If 335 g of water at 65.5 °C loses 9750 J of heat, what is the final temperature of the water? Liquid water has a specific heat of 4.18 J/(g.°C). °C (Answer a number only, no units. Round to the tenth place). This is an example of an endothermic or exothermic reaction?

Q = mc ΔT

-9750 J = (335 g)(4.18 J/(g.°C))(Tf °C - 65.5 ° C)
Tf = ______ °C

Exothermic processes release heat, while endothermic processes absorb heat.

Exothermic because it loses heat

To find the final temperature of the water, we can use the equation:

\(q = m \cdot c \cdot \Delta T\)

Where:
\(q\) is the heat lost/gained by the water (in this case, -9750 J because heat is lost),
\(m\) is the mass of the water (335 g),
\(c\) is the specific heat of water (4.18 J/(g.°C)),
\(\Delta T\) is the change in temperature.

Rearranging the equation, we can solve for \(\Delta T\):

\(\Delta T = \frac{q}{m \cdot c}\)

Plugging in the values, we have:

\(\Delta T = \frac{-9750 \, \text{J}}{335 \, \text{g} \cdot 4.18 \, \text{J/(g.°C)}}\)

Calculating this gives us \(\Delta T = -6.885 \, \text{°C}\).

Since 65.5 °C - 6.885 °C = 58.615 °C, the final temperature of the water is 58.6 °C (rounded to the nearest tenth).

This is an example of an exothermic reaction because the water lost heat (negative value for \(q\)).

To find the final temperature of the water, we can use the equation:

q = m * c * ΔT

Where:
q is the heat lost or gained by the substance
m is the mass of the substance
c is the specific heat of the substance
ΔT is the change in temperature

In this case, the water loses 9750 J of heat, which is represented by the value of q. The mass of the water is given as 335 g, and the specific heat of water is 4.18 J/(g.°C). We need to find the change in temperature, ΔT.

Rearranging the equation:

ΔT = q / (m * c)

Substituting the given values:

ΔT = 9750 J / (335 g * 4.18 J/(g.°C))

ΔT ≈ 7.23 °C

Since the water starts at 65.5 °C, the final temperature can be calculated as:

Final temperature = Initial temperature - ΔT
Final temperature = 65.5 °C - 7.23 °C

Final temperature ≈ 58.3 °C

Therefore, the final temperature of the water is approximately 58.3 °C.

This is an example of an exothermic reaction because the water loses heat.