Heat Transfer in Zinc and Water

Heat Transfer Between Zinc and Water

• Heat is being transferred from zinc to water.
• The relationship can be expressed as:
• Q1 = -Q2
  • Here, ( Q1 ) refers to the heat lost by zinc, while ( Q2 ) is the heat gained by water.

Zinc Properties

• Mass of zinc (unknown, denote as ( m_{Zn} )).
• Specific heat of zinc: 0.39 J/g°C.
• Initial temperature of zinc: 5.2 °C.
• Final temperature of zinc (after energy loss): 42.5 °C.
• Change in temperature for zinc:
• ( \Delta T{Zn} = T{final} - T_{initial} )
• ( \Delta T_{Zn} = 42.5 °C - 5.2 °C = -62.7 °C )
  • Sign indicates zinc is losing heat.

Energy Transfer Calculation for Zinc

• Heat lost by zinc can be formulated as:
• Q1 = m{Zn} \times c{Zn} \times \Delta T{Zn}
  • Where:
  • ( Q_1 ) = energy lost by zinc.
  • ( c_{Zn} ) = specific heat of zinc (0.39 J/g°C).
  • ( \Delta T_{Zn} ) = -62.7 °C.

Water Properties

• Mass of water (unknown, denote as ( m_{water} )).
• Final temperature of water: 42.5 °C.
• Initial temperature of water (assume a starting temperature, for calculation purposes).
• Change in temperature for water: ( \Delta T{water} = T{final} - T_{initial} )
• Equation for heat gained by water:
• Q2 = m{water} \times c{water} \times \Delta T{water}
  • Where:
  • ( Q_2 ) = energy gained by water.
  • ( c_{water} ) = specific heat of water, typically ( 4.18 J/g°C ) (use if given).

Connecting the Calculations

• Set equations equal based on conservation of energy:
• m{Zn} \times c{Zn} \times (-62.7) = - (m{water} \times c{water} \times \Delta T_{water})
• Helps to reduce complexity by cancelling out negatives when substituting values.