Calculate the temperature change in the water upon complete melting of the ice. Hint: Determine how much heat is absorbed by the melting ice and then use q =mC*Delta T to calculate the temperature change of the 314 g of water.
under the following conditions:
A 14.7 g ice cube is placed into 314 g of water.
can someone help me?? im completely lost. or can someone help me start the problem? thanks
actually that's the exact problem. they don't have a starting tempereature or anything. that's why i was lost
OK. I didn't read the problem very well. It asks for the temperature CHANGE so water changes by
mass x specific heat x delta T.
And it's the delta T you want to find.
Of course, I'm here to help explain the steps to solving this problem. Let's break it down:
Step 1: Determine how much heat is absorbed by the melting ice.
To calculate the heat absorbed by the melting ice, we can use the equation Q = m * ΔH_f, where Q is the amount of heat absorbed, m is the mass of the ice, and ΔH_f is the heat of fusion for ice.
The heat of fusion for ice is typically given as 334 J/g. So, in this case, ΔH_f = 334 J/g.
Substituting the given mass of the ice cube (14.7 g) into the equation, we can calculate the amount of heat absorbed by the melting ice.
Q = 14.7 g * 334 J/g
Step 2: Calculate the temperature change of the water.
To find the temperature change of the water, we can use the equation Q = m * C * ΔT, where Q is the amount of heat absorbed, m is the mass of the water, C is the specific heat capacity of water, and ΔT is the change in temperature.
The specific heat capacity of water is approximately 4.18 J/g°C.
Substituting the given mass of water (314 g) and the specific heat capacity of water (4.18 J/g°C) into the equation, we can solve for ΔT.
Q = 314 g * 4.18 J/g°C * ΔT
Step 3: Solve for ΔT.
Since the amount of heat absorbed by the ice in Step 1 is equal to the amount of heat absorbed by the water in Step 2, we can set the two equations equal to each other and solve for ΔT.
14.7 g * 334 J/g = 314 g * 4.18 J/g°C * ΔT
Simplifying the equation, we have:
4894.8 J = 1310.52 g°C * ΔT
Now, we can solve for ΔT:
ΔT = 4894.8 J / (1310.52 g°C)
Follow the hint.
How much heat is required to melt the ice? That will be 14.7 g x heat fusion = ??. That will melt the ice and leave it at zero.
But you failed to provide the temperature of the 314 g H2O so that's all the help I can offer.