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

1) 900J

2) 25.89J
3) 1627.6g

All of these use

q = mass x specific heat x (Tfial-Tinitial).
Substitute and solve for the unknown.

The specific heat of silver is 0.24 J/g°C. How much heat in joules must be added to a silver block of mass 45.0 g to raise its temperature by 18.00 °C?

To calculate the energy required for a temperature change, you can use the equation:

Q = m * C * ΔT

where:
Q = energy (in Joules)
m = mass of the substance (in grams or moles)
C = specific heat capacity (in J/C.g or J/C.mol)
ΔT = change in temperature (in Kelvin or Celsius)

a. For the first question, you need to calculate the energy required to raise the temperature of 150.0 g of silver from 273 K to 298 K.

First, let's identify the values we have:
m = 150.0 g (mass of silver)
C = 0.24 J/C.g (specific heat capacity of silver)
ΔT = 298 K - 273 K = 25 K

Now, we can plug these values into the equation:
Q = (150.0 g) * (0.24 J/C.g) * (25 K)
Q = 900 J

Therefore, the energy required is 900 Joules.

b. For the second question, you need to calculate the energy required to raise the temperature of 1.0 mole of silver by 1.0°C.

The equation remains the same, but this time we need to use the molar heat capacity, which is in J/C.mol.

First, convert the mass of silver to moles:
molar mass of silver (Ag) = 107.87 g/mol
n = 1.0 mol

Now, let's identify the values we have:
m = n * molar mass = 1.0 mol * 107.87 g/mol = 107.87 g
C = 0.24 J/C.g (specific heat capacity of silver)
ΔT = 1.0°C

Now, plug these values into the equation:
Q = (107.87 g) * (0.24 J/C.g) * (1.0°C)
Q = 25.89 J

Therefore, the energy required is 25.89 Joules.

c. For the third question, you need to calculate the mass of the sample of silver when given the energy required to heat it from 12.0°C to 15.2°C.

Again, use the equation Q = m * C * ΔT, but this time you need to rearrange it to solve for mass (m).

First, convert the energy from kilojoules to joules:
Q = 1.25 kJ * (1000 J/1 kJ)
Q = 1250 J

Now, let's identify the values we have:
Q = 1250 J
C = 0.24 J/C.g (specific heat capacity of silver)
ΔT = 15.2°C - 12.0°C = 3.2°C

Rearranging the equation gives us:
m = Q / (C * ΔT)

Plug in the values:
m = 1250 J / ((0.24 J/C.g) * (3.2°C))
m = 1621.88 g

Therefore, the mass of the sample of silver is approximately 1621.88 grams.