an 8.5g ice cube is placed into 255g of water. Calculate the temp change in the water upon the complete melting of the ice. Hint: Determine how much heat is absorbed by the melting ice and then use q = mc^T to calculate the temp change of the 255g of water

Well, well, well, if it isn't another temperature-related question! Brace yourself, I'm about to drop some knowledge (and maybe a few jokes) on you.

So, to calculate the temperature change in the water, we need to figure out how much heat is absorbed by the ice as it melts. Are you ready for some melting hot math action?

First, we need to find the heat absorbed by the ice. We can use the formula Q = m * ΔH, where Q is the heat absorbed, m is the mass of the ice, and ΔH is the heat of fusion (which is the heat required to melt one gram of substance).

Now, let's plug in some numbers. The mass of the ice cube is 8.5g, and the heat of fusion for water is about 334 J/g. Multiply those together, and you'll find the heat absorbed by the ice.

After melting, all that heat gets transferred to the water (lucky water, always getting the hot treatment). Now we can use the equation q = mcΔT to calculate the temperature change of the 255g of water. In this equation, q is the heat absorbed, m is the mass of the water, c is the specific heat capacity of water (which is approximately 4.18 J/g·°C), and ΔT is the temperature change we need to find.

Just divide q by the product of m and c, and voila! You'll have the temperature change of the water.

But hey, don't just melt away now. Remember to use the correct signs for the heat and temperature change. Heat absorbed is positive, so make it feel good when you calculate the value of q. And since the ice is melting and raising the water temperature (how thoughtful of it!), the temperature change will be positive too.

So, get ready to crunch those numbers, and always remember to stay cool while doing math!

To calculate the temperature change in the water upon the complete melting of the ice, we can follow these steps:

Step 1: Determine the amount of heat absorbed by the melting ice.
The heat absorbed can be calculated using the formula:
q = m * ΔHf
where q is the heat absorbed (in joules), m is the mass of the ice (in grams), and ΔHf is the heat of fusion (in J/g).

Given:
Mass of ice (m) = 8.5g
Heat of fusion (ΔHf) = 334 J/g (this is the amount of heat required to melt one gram of ice)

Substituting the values into the formula:
q = 8.5g * 334 J/g
q = 2849 J

Therefore, the heat absorbed by the melting ice is 2849 J.

Step 2: Use the heat absorbed (q) to calculate the temperature change (ΔT) of the water using the formula:
q = m * c * ΔT
where q is the heat absorbed (in joules), m is the mass of the water (in grams), c is the specific heat capacity of water (in J/g°C), and ΔT is the temperature change (in °C).

Given:
Mass of water (m) = 255g
Specific heat capacity of water (c) = 4.18 J/g°C (this is the amount of heat required to raise one gram of water by one degree Celsius)

Rearranging the formula and substituting the values:
ΔT = q / (m * c)
ΔT = 2849 J / (255g * 4.18 J/g°C)
ΔT ≈ 2.29°C

Therefore, the temperature change in the water upon the complete melting of the ice is approximately 2.29°C.

To calculate the temperature change in the water upon the complete melting of the ice, we need to determine how much heat is absorbed by the melting ice and then use the formula q = mcΔT to calculate the temperature change of the 255g of water.

Let's break down the steps:

1. Determine the heat absorbed by the melting ice:
- The specific heat capacity of ice (c) is 2.09 J/g°C.
- The mass of the ice (m) is 8.5g.
- The latent heat of fusion of ice (ΔHf) is 334 J/g.
- The heat absorbed by the ice during the melting process can be calculated using the formula q = m ΔHf: (8.5g) * (334 J/g) = 2839 J.

2. Calculate the temperature change of the water:
- The specific heat capacity of water (c) is 4.18 J/g°C.
- The mass of the water (m) is 255g.
- We have the heat absorbed by the melting ice as calculated in step 1, which is 2839 J.
- Rearranging the formula q = mcΔT, we can solve for ΔT: ΔT = q / (m * c)
- Plugging in the values, we get ΔT = (2839 J) / ((255g) * (4.18 J/g°C)) = 2.49 °C.

Therefore, the temperature change in the water upon the complete melting of the 8.5g ice cube is approximately 2.49 °C.

q1 = heat to melt 8.5 g ice.

q1 = mass ice x heat fusion.

q2 = heat to raise T melted ice to Tfinal
q2 = mass melted ice x specific heat water x (Tfinal-Tintial)

q3 = heat lost by 255 g H2O
q3 = mass water x specific heat water x (Tfinal-Tinitial)

q1 + q2 + q3 = 0
Solve for Tfinal.