Give the specific heat values: Au- 0.128, Ag- 0.235, Cu- 0.385. Fe- 0.449, Al- 0.903. What is the identity of a 10.0 g metal sample that is increased by 14/0 degrees C when 62.9 J of energy is absorbed?
Well, if we look at the heat capacity values you provided, we can see that Au (gold) has a specific heat value of 0.128, Ag (silver) has a specific heat value of 0.235, Cu (copper) has a specific heat value of 0.385, Fe (iron) has a specific heat value of 0.449, and Al (aluminum) has a specific heat value of 0.903.
To identify the metal sample, we can calculate the heat absorbed using the formula Q = mcΔT, where Q is the heat absorbed, m is the mass, c is the specific heat, and ΔT is the change in temperature.
Given that the heat absorbed is 62.9 J, the change in temperature is 14.0 °C, and the mass is 10.0 g, we can use these values to calculate the specific heat. Rearranging the formula, we get c = Q / (m * ΔT).
So, for the given metal sample, the specific heat would be approximately:
c = 62.9 J / (10.0 g * 14.0 °C)
c ≈ 0.449 J/g°C
Comparing this value to the specific heat values provided, we find that it matches the specific heat value for Fe (iron) which is 0.449. Therefore, the identity of the metal sample is iron (Fe).
To determine the identity of the metal sample, we can use the formula:
\(q = m \cdot c \cdot \Delta T\)
where:
- \(q\) is the heat absorbed (in joules)
- \(m\) is the mass of the sample (in grams)
- \(c\) is the specific heat of the metal (in J/g°C)
- \(\Delta T\) is the change in temperature (in °C)
First, rearrange the formula to solve for the specific heat (\(c\)):
\(c = \frac{{q}}{{m \cdot \Delta T}}\)
Now, substitute the given values into the formula:
\(c = \frac{{62.9 \, \text{J}}}{{10.0 \, \text{g} \cdot \frac{{14}}{{0}} \, \text{°C}}}\)
Simplifying this expression:
\(c = \frac{{62.9}}{{10.0 \cdot \frac{{14}}{{0}}}}\)
\(c = \frac{{62.9}}{{140}}\)
\(c = 0.449\)
Comparing the calculated specific heat value (0.449) to the given specific heat values, we can see that it matches the value for Fe (iron). Therefore, the identity of the metal sample is iron (Fe).
To determine the identity of the metal, we need to calculate its specific heat. The formula for specific heat is:
Q = m * c * ΔT
Where:
- Q is the energy absorbed or released (in joules)
- m is the mass of the sample (in grams)
- c is the specific heat of the substance (in J/g°C)
- ΔT is the change in temperature (in °C)
We are given:
- mass (m) = 10.0 g
- change in temperature (ΔT) = 14.0 °C
- energy absorbed (Q) = 62.9 J
We can rearrange the equation to solve for specific heat (c):
c = Q / (m * ΔT)
Plugging in the values, we get:
c = 62.9 J / (10.0 g * 14.0 °C)
c = 62.9 J / 140 g°C
c = 0.449 J/g°C
Comparing the calculated specific heat value of 0.449 J/g°C with the given specific heat values for different metals:
- Au: 0.128 J/g°C
- Ag: 0.235 J/g°C
- Cu: 0.385 J/g°C
- Fe: 0.449 J/g°C
- Al: 0.903 J/g°C
We find that the specific heat value of the metal sample matches the specific heat value of Iron (Fe) at 0.449 J/g°C. Therefore, the identity of the metal sample is Iron (Fe).
62.9=10.0*c*14
solve for c
I wonder what the units of those specific heats given are?