Final answer:
The total heat needed to change 3 g of ice at -30.0°C to steam at 130.0°C can be calculated using specific heat capacities and heat of vaporization. First, calculate the heat required to raise the temperature of the ice. Then calculate the heat required to melt the ice. Finally, calculate the heat required to raise the temperature of the water to steam.
Step-by-step explanation:
The total heat needed to change 3 g of ice at -30.0°C to steam at 130.0°C can be calculated using the formula:
Q = mcΔT + mAHv + mcΔT
Where Q is the total heat, m is the mass, c is the specific heat capacity, ΔT is the change in temperature, and AHv is the heat of vaporization.
First, we need to calculate the heat required to raise the temperature of the ice from -30.0°C to its melting point (0.0°C). This can be done using the equation: Q = mcΔT, where m = 3 g, c = 2.09 J/g·°C (specific heat capacity of ice), and ΔT = 0.0°C - (-30.0°C).
Next, we calculate the heat required to melt the ice. This can be done using the equation: Q = mAHv, where m = 3 g and AHv = 334 J/g (heat of fusion of ice).
Lastly, we calculate the heat required to raise the temperature of the water from its melting point (0.0°C) to steam at 130.0°C. This can be done using the equation: Q = mcΔT, where m = 3 g, c = 4.186 J/g·°C (specific heat capacity of water), and ΔT = 130.0°C - 0.0°C.