Question

Сколько джоулей энергии должны получить молекулы тающего льда массой 300 г, чтобы получилось 200 г талой воды? Сколько льда должно растаять? - ... кг Температура льда составляет - .... °С Температура получившейся воды будет - ...°С Сколько теплоты пойдёт на плавление? - ... кДж Молекулам льда нужно передать энергию - ...Дж

Answer 1

Растаит 0.2 кг льда
должна быть дана начальная температура льда
сначала лед таит до 0 градусов по формуле 1) 2100*темпер*0.2
потом от льда до воды по формуле 2) 0.2*335 - колво теплоты на плавление
в конце сложи 1) и 2) будет колво переданной энергии льду
температура воды будет 0

Answer 2

It looks like you're asking about the energy required to melt ice and the resulting temperature change. Let's break it down step by step.

Energy Required to Melt Ice:

To calculate the energy required to melt ice, we can use the formula:

Q = m * L

Where: - Q is the energy required (in joules) - m is the mass of the substance undergoing a phase change (in kilograms) - L is the specific latent heat of fusion for the substance (in joules per kilogram)

Given: - Mass of ice (m): 300 g = 0.3 kg - Mass of melted water: 200 g = 0.2 kg

The energy required to melt the ice can be calculated using the specific latent heat of fusion for ice, which is approximately 334,000 joules per kilogram [[1]].

Using the formula: Q = m * L Q = 0.3 kg * 334,000 J/kg Q = 100,200 J

So, the energy required to melt the ice is 100,200 joules.

Amount of Ice to Melt:

To find out how much ice needs to melt to produce 200 g of melted water, we can use the fact that the mass remains constant during a phase change.

Given: - Mass of melted water: 200 g = 0.2 kg

Since the mass remains constant during the phase change, the amount of ice that needs to melt to produce 200 g of melted water is also 200 g, or 0.2 kg.

Initial Temperature of Ice:

The initial temperature of the ice is not provided in the question. However, the standard assumption is that the ice is initially at its freezing point, which is 0°C or 273.15 K.

Final Temperature of Water:

The final temperature of the resulting water can be calculated using the specific heat capacity of water and the energy released during the phase change.

Specific Heat Capacity of Water:

The specific heat capacity of water is approximately 4,184 J/(kg·K) [[2]].

Energy Released During Phase Change:

The energy released during the phase change from ice to water is the same as the energy required to melt the ice, which is 100,200 J.

Using the formula: Q = m * c * ΔT Where: - Q is the energy transferred (in joules) - m is the mass of the substance (in kilograms) - c is the specific heat capacity of the substance (in joules per kilogram per degree Celsius) - ΔT is the change in temperature (in degrees Celsius)

We can calculate the change in temperature of the water.

Change in Temperature of Water:

Q = m * c * ΔT 100,200 J = 0.2 kg * 4,184 J/(kg·K) * ΔT ΔT = 100,200 J / (0.2 kg * 4,184 J/(kg·K)) ΔT ≈ 59.9°C

So, the temperature of the resulting water will increase by approximately 59.9°C.

Energy Required to Melt Ice:

The energy required to melt the ice is 100,200 joules.

Energy Required to Raise Temperature of Water:

The energy required to raise the temperature of the resulting water by approximately 59.9°C is 100,200 joules.

Total Energy Required:

The total energy required is the sum of the energy required to melt the ice and the energy required to raise the temperature of the resulting water: Total Energy = Energy to Melt Ice + Energy to Raise Temperature of Water Total Energy = 100,200 J + 100,200 J Total Energy = 200,400 J

So, the total energy required is 200,400 joules.

I hope this helps! Let me know if you have further questions or need additional assistance.