if 95j of heat is added to a pure gold coin with a mass of 16 grams, what is its temperature change? Specific heat capacity of gold is 0.128 j/g degrees C.
q = mass Au x specific heat Au x delta T.
To determine the temperature change of the pure gold coin, we can use the equation:
Q = m * c * ΔT
where:
Q = heat energy (in joules)
m = mass of the gold coin (in grams)
c = specific heat capacity of gold (in J/g°C)
ΔT = temperature change (in °C)
Given:
Q = 95 J
m = 16 g
c = 0.128 J/g°C
Let's rearrange the equation to solve for ΔT:
ΔT = Q / (m * c)
Now let's substitute the values:
ΔT = 95 J / (16 g * 0.128 J/g°C)
Simplifying further:
ΔT = 95 J / 2.048 g°C
ΔT ≈ 46.48 °C
Therefore, the temperature change of the gold coin is approximately 46.48 °C.
To calculate the temperature change of the gold coin, we can use the formula for heat:
Q = m * c * ΔT
where:
Q = heat transferred (in joules)
m = mass of the substance (in grams)
c = specific heat capacity of the substance (in joules/gram °C)
ΔT = change in temperature (in °C)
Given values:
Q = 95 J
m = 16 g
c = 0.128 J/g °C
We need to solve for ΔT. Rearranging the formula, we have:
ΔT = Q / (m * c)
Substituting the given values:
ΔT = 95 J / (16 g * 0.128 J/g °C)
Calculating the values:
ΔT = 95 J / (2.048 g °C)
ΔT ≈ 46.48 °C
Therefore, the temperature change of the gold coin when 95 J of heat is added to it is approximately 46.48 °C.
Delta T= (95Joules) / [ (16g Au) X (0.128 J/g C)]
Change of temp= 46Degree celcius