What will be the final temp of the ice of 20g when it is heated to 1600 Cal
What is the initial temp of ice? The final temp of ice is always OC, as it melts at that temperature.
To find the final temperature of the ice when it is heated with 1600 calories of energy, we can use the formula:
Q = m * C * ΔT
Where:
Q = heat energy (in calories)
m = mass of the substance (in grams)
C = specific heat capacity of the substance (in calories/gram °C)
ΔT = change in temperature (in °C)
In this case, we want to find the final temperature, so we need to rearrange the formula:
ΔT = Q / (m * C)
Given:
Q = 1600 calories
m = 20 grams (mass of ice)
C = 0.5 calories/gram °C (specific heat capacity of ice)
Plugging in the values:
ΔT = 1600 calories / (20 grams * 0.5 calories/gram °C)
= 1600 calories / 10 calories/°C
= 160 °C
Therefore, the final temperature of the ice will be 160°C.
To determine the final temperature of the ice when it is heated, we need to consider the heat energy transferred to the ice and the specific heat capacity of ice.
First, we need to calculate the heat energy transferred to the ice using the formula:
Q = m * c * ΔT
Where:
Q = heat energy transferred in calories
m = mass of the ice in grams
c = specific heat capacity of ice (0.5 cal/g°C)
ΔT = change in temperature in °C
Given:
m = 20 g
Q = 1600 cal
c = 0.5 cal/g°C
Rearranging the formula, we can solve for ΔT:
ΔT = Q / (m * c)
Substituting the given values, we have:
ΔT = 1600 cal / (20 g * 0.5 cal/g°C)
= 1600 cal / 10 g°C
= 160 °C
This means that the temperature change of the ice will be 160 °C when heated with 1600 calories of energy.
To find the final temperature, we need to know the initial temperature of the ice. However, if we assume that the initial temperature is 0 °C (since ice is typically at or below its melting point when heated), then the final temperature can be calculated as:
Final temperature = Initial temperature + ΔT
= 0 °C + 160 °C
= 160 °C
Therefore, the final temperature of the ice, assuming an initial temperature of 0 °C, will be 160 °C.