**Experiment 3: Redox Reaction of Calcium and Water**A student conducted an experiment to measure the change in enthalpy (ΔH) for the redox reaction:\[ \text{Ca}(s) + \text{H}_2\text{O}(l) \rightarrow \text{Ca(OH)}_2(aq) + \text{H}_2(g) \]In this experiment, 0.6418 g of calcium (Ca) was added to 200.0 mL of distilled water contained in a styrofoam cup. The observed change in temperature was +8.4°C. The density of the water used was 1.00 g/mL.**Tasks:**a. **Oxidation and Reduction:** - Identify which element is being oxidized and which is reduced.b. **Energy Absorption by Calorimeter:** - Calculate the energy absorbed by the calorimeter. Use \( C_{\text{cal}} = 20. \, \text{J/°C} \).c. **Energy Absorption by Solution:** - Calculate the energy absorbed by the solution. Use \( S_{\text{soln}} = 4.184 \, \text{J/g°C} \). - Note that \( m_{\text{soln}} \) is the combined weight of water and calcium dissolved into the water.d. **Total Energy Released:** - Calculate the total energy released by the reaction.e. **Enthalpy of Reaction (per gram of calcium):** - Calculate the enthalpy change (ΔH) per gram of calcium.f. **Enthalpy of Reaction (per mole of calcium):** - Calculate the enthalpy change (ΔH) per mole of calcium. These calculations will help in understanding the thermodynamics of the reaction under study.

"Since you have posted a multiple sub-part question, we will solve the first 3 sub-parts for you. For the remaining sub-parts, kindly post the question again with the answers to the a,b, and c subparts. Thank you" For the given redox reaction: Ca(s) +H2O(l) → Ca(OH)2 (aq) +H2 (g) We have to answer the given questions. Given reaction:Ca(s) +H2O(l) → Ca(OH)2 (aq) +H2 (g)Ca=0 H=+1 Ca=+2 H=0We can see that:Calcium is going from 0 in Ca to+2 in Ca(OH)2, hence calcium is oxidizedHydrogen is going from +1 in H2O to 0 in H2, hence hydrogen is reduced. Energy absorbed by calorimeter, qcal = Ccal × ∆Tqcal = 20 J/°C × 8.4 °Cqcal =168 JMass of calcium = 0.6418 g Volume of water = 200.0 mL Density of water = 1g/mL ∴Mass of water = density of water×volumeMass of water =1 g/mL × 200 mLMass of water =200 gTotal mass of solution = mass of calcium+mass of waterTotal mass of solution =0.6418 g+200gTotal mass of solution, msoln = 200.6418 g Energy absorbed by the solution, qsoln = msoln×Ssoln×∆T qsoln = 200.6418 g × 4.184 J/g °C × 8.4 °Cqsoln =7051.68 J

Science

Chemistry

3. A student added calcium to water and measured the increase in temperature to determine AH for the redox reaction: Ca(s) + H₂O(l) → Ca(OH)₂ (aq) + H₂(g). When 0.6418 g Ca was added to 200.0 mL of distilled water in a styrofoam cup, the change in temperature was +8.4°C The density of the water was 1.00 g/mL. a. Which element is being oxidized in this reaction? Which is reduced? b. Calculate the Joules of energy absorbed by the calorimeter, given that Ccal = 20. J/°C. Calculate the Joules of energy absorbed by the solution, given that Ssoln = 4.184 J/g°C. [Note that msoln is the combined weight of water and calcium dissolved into water] d. Calculate the Joules of energy released by the reaction. C.

3. A student added calcium to water and measured the increase in temperature to determine AH for the redox reaction: Ca(s) + H₂O(l) → Ca(OH)₂ (aq) + H₂(g). When 0.6418 g Ca was added to 200.0 mL of distilled water in a styrofoam cup, the change in temperature was +8.4°C The density of the water was 1.00 g/mL. a. Which element is being oxidized in this reaction? Which is reduced? b. Calculate the Joules of energy absorbed by the calorimeter, given that Ccal = 20. J/°C. Calculate the Joules of energy absorbed by the solution, given that Ssoln = 4.184 J/g°C. [Note that msoln is the combined weight of water and calcium dissolved into water] d. Calculate the Joules of energy released by the reaction. C.

