The specific heat capacity of silver is 0.24 J/°C·g.
(a) Calculate the energy required to raise the temperature of 140.0 g Ag from 273 K to 295 K.
J
(b) Calculate the energy required to raise the temperature of 1.0 mol Ag by 1.0°C (called the molar heat capacity of silver).
J/mol°C
a)
q = mass Ag x specific heat Ag x (Tf - Ti)
You have mass Ag, sp. H. Ag, and Tf (final T) and Ti (initial T). Solve for q.
b)
You have specific heat Ag which is the energy required to raise 1 g Ag by 1 degree C.
0.24 J/g*c x (107.87 g Ag/mol) = ??
I will be happy to critique your work.
a. energy= mass*c*deltaTemp
b. energy/mole= energy/gram*grams/mole
to find C am i just using the equation from a?
i don't understand b.
You didn't post a c part.
You have specific heat in J/g. So you multiply the molar mass to obtain J/mol.
To calculate the energy required, we can use the formula:
Q = m * c * ΔT
Where Q is the energy required, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
(a) Energy required to raise the temperature of 140.0 g Ag from 273 K to 295 K:
Step 1: Convert the mass to kilograms.
140.0 g Ag = 0.140 kg Ag
Step 2: Calculate the change in temperature.
ΔT = 295 K - 273 K = 22 K
Step 3: Plug the values into the formula and calculate.
Q = 0.140 kg * 0.24 J/°C·g * 22 K = 0.7392 J
Therefore, the energy required to raise the temperature of 140.0 g Ag from 273 K to 295 K is 0.7392 J.
(b) Energy required to raise the temperature of 1.0 mol Ag by 1.0°C:
Step 1: Calculate the molar mass of silver (Ag).
The atomic mass of Ag is 107.87 g/mol.
Step 2: Convert 1.0 mol Ag to grams.
1.0 mol Ag = 1.0 mol * 107.87 g/mol = 107.87 g Ag
Step 3: Calculate the change in temperature.
ΔT = 1.0°C
Step 4: Plug the values into the formula and calculate.
Q = 107.87 g * 0.24 J/°C·g * 1.0°C = 25.8888 J
Therefore, the energy required to raise the temperature of 1.0 mol Ag by 1.0°C is 25.8888 J.