Question

If it takes 7,529 calories of heat to warm 750.0 grams of water, what was the temperature change? The specific heat of water in calories is 1.00 cal/(g•°C).

Answer 1

Answer:

The temperature change was 10.04 °C.

Explanation:

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system. In this way, there is a direct proportional relationship between heat and temperature. The constant of proportionality depends on the substance that constitutes the body as on its mass, and is the product of the specific heat by the mass of the body. So, the equation that allows calculating heat exchanges is:

Q = c * m * ΔT

Where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.

In this case you know:

• Q= 7,529 calories (cal)

• c= 1 $\frac{cal}{g*C}$

• M=750 grams

Replacing:

7,529 cal= 1  $\frac{cal}{g*C}$ *750 g* ΔT

Solving you get:

ΔT=$\frac{7,529 cal}{1 \frac{cal}{g*C}*750 g }$

ΔT= 10.04 °C

So, the temperature change was 10.04 °C.

Answer 2

Answer:

10.04 ° C.

Explanation:

Specific Heat Capacity can be defined as the heat or energy required to raise the temperature of a given mass of the substance by changes in temperature. Specific heat, C has units of cal/g. °C or J/g. °C.

Specific heat can be represented mathematically by using the formula below;

C = Q/ m. ∆T -----------------------------(1).

Where Q= quantity of heat = 7,529 calories, m= mass of the substance= 750.0 grams and ∆T = change in temperature = unknown and C= specific heat= 1.00 cal/(g•°C).

Therefore, slotting the above parameters into equation (1) above we have;

1.00 cal/(g•°C) = 7,529 calories/ 750.0 grams × ∆T.

7,529 calories = 750.0 grams × ∆T × 1.00 cal/(g•°C) .

7,529 = 750.0 ∆T.

∆T = 10.04 °C.