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To calculate the heat required to melt 22 g of ice at -18°C, we first need to raise the temperature of the ice to 0°C using the specific heat capacity of ice, which is approximately 2.09 J/g°C. The heat required for this step is ( Q_1 = m \cdot c \cdot \Delta T = 22 , \text{g} \cdot 2.09 , \text{J/g°C} \cdot (0 - (-18)) \approx 22 \cdot 2.09 \cdot 18 \approx 8,190 , \text{J} ). Next, we need to melt the ice at 0°C, which requires the heat of fusion of ice, about 334 J/g; thus, ( Q_2 = 22 , \text{g} \cdot 334 , \text{J/g} \approx 7,348 , \text{J} ). The total heat required is ( Q_{total} = Q_1 + Q_2 \approx 8,190 , \text{J} + 7,348 , \text{J} \approx 15,538 , \text{J} ).
What else can I help you with?
What is the measurement of how much heat energy is required for a substance to melt?
The measurement of how much heat energy is required for a substance to melt is called the heat of fusion. It is the amount of energy required to change a substance from a solid to a liquid at its melting point.
How much energy is required to melt 56g?
The energy required to melt a substance can be calculated using the formula: Energy = mass x heat of fusion. For water, the heat of fusion is 334 J/g. Therefore, the energy required to melt 56g of water would be 56g x 334 J/g = 18,704 J.
How much energy is required to melt 10g of ice?
The energy required to melt ice is known as the heat of fusion, which is about 334 joules per gram. Therefore, it would take approximately 3340 joules of energy to melt 10g of ice.
How much heat would be required to raise the temperature of 17.8 g Ag by 22C?
The answer is 4,18 joule.
How much ice melts?
Under standard atmospheric conditions it just needs a temperature above 0˚C and time. If you have a defined mass or ice and external temperature you could find the time required to melt the ice. what may also help is that the latent heat of fusion for water ( the energy required to melt ice) is 334 kJ/kg so if you times that by your mass in kg you will find the energy needed to melt the amount of ice you have.
What is the measurement of how much heat energy is required for a substance to melt?
The measurement of how much heat energy is required for a substance to melt is called the heat of fusion. It is the amount of energy required to change a substance from a solid to a liquid at its melting point.
Can wood be use to melt copper?
No, wood cannot be used to melt copper because the temperature required to melt copper (1,984°F or 1,085°C) is much higher than the ignition point of wood (around 572°F or 300°C). To melt copper, a heat source such as a furnace or a torch that can reach the required temperature must be used.
How much heat is required to melt 2 kg of gold?
The specific heat capacity of gold is 0.129 J/g°C. The heat required to melt 2 kg of gold can be calculated by using the formula Q = m * c * ΔT, where Q is the heat, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature. Assuming gold melts at 1064°C and starting from room temperature (20°C), the total heat required to melt 2 kg of gold is approximately 3.6 x 10^5 Joules.
How much heat does it take to melt 3 kg of helium?
Helium is a gas at room temperature and pressure, so it does not melt. Instead, it turns into a liquid at extremely low temperatures (-268.9°C or -452°F). The amount of heat required to liquefy 3 kg of helium would depend on how much of it is in gas form and the specific heat capacity of helium at that temperature.
How much heat is required to melt 68.5 g of ice at its melting point?
The heat required to melt ice at its melting point is known as the heat of fusion, which is 334 J/g. Therefore, the heat needed to melt 68.5 g of ice is 68.5 g x 334 J/g = 22,939 J.
How much energy is required to melt 1.5 kg gold?
The specific heat of gold is 0.129 J/g°C, and its melting point is 1064°C. The energy required to melt 1.5 kg of gold can be calculated using the formula: Energy = mass * specific heat * temperature change. So, the energy required would be approximately 2.3 x 10^6 Joules.
How much heat is necessary to vaporize 500 grams of ice at its freezing point?
The heat required to vaporize 500 grams of ice at its freezing point is the sum of the heat required to raise the temperature of the ice to its melting point, the heat of fusion to melt the ice, the heat required to raise the temperature of water to its boiling point, and finally the heat of vaporization to vaporize the water. The specific heat capacity of ice, heat of fusion of ice, specific heat capacity of water, and heat of vaporization of water are all needed to perform the calculations.
Is the amount of heat required to boil 1kg of water equal to the amount of heat required to melt 1kg of ice?
No, the amount of heat required to boil 1kg of water is much higher than the amount of heat required to melt 1kg of ice. Boiling water requires additional heat to overcome the latent heat of vaporization, while melting ice only requires heat to overcome the latent heat of fusion.
How much energy is required to melt 56g?
The energy required to melt a substance can be calculated using the formula: Energy = mass x heat of fusion. For water, the heat of fusion is 334 J/g. Therefore, the energy required to melt 56g of water would be 56g x 334 J/g = 18,704 J.
How much heat does it take to melt 2 kg of mercury?
The heat required to melt 2 kg of mercury can be calculated using its specific heat capacity (0.14 J/g°C) and its melting point (−38.83°C). The formula Q = mcΔT can be used to find the heat needed, where Q is the heat, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
How much heat is required to raise the temperature of the room?
The amount of heat required to raise the temperature of a room depends on the room's size, insulation, current temperature, and the desired temperature. It can be calculated using the specific heat capacity of air, room volume, and the temperature difference.
How much energy is required to melt 10g of ice?
The energy required to melt ice is known as the heat of fusion, which is about 334 joules per gram. Therefore, it would take approximately 3340 joules of energy to melt 10g of ice.
