Question

The specific heat capacity of silver is 0.24 J/°C·g.
(a) Calculate the energy required to raise the temperature of 160.0 g Ag from 273 K to 303 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
(c) It takes 1.15 kJ of energy to heat a sample of pure silver from 12.0°C to 15.1°C. Calculate the mass of the sample of silver.
____ in grams

Answer 1

Question #80200

The specific heat capacity of silver is 0.24 J/°C·g.

(a) Calculate the energy required to raise the temperature of 160.0 g Ag from 273 K to 303 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

(c) It takes 1.15 kJ of energy to heat a sample of pure silver from 12.0°C to 15.1°C. Calculate the mass of the sample of silver.

☐ in grams

Answer:

According to the equation $Q = C^{*} \Delta T^{*} m$:

(a) $\Delta T = 303K - 273K = 30^{\circ}C$

$Q = 0.24 * 30 * 160 = 1152 \, \text{J}$

So, the right answer is 1152 J.

(b) $\Delta T = 1^{\circ}C$

1 mole of Ag = 108 g of Ag

$Q = 0.24 * 1 * 108 = 25.92 \, \text{J}$

C = 25.92 J/mol°C

So, the right answer is 25.92 J/mol°C.

(c) $\Delta T = 15.1^{\circ}C - 12.0^{\circ}C = 3.1^{\circ}C$

$m = Q / (C^{*} \Delta T) = 1.15 * 1000 / (0.24 * 3.1) = 1545.7 \, \text{g}$

So, the right answer is 1545.7 g.