To solve this problem, we need to use the formula for heat transfer:

q = mcΔT

where:
q = heat absorbed or released (in Joules)
m = mass (in grams)
c = specific heat capacity (in J/g°C)
ΔT = change in temperature (in °C)

We know that:
q = 4.689 kJ = 4689 J (since 1 kJ = 1000 J)
m = 34.2 g
c = 0.385 J/g°C

We want to find ΔT, which is (T_final - T_initial). We know that T_initial = 25°C.

Substituting the known values into the formula, we get:

4689 J = 34.2 g * 0.385 J/g°C * ΔT

Solving for ΔT, we get:

ΔT = 4689 J / (34.2 g * 0.385 J/g°C) = 353.5°C

So, the final temperature T_final = T_initial + ΔT = 25°C + 353.5°C = 378.5°C

The closest answer to this is 381°C.

Question

To solve this problem, we need to use the formula for heat transfer:

q = mcΔT

where:
q = heat absorbed or released (in Joules)
m = mass (in grams)
c = specific heat capacity (in J/g°C)
ΔT = change in temperature (in °C)

We know that:
q = 4.689 kJ = 4689 J (since 1 kJ = 1000 J)
m = 34.2 g
c = 0.385 J/g°C

We want to find ΔT, which is (T_final - T_initial). We know that T_initial = 25°C.

Substituting the known values into the formula, we get:

4689 J = 34.2 g * 0.385 J/g°C * ΔT

Solving for ΔT, we get:

ΔT = 4689 J / (34.2 g * 0.385 J/g°C) = 353.5°C

So, the final temperature T_final = T_initial + ΔT = 25°C + 353.5°C = 378.5°C

The closest answer to this is 381°C.

Knowee AI · Accepted Answer