0. A sample of solid iridium is at its melting point of 2466 ∘ C. It has a specific latent heat of fusion of 0.135MJ/kg. How much iridium would be melted if 200 kJ of thermal energy is supplied, assuming that there is no resulting temperature change?
Question
- A sample of solid iridium is at its melting point of 2466 ∘ C. It has a specific latent heat of fusion of 0.135MJ/kg. How much iridium would be melted if 200 kJ of thermal energy is supplied, assuming that there is no resulting temperature change?
Solution
To solve this problem, we need to use the formula for heat transfer during a phase change, which is:
Q = mL
where: Q is the heat energy supplied, m is the mass of the substance, L is the specific latent heat of fusion.
We are given Q = 200 kJ = 200,000 J (since 1 kJ = 1000 J) and L = 0.135 MJ/kg = 135,000 J/kg (since 1 MJ = 1,000,000 J). We need to find m.
Rearranging the formula to solve for m gives us:
m = Q / L
Substituting the given values into this equation gives us:
m = 200,000 J / 135,000 J/kg = 1.48 kg
So, if 200 kJ of thermal energy is supplied, approximately 1.48 kg of iridium would be melted, assuming that there is no resulting temperature change.
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