The initial temperature of a bomb calorimeter is 28.50°C. When a chemist carries out a reaction in this calorimeter, its temperature decreases to 27.45°C.

If the calorimeter has a mass of 1.400 kg and a specific heat of 3.52 J/(gi°C), how much heat is absorbed by the reaction?

Well, it seems the reaction was really cool, literally! Let's calculate the heat absorbed using some numerical fun. We can use the formula:

q = mcΔT

Where:
q is the heat absorbed,
m is the mass of the calorimeter,
c is the specific heat of the calorimeter, and
ΔT is the change in temperature.

Given that:
m = 1.400 kg,
c = 3.52 J/(gi°C),
ΔT = 27.45°C - 28.50°C = -1.05°C.

Now, let's plug these values into the equation:

q = (1.400 kg) * (3.52 J/(gi°C)) * (-1.05°C)

And after crunching the numbers, voila! We find that the heat absorbed by the reaction is approximately equal to -5.592 J. So it looks like the reaction absorbed a negative amount of heat. Perhaps that's why the temperature decreased!

To calculate the heat absorbed by the reaction, we can use the formula:

q = mcΔT

Where:
q = heat absorbed by the reaction
m = mass of the calorimeter
c = specific heat of the calorimeter
ΔT = change in temperature

Given:
Initial temperature (T1) = 28.50°C
Final temperature (T2) = 27.45°C
Mass of the calorimeter (m) = 1.400 kg
Specific heat of the calorimeter (c) = 3.52 J/(g·°C)

First, we need to convert the mass from grams to kilograms:
m = 1.400 kg

Next, calculate the change in temperature (ΔT):
ΔT = T2 - T1
= 27.45°C - 28.50°C
= -1.05°C

Now we can calculate the heat absorbed by the reaction:
q = mcΔT
= (1.400 kg) (3.52 J/(g·°C)) (-1.05°C)

Converting mass to grams:
= (1400 g) (3.52 J/(g·°C)) (-1.05°C)

Multiplying the values:
= -5196 J

Therefore, the heat absorbed by the reaction is -5196 J. Note that the negative sign indicates that the reaction released heat.

To find the amount of heat absorbed by the reaction, we need to use the formula:

Q = mcΔT

Where:
Q is the amount of heat absorbed/lost by the system (in this case, the reaction),
m is the mass of the calorimeter,
c is the specific heat of the calorimeter, and
ΔT is the change in temperature.

Given:
Initial temperature (Ti) = 28.50°C
Final temperature (Tf) = 27.45°C
Mass of the calorimeter (m) = 1.400 kg
Specific heat of the calorimeter (c) = 3.52 J/(g°C)

First, we need to calculate the change in temperature (ΔT):

ΔT = Tf - Ti
= 27.45°C - 28.50°C
= -1.05°C

The negative sign indicates a decrease in temperature.

Now, we can calculate the amount of heat (Q) absorbed by the reaction:

Q = mcΔT
= (1.400 kg) * (3.52 J/(g°C)) * (-1.05°C)
= -5.8632 kJ

The negative sign indicates that heat is lost by the calorimeter/reaction.

Therefore, the amount of heat absorbed by the reaction is approximately -5.8632 kJ.