Question

In: Chemistry

1. A 30 g piece of metal (160.9 g/mol) melts at 1,560°C and its enthalpy of...

1. A 30 g piece of metal (160.9 g/mol) melts at 1,560°C and its enthalpy of fusion is 12.6 kJ/mol. Calculate the entropy of fusion (J/k) per mole of the metal.

2. The temperature of a 374 g piece of granite is increased from 38.4°C to 62.6°C. What is its change in entropy (J/K)? The specific heat capacity of granite is 0.790 J/g.K.

Solutions

Expert Solution

queen_honey_blossom answered 7 months ago
Next > < Previous

Related Solutions

Ethanol melts at -114.0 ∘C. The enthalpy of fusion is 5.02 kJ/mol and the enthalpy of...
Ethanol melts at -114.0 ∘C. The enthalpy of fusion is 5.02 kJ/mol and the enthalpy of vaporization is 38.6 kJ/mol. The specific heats of solid and liquid ethanol are 0.970 J/g⋅K and 2.30 J/g⋅K, respectively. How much heat is needed to convert 39.0 g of solid ethanol at -160.0 ∘C to liquid ethanol at -35.0 ∘C ? I am really confused on this, any help would be greatly appreciated. Thanks!
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of...
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 J/g⋅K are 2.3 J/g⋅Krespectively. 1. How much heat is required to convert 48.5 g of ethanol at 40 ∘C to the vapor phase at 78 ∘C? Express your answer using two significant figures. 2. How much heat is required to convert 48.5...
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of...
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 J/g⋅K are 2.3 J/g⋅Krespectively. How much heat is required to convert 48.0 g of ethanol at -157 ∘C to the vapor phase at 78 ∘C?
Ethanol (C2H5OHC2H5OH) melts at -114 ∘C∘C and boils at 78 ∘C∘C. The enthalpy of fusion of...
Ethanol (C2H5OHC2H5OH) melts at -114 ∘C∘C and boils at 78 ∘C∘C. The enthalpy of fusion of ethanol is 5.02 kJ/molkJ/mol, and its enthalpy of vaporization is 38.56 kJ/molkJ/mol. The specific heat of solid and liquid ethanol are 0.97 J/g⋅KJ/g⋅K are 2.3 J/g⋅KJ/g⋅K respectively. