3. A 74.5 g piece of metal at 86.0°C is placed in 133 g of water at 21.0°C contained in a calorimeter. The metal and water come to the same temperature at 24.2°C. How much heat (in J) did the metal give up to the water? (Assume the specific heat of water is 4.18 J/g·°C across the temperature range.) JWhat is the specific heat (in J/g·°C) of the metal? J/g·°C4. A 0.528 g sample of KCl is added to 51.7 g of water in a calorimeter. If the temperature decreases by 1.07°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C? JIs the reaction exothermic or endothermic?exothermicendothermic 5. When 2.56 g of methane burns in oxygen, 128 kJ of heat is produced. What is the enthalpy of combustion (in kJ) per mole of methane under these conditions? kJ/mol methane6. Joseph Priestly prepared oxygen in 1774 by heating red mercury(II) oxide with sunlight focused through a lens. How much heat (in kJ) is required to decompose 1.18 mol of red HgO(s) to Hg(l) and O2(g) under standard conditions? kJCalculate ΔH (in kJ) for the process Hg2Br2(s) → 2 Hg(l) + Br2(l) from the following information.Hg(l) + Br2(l) → HgBr2(s) ΔH⁰298 = −170.7 kJ Hg(l) + HgBr2(s) → Hg2Br2(s) ΔH⁰298 = −36.2 kJ kJ8. Using the Supplemental Data, calculate the standard enthalpy change (in kJ/mol) for each of the following reactions.(a) 2 Cu(s) + Cl2(g) → 2 CuCl(s) kJ/mol(b) 2 NaOH(s) + CO2(g) → Na2CO3(s) + H2O(g) kJ/mol(c) Al2O3(s) + 3 H2(g) → 2 Al(s) + 3 H2O(l) kJ/mol(d) Si(s) + 2 Cl2(g) → SiCl4(g) kJ/mol9.The oxidation of the sugar glucose, C6H12O6, is described by the following equation.C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(l) ΔH = −2802.5 kJ/molThe metabolism of glucose gives the same products, although the glucose reacts with oxygen in a series of steps in the body.(a) How much heat in kilojoules can be produced by the metabolism of 13.1 g of glucose? kJ(b) How many Calories can be produced by the metabolism of 13.1 g of glucose? Cal10. Which bond in each of the following pairs of bonds is the strongest?(a) C–C or C≡C C–CC≡C (b) S–H or P–H S–HP–H (c)H–Br or H–FH–BrH–F (d)C–N or C=NC–NC=N (e)C–O or C≡OC–OC≡O (f)C–O or C–NC–OC–N 11. Using the bond enthalpies in the Average Bond Enthalpies table, determine the approximate enthalpy (in kJ) for each of the following reactions. (Assume the average bond enthalpy of the Cl–F bond is 254 kJ/mol.)(a) Cl2(g) + 3 F2(g) → 2 ClF3(g) kJ(b) H2C=CHCH3(g) + H2(g) → H3CCH2CH3(g) kJ(c) 2 CH3(C=O)H(g) + 5 O2(g) → 4 CO2(g) + 4 H2O(g) kJ

“Since you have asked multiple questions, we will solve the first question for you. If you want any specific question to be solved, then please specify the question number or post only that question.” The heat capacity is the ratio of the energy supplied in the form of heat to the rise in the temperature of the system. The mathematical relation for the heat capacity is shown below.Mass of metal = 74.5 g Mass of water =133 g The initial temperature of metal and water is 86.0 oC (359 K) and 21.0 oC (294 K) respectively. The final temperature of the system is 24.2 oC (297.2 K). The specific heat capacity of water is 4.18 J/g. oC. We can assume that, there is no energy lost to the surroundings. Therefore, the heat loss by the ice is equal to the heat gained by the water. The mathematical expression representing this is shown below. Therefore, the specific heat of the metal is 7.49 J/g·°C. Now, we will calculate the heat which will be given up by the metal to the water as follows: Thus, the heat which will be given up by the metal to the water is 61.563 kJ.

Answered: 3. A 74.5 g piece of metal at 86.0°C is…

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

Question

3. A 74.5 g piece of metal at 86.0°C is placed in 133 g of water at 21.0°C contained in a calorimeter. The metal and water come to the same temperature at 24.2°C. How much heat (in J) did the metal give up to the water? (Assume the specific heat of water is 4.18 J/g·°C across the temperature range.)

What is the specific heat (in J/g·°C) of the metal?

J/g·°C

4. A 0.528 g sample of KCl is added to 51.7 g of water in a calorimeter. If the temperature decreases by 1.07°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C?

Is the reaction exothermic or endothermic?

exothermicendothermic

5. When 2.56 g of methane burns in oxygen, 128 kJ of heat is produced. What is the enthalpy of combustion (in kJ) per mole of methane under these conditions?

kJ/mol methane

6. Joseph Priestly prepared oxygen in 1774 by heating red mercury(II) oxide with sunlight focused through a lens. How much heat (in kJ) is required to decompose 1.18 mol of red HgO(s) to Hg(l) and O₂(g) under standard conditions? kJ

Calculate ΔH (in kJ) for the process Hg₂Br₂(s) → 2 Hg(l) + Br₂(l) from the following information.

Hg(l) + Br₂(l) → HgBr₂(s)

ΔH^⁰₂₉₈

= −170.7 kJ Hg(l) + HgBr₂(s) → Hg₂Br₂(s)

ΔH^⁰₂₉₈

= −36.2 kJ

8. Using the Supplemental Data, calculate the standard enthalpy change (in kJ/mol) for each of the following reactions.

(a) 2 Cu(s) + Cl₂(g) → 2 CuCl(s)

kJ/mol

(b) 2 NaOH(s) + CO₂(g) → Na₂CO₃(s) + H₂O(g)

kJ/mol

(c) Al₂O₃(s) + 3 H₂(g) → 2 Al(s) + 3 H₂O(l)

kJ/mol

(d) Si(s) + 2 Cl₂(g) → SiCl₄(g)

kJ/mol

9.The oxidation of the sugar glucose, C₆H₁₂O₆, is described by the following equation.

C₆H₁₂O₆(s) + 6 O₂(g) → 6 CO₂(g) + 6 H₂O(l)

ΔH = −2802.5 kJ/mol

The metabolism of glucose gives the same products, although the glucose reacts with oxygen in a series of steps in the body.

(a) How much heat in kilojoules can be produced by the metabolism of 13.1 g of glucose?

(b) How many Calories can be produced by the metabolism of 13.1 g of glucose?

Cal

10. Which bond in each of the following pairs of bonds is the strongest?

(a) C–C or C≡C C–CC≡C

(b) S–H or P–H S–HP–H

(c)

H–Br or H–F

H–BrH–F

(d)

C–N or C=N

C–NC=N

(e)

C–O or C≡O

C–OC≡O

(f)

C–O or C–N

C–OC–N

11. Using the bond enthalpies in the Average Bond Enthalpies table, determine the approximate enthalpy (in kJ) for each of the following reactions. (Assume the average bond enthalpy of the Cl–F bond is 254 kJ/mol.)

(a) Cl₂(g) + 3 F₂(g) → 2 ClF₃(g)

(b) H₂C=CHCH₃(g) + H₂(g) → H₃CCH₂CH₃(g)

(c) 2 CH₃(C=O)H(g) + 5 O₂(g) → 4 CO₂(g) + 4 H₂O(g)

Expert Solution

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 3 images

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.