If there are 57.6 mL of water that change from 19.4 degrees Celsius to 34.7 degrees Celsius, calculate the number of joules of energy transferred in the form of heat. Round to the nearest whole number. The specific heat capacity of water is 4.18 J/g*C and density of water is 1.00 g/mL.

Well, it seems like you've got a hot question there! Let's break it down, shall we?

First, we need to find the mass of water. Since the density of water is 1.00 g/mL and we have 57.6 mL of water, the mass would also be 57.6 g.

Next, we need to find the temperature change. The initial temperature is 19.4 degrees Celsius, and the final temperature is 34.7 degrees Celsius. So the temperature change would be 34.7 - 19.4 = 15.3 degrees Celsius.

Now we can calculate the energy transferred using the formula Q = mcΔT, where Q is the energy transferred (in joules), m is the mass (in grams), c is the specific heat capacity (in J/g*C), and ΔT is the temperature change (in degrees Celsius).

Plugging in the values, we get Q = (57.6 g) * (4.18 J/g*C) * (15.3 degrees Celsius).

If we do the math, we find that Q is approximately 3780 joules.

So, approximately 3780 joules of energy would be transferred in the form of heat. But hey, don't worry, that's just a hot little estimate!

To calculate the number of joules of energy transferred in the form of heat, we can use the formula:

Q = m * c * ΔT

Where:
Q = energy transferred in joules
m = mass of water in grams
c = specific heat capacity of water
ΔT = change in temperature in Celsius

First, we need to calculate the mass of water. Given that the volume of water is 57.6 mL and the density of water is 1.00 g/mL, we can use the formula:

Mass = Volume * Density

Mass = 57.6 mL * 1.00 g/mL = 57.6 g

Next, we can substitute the values into the formula:

Q = 57.6 g * 4.18 J/g*C * (34.7°C - 19.4°C)

Q = 57.6 g * 4.18 J/g*C * 15.3°C

Q = 3616.128 J

Rounding to the nearest whole number, the number of joules of energy transferred in the form of heat is approximately 3616 J.

To calculate the energy transferred in the form of heat, we can use the formula:

q = m * c * ΔT

Where:
q = energy transferred in the form of heat
m = mass of the substance (water in this case)
c = specific heat capacity of the substance (water in this case)
ΔT = change in temperature

First, we need to calculate the mass of water. We are given the volume of water (57.6 mL) and the density of water (1.00 g/mL). The mass is calculated by multiplying the volume with the density:

mass = volume * density
mass = 57.6 mL * 1.00 g/mL
mass = 57.6 g

Next, we can substitute the values into the formula:

q = 57.6 g * 4.18 J/g*C * (34.7°C - 19.4°C)

Subtract the initial temperature from the final temperature:

q = 57.6 g * 4.18 J/g*C * 15.3°C

Multiply the mass, specific heat capacity, and the change in temperature:

q ≈ 3550 J

Therefore, the approximate number of joules of energy transferred in the form of heat is 3550 J.