Question 1: [A] The molar heat cacpacity of silver is 25.35 J/ mol C. How much e

Question

Question 1:

[A] The molar heat cacpacity of silver is 25.35 J/ mol C. How much energy would it take to raise the temperature of 11.1g of silver by 14.2 C?

[B] Find the specific heat of silver?

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Question 2:

[A] A voulume of 120.0 mL of H2O is initally at room temp (22.0 C). A Chilled steel rod at 2.00 C is placed in the water, if the final temp of the system is 21.5 C, what is the mass of the steel bar (in grams)?  Sepecfic heat of H2O = 4.18J/ gC; Heat of Metal = 0.452J/gC

[B] The specific heat of water is 4.18 J/gC. What is the molar heat of capacity of water. Use apporpiriate units.

Explanation / Answer

1.Given -
The molar heat capacity of silver = 25.35 J/mol
Temperature change, ?T = 14.20C
The specific heat capacity of silver, Ag = molar heat capacity*molar mass
= (25.35 J/mol) / (108 g/mol)
= 0.234 J/g------------------2nd answer
Therefore -
The energy required to rise the given temperature,
q = m*s*delta T
= (11.1 g) (0.234 J/g)(14.2 deg C)
= 36.88 J----------------------answer

b.
heat lost by water = heat gained by steel
(m Cp dT) water = (m Cp dT) steel
mass steel = (m Cp dT) water / (Cp dT) steel
mass steel = (120 g) x (4.18 J/gC) x (22.0-21.5 C) / [(0.452 J/gC) x (21.5 - 2.0 C)]

= 28.45 g steel----------------answer
molar heat capacity is J/mole C not J/gC
4.18 J/gC x (18.0 g / mole) = 75.2 J/moleC---------answer

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