18.5g

Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

General Chemistry 4th Edition
McQuarrie • Rock • Gallogly
University Science Books
presented by Macmillan Learning
A 2.50 g sample of powdered zinc is added to 100.0 mL of a 2.00 M aqueous solution of hydrobromic acid in a calorimeter. The
total heat capacity of the calorimeter and solution is 448 J/K. The observed increase in temperature is 21.1 K at a constant
pressure of one bar. Calculate the standard enthalpy of reaction using these data.
Zn(s) + 2 HBr(aq)
ZnBr, (aq) + H,(g)
AHan =
kJ/mol
rxn
Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry| Publisher: University Science Books
étv
MacBook Air
DU
888
F7
FO
F4
%
T0
delet
%23
8.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Final answer

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A 2.50 g sample of powdered zinc is added to 100.0 mL of a 2.00 M aqueous solution of hydrobromic acid in a calorimeter. The total heat capacity of the calorimeter and solution is 448 J/K. The observed increase in temperature is 21.1 K at a constant pressure of one bar. Calculate the standard enthalpy of reaction using these data. Zn(s) + 2 HBr(aq) →→→→ ZnBr₂(aq) + H₂(g) AHin = kJ/mol
The compound WO3(s) is utilized in the refining process of tungsten from its mineral ore. Tungsten can be produced as follows: Reaction 1: WO3(s) + 3H2(g) → W(s) + 3H2O(g) a) From the following data calculate the enthalpy of the above reaction Reaction 2: 2W(s) + 3O2(g) → 2WO3(s) ΔH = –1685.4 kJ Reaction 3: 2H2(g) + O2(g) → 2H2O(g) ΔH = –477.84 kJb) Estimate the change of internal energy for Reaction 1. c) Is Reaction 1 exothermic or endothermic?
Measurements show that the energy of a mixture of gaseous reactants decreases by 175. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 79. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture during the reaction. Be sure your answer has the correct number of significant digits. x10 exothermic Is the reaction exothermic or endothermic? endothermic
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. 1. Write the balanced equation for the reaction between HCl and MgO.2. Which is the limiting reactant? Show your solution.3. Calculate heat released by the reaction, qrxn, in the calibration step (in kJ).
A piece of metal of mass 15 g at 99◦C is placed in a calorimeter containing 41.3 g of water at 19◦C. The final temperature of the mixture is 40.2◦C. What is the specific heat capacity of the metal? Assume that there is no energy lost to the surroundings. Answer in units ofJg·◦C.
Let's use our knowledge of constant volume (bomb) calorimetry to determine the heat energy in a given food sample, say a hamburger. A typical hamburger has a serving size of 105 g and consists of approximately 20% protein (21.0 g), 33% fat (34.7 g), and 47% carbohydrate (49.3 g). Assume that the heat capacity of the bomb calorimeter is 8.39 kJ K-¹, and the increase in water temperature was 13.2 K. Q5.38 Homework Unanswered How many Calories (Cal) are in the hamburger described above? Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 105) Type your numeric answer and submit Unanswered • 4 attempts left Submit
Find the molar enthalpy of combustion in kJ/mol of glucose at some temperature and pressure C6H12O6 (s) + 6 O2 (g) → 6 CO2 (g) + 6 H2O (l) given that in an experiment under the same conditions the combustion of 0.108 g of glucose raised the temperature of a calorimeter with total heat capacity C= 1.155 kJ/°C by 1.31 °C. The molar mass of glucose is 180.1 g/mol. Ignore the heat absorbed by the combustion products; assume this is negligible, and all heat went into the calorimeter itself. Give the answer with 5 or more significant figures.
When 60.0 mL of a 0.400 M solution of HNO3(aq) is combined with 60.0 mL of a 0.400 M solution of NaOH(aq) in a coffee-cup calorimeter, the final temperature of the solution is measured to be 26.6 °C. The initial temperature of the solutions is 24.0 °C. Calculate qrxn in joules, assuming the specific heat capacity of the final solution is 3.90 J.g-¹.°C-¹, the density of the final solution is 1.04 g/mL, and the calorimeter constant is 45 J/°C. (Hint: start with 9rxn+qsoln+qcal = 0.) The balanced chemical equation for this reaction is: HNO3(aq) + NaOH(aq) → H₂O(1) + NaNO3 (aq)
An ideal gas sealed in a rigid 3.13-L cylinder, initially at pressure Pi=12.70 atm, is cooled until the pressure in the cylinder is Pf=1.18 atm. What is the enthalpy change for this process?What is the change in internal energy for this process?
A 1.22 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/oC, contained 7 g of water. The temperature of the calorimeter and its contents increased from 23.47oC to 27.95oC. What is ΔH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place. Do not include the unit.)
A 1.6 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/oC, contained 7 g of water. The temperature of the calorimeter and its contents increased from 23.58oC to 27.95oC. What is ΔH
Measurements show that the enthalpy of a mixture of gaseous reactants decreases by 253. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 149. kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Round your answer to 3 |kJ х10 significant digits. exothermic Is the reaction exothermic or endothermic? endothermic