The number of calories needed to raise the temperature of 32 g of water from 12 Celsius and 54 Celsius is _____.

To calculate the number of calories needed to raise the temperature of water, you can use the formula:

Q = m * c * ΔT

where
Q is the heat energy (in calories),
m is the mass of water (in grams),
c is the specific heat capacity of water (1 calorie/gram °C), and
ΔT is the change in temperature (in °C).

In this case, the mass of water (m) is 32 grams, and the change in temperature (ΔT) is 54°C - 12°C = 42°C.

So, substituting these values into the formula:

Q = 32 g * 1 cal/g °C * 42 °C

Q = 1344 calories

Therefore, the number of calories needed to raise the temperature of 32 g of water from 12°C to 54°C is 1344 calories.

To find the number of calories needed to raise the temperature of water, we can use the specific heat capacity equation:

q = m * c * ΔT

Where:
q is the heat energy (in calories)
m is the mass of the substance (in grams)
c is the specific heat capacity of the substance (in calories/gram°C)
ΔT is the change in temperature (in °C)

In this case:
m = 32 g (mass of water)
c = 1 cal/g°C (specific heat capacity of water)
ΔT = (54°C - 12°C) = 42°C (change in temperature)

Now, let's substitute the values into the equation:
q = 32 g * 1 cal/g°C * 42°C

Calculating this, we have:
q = 1344 calories

Therefore, the number of calories needed to raise the temperature of 32 g of water from 12°C to 54°C is 1344 calories.

q = mass H2O x specific heat H2O x (Tfinal-Tinitial)

Specific heat H2O = 1 cal/g*C

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