Questions: How much heat is required to raise the temperature of a 10.35 g sample of carbon tetrachloride from 32.1°C to 56.4°C? The specific heat of carbon tetrachloride is 0.85651 J / g°C.

Solution Steps

We are given the following values:

• Mass of carbon tetrachloride, \( m = 10.35 \, \text{g} \)
• Initial temperature, \( T_i = 32.1^\circ \text{C} \)
• Final temperature, \( T_f = 56.4^\circ \text{C} \)
• Specific heat capacity, \( c = 0.85651 \, \text{J/g}^\circ \text{C} \)

The change in temperature, \(\Delta T\), is calculated as: \[ \Delta T = T_f - T_i = 56.4^\circ \text{C} - 32.1^\circ \text{C} = 24.3^\circ \text{C} \]

The heat required, \( q \), is calculated using the formula: \[ q = m \cdot c \cdot \Delta T \] Substituting the known values: \[ q = 10.35 \, \text{g} \times 0.85651 \, \text{J/g}^\circ \text{C} \times 24.3^\circ \text{C} \]

Calculate the heat required: \[ q = 10.35 \times 0.85651 \times 24.3 = 215.5 \, \text{J} \]

Final Answer