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: Consider these reactions, where M represents a generic metal. 2 M(s) + 6 HCI(aq) → 2 MCI, (aq) + 3…

A: Hess's law states the enthalpy change for the overall reaction is the sum of the enthalpies of…

Q: what quantity of coal must be burned to supply 3.18*10^6 KJ, assuming that the only combustion…

A: Given: The heat released = 3.18 × 106 kJ Standard data: The heat of combustion of solid carbon =…

Q: Identify the type of reactions below as endo or exothermic and give reason. 1) 2 So, (g) → 2 S (s) +…

A: The reaction which releases heat energy resulting in the rise of temperature of the surrounding…

Q: Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions…

A: The balanced reaction taking place is given as, 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)…

Q: A student dissolves 12.7 g of sodium chloride (NaCl)in 250. g of water in a well-insulated open cup.…

A: It is based on the concept of enthalpy of dissolution of salt Here we are required to find the…

Q: In a constant-pressure calorimeter, 60.0 mL of 0.320 M Ba(OH), was added to 60.0 mL of 0.640 M HCI.…

A: In the given reaction both reactants are present in equal moles. Calculate the moles of water,

Q: Given the reactions, X(s) + 0,(g) – XO(s) AH = -532.9 kJ %3D XCO,(s) XO(s) + CO,(g) AH = +290.3 kJ…

Q: Write a balanced chemical equation for the standard formation reaction of solid aluminum hydroxide…

A: Aluminium hydroxide is formed by reacting aluminium carbide with water as shown below. Al4C3 + H2O…

Q: Balance each of the following reactions, and identify the type of reaction KClO3(s)Δ→KCl(s)+O2(g)

A: Chemical reactions are those reactions which undergo any chemical change. Chemical reaction is…

Q: When we exercise, we rely on the oxidation of glucose (C6H12O6) to carbon dioxide and water for…

Q: A chemist measures the enthalpy change AH during the following reaction: 2 Al(s) + Fe,O3(s)→Al,O3(s)…

A: Given, 2 Al(s) + Fe2O3(s) ➝ Al2O3(s) + 2 Fe(s) ∆H = -852 kJ Calculating the values of ∆H for the…

Q: Identify each of the following unbalanced reactions as a redox-reaction or a non-redox reaction.…

A: Identify the reactions as redox or non-redox reactions.

Q: A student performs a calorimetry experiment. The student combines 100. g of 0.40 M HC1(aq) with 100.…

A: Heat absorbed by the particular species = mass × heat capacity × temperature change

Q: 7. Consider the reaction A→2 B. Initially 1.5 mol of A is present and no B. What are the amounts of…

Q: Given that the enthalpy of neutralization for the reaction of HCl (a strong acid) and NaOH (a strong…

Q: A student dissolves 12.1 g of lithium chloride (LiCl)in 300. g of water in a well-insulated open…

A: Mass of lithium chloride = 12.1 g Initial temperature, T1 = 21.0 °C Final temperature, T2 = 27.8 °C…

Q: For each reaction, write the chemical formulae of the oxidized reactants in the space provided.…

Q: 2 M(s) + 6 HC1(aq) - 2 МСL, (aq) + 3Н, () AH = -581.0 kJ 2. HCI(g) → HC(aq) AH, = -74,8 kJ 3. H, (g)…

Q: [COC14]¯ (alc) + 6H,O(alc) [Co(H,O),J?+ (alc) + 4C1¯(alc) deep blue rose pink

A: Exothermic: Heat is evolved. This is when product is more stable than the reactant Endothermic:…

Q: Please help me solve the following question, explain and make sure everything is correct, thank you…

