The specific heat of solid gold is 0.13 J/g • °C. How much heat is needed to raise the temperature of 25.0 g of gold from 23°C to its melting point at 1063°C?
just looking at the units involved, I'd say
.13J/g°C * 25.0g * (1063-23)°C = 3380J
Well, well, well! Let's calculate that heat, shall we? Now, the heat needed can be found using the formula: Q = m * c * ΔT, where Q is the heat, m is the mass, c is the specific heat, and ΔT is the change in temperature.
So, we have:
m = 25.0 g
c = 0.13 J/g • °C
ΔT = (1063°C - 23°C)
Now just plug in those values and calculate:
Q = 25.0 g * 0.13 J/g • °C * (1063°C - 23°C)
Careful with the math, though! Don't want to melt your brain before the gold!
To calculate the heat needed to raise the temperature of a substance, we can use the formula:
q = m * c * ΔT
where:
q = heat (in Joules)
m = mass (in grams)
c = specific heat capacity (in J/g • °C)
ΔT = change in temperature (in °C)
Given:
m = 25.0 g (mass of gold)
c = 0.13 J/g • °C (specific heat of gold)
ΔT = (1063°C - 23°C) = 1040°C
Substituting the given values into the formula, we can calculate the heat (q):
q = 25.0 g * 0.13 J/g • °C * 1040°C
q = 3380 Joules
Therefore, the heat needed to raise the temperature of 25.0 g of gold from 23°C to its melting point at 1063°C is 3380 Joules.
To calculate the amount of heat needed to raise the temperature of a substance, we can use the formula:
Q = m * c * ΔT
Where:
Q represents the amount of heat (in joules)
m represents the mass of the substance (in grams)
c represents the specific heat capacity of the substance (in J/g • °C)
ΔT represents the change in temperature (in °C)
In this case, we are given:
m = 25.0 g (mass of gold)
c = 0.13 J/g • °C (specific heat of gold)
ΔT = 1063°C - 23°C (change in temperature)
Now let's calculate the amount of heat required:
ΔT = 1063°C - 23°C = 1040°C
Q = 25.0 g * 0.13 J/g • °C * 1040°C
Multiply the values:
Q = 338 J
Therefore, it will take 338 joules of heat to raise the temperature of 25.0 g of gold from 23°C to its melting point at 1063°C.