The specified heat capacity of silver is 0.24 J/C.g. Please help with this Ap chem quastion.?
a. Calculate the energy required to raise the temperature of 150.0 g Ag from 273 K to 298.
b. Calculate the energy required to raise the temperature of 1.0 mol Ag by 1.0C (called the molar heat capacity of silver).
c. It takes 1.25 Kj of energy to heat a sample of pure silver from 12.0C to 15.2C. Calculate the mass of the sample of silver
Heat energy= mass*specificheatcapacity*(Tf-Ti)
Can you take if from here?
I gave the information to work all of these. Surely you can plug in the numbers.
To solve these questions, you need to use the equation Q = mcΔT, where Q is the heat energy transferred, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature.
a. First, we need to convert the given mass of silver from grams to kilograms (since the specific heat capacity is given in J/C.g).
150.0 g Ag = 0.150 kg Ag
Then, we can calculate the energy required using the equation Q = mcΔT:
Q = (0.150 kg)(0.24 J/C.g)(298 K - 273 K)
Q = (0.150 kg)(0.24 J/C.g)(25 K)
Q = 0.90 J (or 0.9 J)
Therefore, the energy required to raise the temperature of 150.0 g of silver from 273 K to 298 K is 0.9 J.
b. The molar heat capacity (C) is defined as the energy required to raise the temperature of 1 mole of a substance by 1 degree Celsius.
To calculate the molar heat capacity of silver, we need to determine the number of moles of silver in 1.0 mol.
Using the molar mass of silver, which is approximately 107.87 g/mol, we can convert the given mass of silver (1.0 mol Ag) to grams:
1.0 mol Ag = 1.0 mol Ag * 107.87 g/mol = 107.87 g Ag
Using the equation Q = mcΔT, we can calculate the energy required:
Q = (107.87 g)(0.24 J/C.g)(1.0 C)
Q = 25.88 J/mol.C
Therefore, the energy required to raise the temperature of 1 mole of silver by 1.0 C is 25.88 J/mol.C.
c. The equation Q = mcΔT can be rearranged to solve for mass:
m = Q / (cΔT)
First, we need to convert the given energy (1.25 kJ) to joules:
1.25 kJ = 1.25 * 10^3 J
Next, we can plug the values into the equation and solve for mass:
m = (1.25 * 10^3 J) / ((0.24 J/C.g)(15.2C - 12.0C))
m = (1.25 * 10^3 J) / (0.72 J/g.C)
m ≈ 1736.1 g
Therefore, the mass of the sample of silver is approximately 1736.1 grams.
To solve these questions, you need to use the specific heat capacity equation:
q = m * c * ΔT
Where:
q is the amount of heat energy,
m is the mass of the substance,
c is the specific heat capacity of the substance, and
ΔT is the change in temperature.
a. To calculate the energy required to raise the temperature of 150.0 g Ag from 273 K to 298 K, you can use the equation mentioned above.
First, convert the temperature to Celsius by subtracting 273 from each value:
ΔT = 298 K - 273 K = 25 °C
Using the equation and rearranging it, we have:
q = m * c * ΔT
q = 150.0 g * 0.24 J/(C.g) * 25 °C
q = 900 J
Therefore, the energy required is 900 J.
b. To calculate the energy required to raise the temperature of 1.0 mol Ag by 1.0 °C, you need to consider the molar heat capacity of silver.
The molar heat capacity (C) is defined as the amount of heat energy required to raise the temperature of one mole of a substance by one degree Celsius.
To calculate the energy, we can use the equation:
q = n * C * ΔT
Where:
q is the amount of heat energy,
n is the number of moles,
C is the molar heat capacity, and
ΔT is the change in temperature.
Since you have 1.0 mol of Ag and you want to raise the temperature by 1.0 °C, simply plug in the values:
q = 1.0 mol * C * 1.0 °C
Unfortunately, the molar heat capacity of silver (C) is not given. It may be necessary to consult a reference source or table to find the specific molar heat capacity value for silver.
c. To calculate the mass of a sample of silver, given that it takes 1.25 kJ of energy to heat it from 12.0 °C to 15.2 °C, we will use the specific heat capacity equation again.
Convert the energy from kilojoules to joules:
1.25 kJ = 1.25 * 10^3 J
Convert the temperature change from Celsius to Kelvin:
ΔT = 15.2 °C - 12.0 °C = 3.2 K
Using the equation again:
q = m * c * ΔT
Rearrange the equation to solve for mass (m):
m = q / (c * ΔT)
m = (1.25 * 10^3 J) / (0.24 J/(C.g) * 3.2 K)
Calculate the mass:
m ≈ 16.28 g
Therefore, the mass of the sample of silver is approximately 16.28 g.