A: Step 1:Given reaction:AgCl(s)→Ag(s)+Cl(g)Enthalpy change for this reaction is 248kJ/mol, that means…

Q: Consider all the salts that could be made by using combining choosing the cation(s) from the list…

A: ΔsolutionS∘ has not been written in proper format. So this part cannot be answered. Only the first…

Q: Given the standard enthalpy changes for the reactions: Pals) + 302(8) → PaO6[s) AH° = -1640 kJ/mol…

A: Equation 1: P4(s) + 3O2(g) → P4O6(s) ∆H° = - 1640 KJ/mol Equation 2: P4(s) + 5O2(g)→ P4O10(s)…

Q: For each reaction, write the chemical formulae of the oxidized reactants in the space provided.…

Q: Given the equation below, which of the following is true? 2 Mg(s) + O2(g) → 2 MgO(s) + 72.3 kJ 12.…

A: 2Mg + O2->2MgO+72.3KJ

Q: Al' ( ) + HCl ( ) → AlCl3 ( ) + H₂() 9. In the above reaction please list the states of each of the…

A: Balanced chemical equation can be define as the reaction in which number of atoms of all the…

Q: How much heat (in kilojoules) is involved in the oxidation of 105.4 g of Fe at 25Â°C? 4 Fe(s) + 3 O…

A: Given:- 4 Fe(s) + 3 O 2(g)↔ 2 Fe 2O 3(l) ΔH = -1648 kJ mass of Fe = 105.4 g To be calculated :-…

Q: Determine the value of A¡H for the following reaction: 1 MnO2 (s) → MnO(s) + O2 (g) 2

Q: [Review Topics] [References] Iron metal is obtained by reduction of iron(III) oxide with powdered…

A: The chemical equation, Al(s) + Fe2O3(s) -------> Fe(l) + Al2O3(l) Oxidation reaction, 2Al…

Q: Mg(s) + HBr (aq)→ Zn(s) + Ni(NO,)a (aq) → Ca(s) + H,SO, (aq)→ Write an equation for the reaction if…

A: Balance Chemical equation means no of atoms or ions should be equaal in both side reactant and…

Q: When 0.400 g of Na2SO4(s) is fully dissolved in water to make 6.78 mL of solution, the reaction…

A: Sodium sulphate dissolves in water to give two moles of sodium ions and one mole of sulphate ions.

Q: Given these reactions, X(6) + 0,@) – xO(6) AH = -653.9 kJ/mol XCo,(6) – XO(s) + CO,(g) AH = +444.5…

A: If two reactions are added then ∆H value also added.

Q: 6A + 2C 6D Determine the enthalpy(AH) in kJ of the above reaction using the reactions below: 6B 2C…

A: The enthalpy change is a state function and the Hess law states that the change of enthalpy in a…

Q: Determine the enthalpy (in kJ/mol) for the reaction 3 SiCl₄ (s) + 4 Fe (s) → 4 FeCl₃ (s) + 3 Si (s)…

A: To solve this we have to do some mathematical operations with the given two equations to get the…

Q: The bombardier beetle uses an explosive discharge as a defensive measure. The chemical reaction…

A: The given reaction is, C6H4(OH)2(aq) + H2O2(aq) ---> C6H4O2(aq) + 2H2O(l) The given data…

Q: Determine how much energy in kJ is absorbed when 6.03 g of HA, the limiting reactant, are completely…

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

**Experiment 3: Redox Reaction of Calcium and Water**

A student conducted an experiment to measure the change in enthalpy (ΔH) for the redox reaction:

\[ \text{Ca}(s) + \text{H}_2\text{O}(l) \rightarrow \text{Ca(OH)}_2(aq) + \text{H}_2(g) \]

In this experiment, 0.6418 g of calcium (Ca) was added to 200.0 mL of distilled water contained in a styrofoam cup. The observed change in temperature was +8.4°C. The density of the water used was 1.00 g/mL.

