How much ice (in grams) would have to melt to lower the temperature of 53.4g of water from 65 C to 0C?
I know there are more than one step here, I would appreciate an answer that does not do the work for me, but show me how to lay out the problems and in which order... thank you!
the sum of heats gained is zero.
Heatgainedicemelting+heatgainedwater=0
massice*Hf+53.4grams*specificheatwater*(0-65)=0
massice=53.4g*1cal/gramC *53.4C / 80cal/g
= 53.4*65/80 grams
Thank you Bob for your time! I believe there was a misunderstanding in the question,my mistake... C is equal to degree celcius.
Note the correct spelling of celsius.
Celsius is all that is needed. It need not be converted to kelvin.
Thank you again!
To find out how much ice would need to melt to lower the temperature of the water from 65°C to 0°C, you can use the concept of heat transfer.
Here's how you can approach this problem step by step:
Step 1: Calculate the heat lost by the 53.4g of water as it cools from 65°C to 0°C.
To do this, you can use the specific heat capacity of water, which is 4.18 J/g°C. The formula to calculate heat is:
Q = m * C * ΔT
where:
Q = heat transferred (in joules)
m = mass of the substance (in grams)
C = specific heat capacity (in J/g°C)
ΔT = change in temperature (in °C)
In this step, you need to calculate Q.
Step 2: Convert the heat lost by the water to heat gained by the ice.
Since heat is conserved in this process, the heat lost by the water is equal to the heat gained by the ice. We can use the equation:
Q_water = Q_ice
In this step, you already know Q_water from Step 1, and you need to calculate Q_ice.
Step 3: Calculate the mass of ice that would need to melt to absorb the calculated amount of heat.
The heat absorbed by the ice is used to melt it without a change in temperature. The heat required to melt ice is known as the heat of fusion, which is 334 J/g. The formula to calculate the mass of ice is:
m_ice = Q_ice / ΔH_fusion
where:
m_ice = mass of ice (in grams)
Q_ice = heat gained by the ice (in joules)
ΔH_fusion = heat of fusion of ice (in J/g)
In this step, you already know Q_ice from Step 2, and you can use the given value of ΔH_fusion.
By following these steps, you can find out how much ice (in grams) would need to melt to lower the temperature of the water from 65°C to 0°C.