A 6.75-g sample of gold (specific heat capacity = 0.130 J/g °C) is heated using 55.8 J of energy. If the original temperature of the gold is 25.0°C, what is its final temperature?
i got 88.6 degree celcius is it right?
q = mass Au x specific heat Au x (Tfinal-Tinitial)
right
Q=m*s*dT
To find the final temperature of the gold, we can use the formula:
Q = m * c * ΔT
Where:
Q is the amount of energy transferred to the substance (in joules),
m is the mass of the substance (in grams),
c is the specific heat capacity of the substance (in J/g °C),
ΔT is the change in temperature (in °C).
In this case, we know:
Q = 55.8 J
m = 6.75 g
c = 0.130 J/g °C
ΔT = ?
Rearranging the formula, we have:
ΔT = Q / (m * c)
Substituting the given values, we get:
ΔT = 55.8 J / (6.75 g * 0.130 J/g °C)
Simplifying further:
ΔT = 55.8 J / 0.8775 J/°C
Calculating:
ΔT = 63.57 °C
Since we want to find the final temperature, we add ΔT to the initial temperature:
Final temperature = Initial temperature + ΔT
Final temperature = 25.0 °C + 63.57 °C
Final temperature ≈ 88.6 °C
Therefore, the final temperature of the gold is approximately 88.6 °C.