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1 Calculate the amount of heat needed to raise the temperature of 50.0 g of iron from 21.0°C to 100°C. The specific heat capacity of iron is 0.450 J g-¹ °C-¹. Colaul

1 Calculate the amount of heat needed to raise the temperature of 50.0 g of iron from 21.0°C to 100°C. The specific heat capacity of iron is 0.450 J g-¹ °C-¹. Colaul

Chemistry
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...
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1 Calculate the amount of heat needed to raise the temperature of 50.0 g of iron from 21.0°C to 100°C. The specific heat capacity of iron is 0.450 J g-¹ °C-1. 2 Calculate the temperature reached when 100 g of water at 18.2°C absorbs 9.45 kJ of heat energy. The specific heat capacity of water is 4.18 J g-¹°C-1. 3 Draw labelled energy level diagrams for the following reactions: - a S(s) + O₂(g) → SO₂(g) AH* = -297 kJ mol-1 b 6C0₂(aq) + 6H₂O(l) →→ C6H₁206(aq) + 60₂(g) 12 AH = +2800 kJ mol-¹ C6H₁2O6 Wais
Transcribed Image Text:1 Calculate the amount of heat needed to raise the temperature of 50.0 g of iron from 21.0°C to 100°C. The specific heat capacity of iron is 0.450 J g-¹ °C-1. 2 Calculate the temperature reached when 100 g of water at 18.2°C absorbs 9.45 kJ of heat energy. The specific heat capacity of water is 4.18 J g-¹°C-1. 3 Draw labelled energy level diagrams for the following reactions: - a S(s) + O₂(g) → SO₂(g) AH* = -297 kJ mol-1 b 6C0₂(aq) + 6H₂O(l) →→ C6H₁206(aq) + 60₂(g) 12 AH = +2800 kJ mol-¹ C6H₁2O6 Wais
4 Write the thermochemical equation that represents: a the combustion of butane, C4H₁0(g) b the formation of butane 5 Draw a Hess's law cycle and use it, together with the data given, to calculate the enthalpy change for the reaction: P(s) + 12Cl₂(g) → PCL3 (1) Data: P(s) + 2Cl₂(g) → PCL5 (s) AH=-463 kJ mol-1 PCl₂(l) + Cl₂(g) →→→ PCL,(s) AH = -124 kJ mol-¹
Transcribed Image Text:4 Write the thermochemical equation that represents: a the combustion of butane, C4H₁0(g) b the formation of butane 5 Draw a Hess's law cycle and use it, together with the data given, to calculate the enthalpy change for the reaction: P(s) + 12Cl₂(g) → PCL3 (1) Data: P(s) + 2Cl₂(g) → PCL5 (s) AH=-463 kJ mol-1 PCl₂(l) + Cl₂(g) →→→ PCL,(s) AH = -124 kJ mol-¹
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