A.) A scientist adds 193 g of water at 51°C to ice at 0°C. If the final temperature of this closed system is 0°C, determine HOW MUCH ICE MELTED.B.) The scientist then adds 0.23 kg of steam at 100°C to 1.02 kg of ice at 0°C. Determine the temperature of the mixture once thermal equilibrium is reached. ### Specific Heat Capacities of Substances#### Solids- **Aluminum**: 900 J/kg·K- **Brass**: 402 J/kg·K- **Copper**: 377 J/kg·K- **Glass**: 840 J/kg·K- **Gold**: 126 J/kg·K- **Ice**: 2095 J/kg·K- **Iron**: 461 J/kg·K- **Lead**: 130 J/kg·K- **Nickel**: 502 J/kg·K- **Silver**: 239 J/kg·K- **Styrofoam**: 1131 J/kg·K- **Zinc**: 390 J/kg·K#### Liquids- **Bromine**: 473 J/kg·K- **Ethyl Alcohol**: 2400 J/kg·K- **Gasoline**: 2220 J/kg·K- **Glycerin**: 2430 J/kg·K- **Mercury**: 140 J/kg·K- **Water**: 4186 J/kg·K#### Latent Heat of SubstancesA table shows the latent heat values for phase changes:- **Steam ⇌ Water**: 2,260,000 J/kg- **Ice ⇌ Water**: 333,000 J/kgEach column represents the specific heat capacity values for different materials, comparing solids and liquids. Additionally, the latent heat table provides the energy required for phase changes between steam and water, and ice and water.

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