**Tasks:**

a. **Oxidation and Reduction:**
- Identify which element is being oxidized and which is reduced.

b. **Energy Absorption by Calorimeter:**
- Calculate the energy absorbed by the calorimeter. Use \( C_{\text{cal}} = 20. \, \text{J/°C} \).

c. **Energy Absorption by Solution:**
- Calculate the energy absorbed by the solution. Use \( S_{\text{soln}} = 4.184 \, \text{J/g°C} \).
- Note that \( m_{\text{soln}} \) is the combined weight of water and calcium dissolved into the water.

d. **Total Energy Released:**
- Calculate the total energy released by the reaction.

e. **Enthalpy of Reaction (per gram of calcium):**
- Calculate the enthalpy change (ΔH) per gram of calcium.

f. **Enthalpy of Reaction (per mole of calcium):**
- Calculate the enthalpy change (ΔH) per mole of calcium.

These calculations will help in understanding the thermodynamics of the reaction under study.

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

Answer to (a)

Answer to (b)

Answer to part (c)

Trending now

This is a popular solution!

Step by step

Solved in 4 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

What reaction corresponds to the heat of formation of solid Mg(NO3)2
How much energy in kJ is released when 14.17 g of aluminum react with an excess of copper oxide? 3 CuO + 2 Al -> 3 Cu + Al2O3 △ H = 1190 kJ/mol
For each reaction, write the chemical formulae of the oxidized reactants in the space provided. Write the chemical formulae of the reduced reactants in the space provided. reactants oxidized: Al (s) + FeBr, (aq) AlBr, (aq) + Fe(s) reactants reduced: reactants oxidized: Cu Cl, (aq) + Mg(s) MgCl, (aq) + Cu(s) reactants reduced: reactants oxidized: Pb(s) + Hg (NO,),(aq) → Hg (1) + 2 reactants reduced:
The copper mineral chalcocite, Cu2S, can be converted to copper simply by heating in air: Cu,S(s) + 0,(g) → 2Cu(s) + SO, (g)
A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 22.4 mL of 6.45 M hydrochloric acid. The temperature of the mixture rises 17.2 ° C. The density of the resulting solution is 1.00 g mL and has a specific heat capacity of 4.184 J g · ° C . The heat capacity of the calorimeter is 16.97 J ° C . Part 1: (a) Identify the limiting reagent for the reaction. Part 2: (b) Calculate the heat of reaction (in J). qrxn = × 10 JEnter your answer in scientific notation. Part 3 out of 3 (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization = ____ kj/mol
A chemist measures the enthalpy change AH during the following reaction: 2 Al(OH)3(s)→Al,03(s) + 3 H,0(1) AH=41. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ x10 2 Al,0, (s) + H,0(1) Al(OH), (s) kJ 3 3 Al, O, (s) + 3H,0(1) → 2A1(OH), (s) kJ 3 Al(OH), (s) → Al, 0, (s) + H,0() |kJ 3
In a constant-pressure calorimeter, 70.0 mL of 0.340 M Ba(OH), was added to 70.0 mL of 0.680 M HCI. The reaction caused the temperature of the solution to rise from 24.12 °C to 28.75 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g · °C.) respectively), what is AH for this reaction (per mole H, O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H,O
3
Hello! Need help on these three questions. Thanks a lot!
potential energy diagrams for the following reactions: 2 Ag (s) + Cl2 (g) = 2 AgCl(s) +254 kj
Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCl(aq) → 2 MCI, (aq) + 3 H, (g) AH = -931.0 kJ HCI(g) → HCI(aq) AH2 = -74.8 kJ H,(g) + Cl,(g) → 2 HCI(g) AH3 = -1845.0 kJ 4. MCI, (s) → MCI, (aq) AH, = -118.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g) → 2 MCI, (s) 2. 3.
Consider the reaction: NO,(g) + CO(g) → NO(g) + CO,(g) How many electrons are transferred in this reaction?