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Mass of iron 64.8973 g Mass of water 61.9272 g Initial temperature of iron (boiling water Tm) 98.0 °C Initial temperature of calorimeter + water, T; 22.1 °C Final temperature, T¡ 30.3 °C

Mass of iron 64.8973 g Mass of water 61.9272 g Initial temperature of iron (boiling water Tm) 98.0 °C Initial temperature of calorimeter + water, T; 22.1 °C Final temperature, T¡ 30.3 °C

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please how I find the q Fe,q water, q cal with the ungrounded and rounded  values please. 

### Temperature Change - **ΔT for iron, °C**: -67.7 - **ΔT for water, °C**: 8.2 (Both values are confirmed correct with check marks.) --- ### Heat - **The specific heat of water**: 4.184 J g⁻¹ K⁻¹ - **The specific heat of iron**: 0.450 J g⁻¹ K⁻¹ #### Heat Values (in Joules) - **qFe (Iron)** - Unrounded: [editable field] - Rounded: [locked field] - **qwater (Water)** - Unrounded: [editable field] - Rounded: [locked field] - **qCal (Calorimeter)** - Unrounded: [editable field] - Rounded: [locked field] (Note: The placeholders for heat values are indicated and have options for selecting decimal places.) This section provides details on calculating temperature changes and heat interactions involving iron and water, emphasizing the importance of rounding in scientific calculations.
Transcribed Image Text:### Temperature Change - **ΔT for iron, °C**: -67.7 - **ΔT for water, °C**: 8.2 (Both values are confirmed correct with check marks.) --- ### Heat - **The specific heat of water**: 4.184 J g⁻¹ K⁻¹ - **The specific heat of iron**: 0.450 J g⁻¹ K⁻¹ #### Heat Values (in Joules) - **qFe (Iron)** - Unrounded: [editable field] - Rounded: [locked field] - **qwater (Water)** - Unrounded: [editable field] - Rounded: [locked field] - **qCal (Calorimeter)** - Unrounded: [editable field] - Rounded: [locked field] (Note: The placeholders for heat values are indicated and have options for selecting decimal places.) This section provides details on calculating temperature changes and heat interactions involving iron and water, emphasizing the importance of rounding in scientific calculations.
**Data:** - **Mass of iron**: 64.8973 g - **Mass of water**: 61.9272 g - **Initial temperature of iron (boiling water, \( T_m \))**: 98.0 °C - **Initial temperature of calorimeter + water, \( T_i \)**: 22.1 °C - **Final temperature, \( T_f \)**: 30.3 °C This data might be used in an experiment to determine the heat capacity of materials, likely involving a calorimeter setup. The temperatures recorded indicate the initial conditions of the substances involved and the equilibrium temperature reached during the process.
Transcribed Image Text:**Data:** - **Mass of iron**: 64.8973 g - **Mass of water**: 61.9272 g - **Initial temperature of iron (boiling water, \( T_m \))**: 98.0 °C - **Initial temperature of calorimeter + water, \( T_i \)**: 22.1 °C - **Final temperature, \( T_f \)**: 30.3 °C This data might be used in an experiment to determine the heat capacity of materials, likely involving a calorimeter setup. The temperatures recorded indicate the initial conditions of the substances involved and the equilibrium temperature reached during the process.
Expert Solution
Step 1

Given: 

Specific heat of iron = 0.450 J/g K

Specific heat of water = 4.184 J/g K

Specific heat is heat taken for 1 g of a substance to raise its temperature by 10 C or 1 K. It is denoted by small c.

Now,

heat, q = m c ∆T                                                    ........equation (1)

where m = mass of susbtance

c=  specific heat of substance

 ∆T = Tfinal - Tinitial = change in temperature of the substance

 

 

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