Calculate the number of joules given off when 32.0 grams of steam cools from 110.0 °C to ice at -40.0 °C.
The amount of energy given off is 99 600 J.
There are five heats to consider:
The total heat evolved is
1. Cooling the Steam For steam, the specific heat capacity, 2. Condensing the Steam 3. Cooling the Water For liquid water, the specific heat capacity, 4. Freezing the Water 5. Cooling the Ice The specific heat capacity of ice, Adding them all up
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To calculate the energy change, use the formula:
Q = mcΔT
Where Q is the heat energy, m is the mass, c is the specific heat, and ΔT is the change in temperature.
For steam to ice transition, you need to consider the heat for cooling steam to water and then freezing water to ice. Use the specific heat values for water and steam, and the heat of fusion for water.
Calculate Q1 for cooling steam to water: Q1 = (32.0 g) * (2.0 J/g°C) * (110.0°C - 100.0°C)
Calculate Q2 for phase change (steam to water): Q2 = (32.0 g) * (2260 J/g)
Calculate Q3 for cooling water to ice: Q3 = (32.0 g) * (4.18 J/g°C) * (-40.0°C - 0.0°C)
Add Q1, Q2, and Q3 to get the total heat energy.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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