Questions: Calculate the heat required to raise the temperature of 28.6 g of sodium from 33.7°C to 73.8°C. The specific heat capacity of sodium is 1.23 J /(g · °C). 1.41 x 10^3 J 932 J 1.19 x 10^3 J 2.60 x 10^3 J

Calculate the heat required to raise the temperature of 28.6 g of sodium from 33.7°C to 73.8°C. The specific heat capacity of sodium is 1.23 J /(g · °C).
1.41 x 10^3 J
932 J
1.19 x 10^3 J
2.60 x 10^3 J
Transcript text: Calculate the heat required to raise the temperature of 28.6 g of sodium from $33.7^{\circ} \mathrm{C}$ to $73.8^{\circ} \mathrm{C}$. The specific heat capacity of sodium is $1.23 \mathrm{~J} /\left(\mathrm{g} \cdot{ }^{\circ} \mathrm{C}\right)$. $1.41 \times 10^{3} \mathrm{~J}$ 932 J $1.19 \times 10^{3} \mathrm{~J}$ $2.60 \times 10^{3} \mathrm{~J}$
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Solution

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Solution Steps

Step 1: Identify the Given Values

We are given:

  • Mass of sodium, \( m = 28.6 \, \text{g} \)
  • Initial temperature, \( T_i = 33.7^\circ \text{C} \)
  • Final temperature, \( T_f = 73.8^\circ \text{C} \)
  • Specific heat capacity of sodium, \( c = 1.23 \, \text{J/g} \cdot {}^\circ \text{C} \)
Step 2: Calculate the Temperature Change

The change in temperature, \(\Delta T\), is calculated as: \[ \Delta T = T_f - T_i = 73.8^\circ \text{C} - 33.7^\circ \text{C} = 40.1^\circ \text{C} \]

Step 3: Use the Heat Formula

The formula to calculate the heat required is: \[ q = m \cdot c \cdot \Delta T \] Substituting the given values: \[ q = 28.6 \, \text{g} \cdot 1.23 \, \text{J/g} \cdot {}^\circ \text{C} \cdot 40.1^\circ \text{C} \]

Step 4: Perform the Calculation

Calculate the heat required: \[ q = 28.6 \times 1.23 \times 40.1 = 1410.1 \, \text{J} \]

Final Answer

The heat required to raise the temperature of 28.6 g of sodium from \(33.7^\circ \text{C}\) to \(73.8^\circ \text{C}\) is \(\boxed{1.41 \times 10^3 \, \text{J}}\).

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