Uma massa de gelo de 500 g, inicialmente a uma temperatura de 250 K, é colocada dentro de um recipiente de alumínio de 60 g, em equilíbrio térmico com o gelo. Então, é cedida a esse sistema uma quantidade de calor igual a 60570 Cal, enquanto a pressão é mantida constante. Considerando o ponto de fusão do gelo a 273 K, desprezando as trocas de calor do sistema com o ambiente e sabendo que o calor específico médio da água vale 1 cal/g.ºC, que o calor latente de fusão para o gelo é igual a 80 Cal/g, que o calor específico do gelo vale 0,5 cal/g.ºC e que o calor específico do alumínio é igual a 0,22 cal/g.ºC, ao final desse processo, obtém-se

To solve this problem, we need to break it down into several stages. Initially, we have a 500g ice block at 250K, which is in thermal equilibrium with the 60g aluminum container. Then, 60570 cal of heat is added to the system while maintaining constant pressure. We need to find the final temperature of the system.

First, let's calculate the heat required to raise the temperature of the ice from 250K to 273K (its melting point). The specific heat of ice is 0.5 cal/g°C, so the heat required is:Q = mcΔT = 500g × 0.5 cal/g°C × (273K - 250K) = 1150 cal

Next, we need to calculate the heat required to melt the ice. The latent heat of fusion for ice is 80 cal/g, so:Q = mL = 500g × 80 cal/g = 40000 cal

Now, let's calculate the heat required to raise the temperature of the resulting water from 273K to its final temperature. We'll call this temperature T. The specific heat of water is 1 cal/g°C, so:Q = mcΔT = 500g × 1 cal/g°C × (T - 273K)

The heat required to raise the temperature of the aluminum container is:Q = mcΔT = 60g × 0.22 cal/g°C × (T - 273K)

The total heat added to the system is 60570 cal, which is equal to the sum of the heats required for the above three stages:60570 cal = 1150 cal + 40000 cal + 500g × 1 cal/g°C × (T - 273K) + 60g × 0.22 cal/g°C × (T - 273K)

Simplifying the equation, we get:60570 = 41150 + 500(T - 273) + 13.2(T - 273)

Solving for T, we get:T ≈ 301.3 K

Therefore, the correct answer is B) 301.3 K.

Explanation: We broke down the problem into three stages: raising the temperature of the ice, melting the ice, and raising the temperature of the resulting water and the aluminum container. We calculated the heat required for each stage and set up an equation to find the final temperature of the system. Solving the equation, we get the final temperature as approximately 301.3 K.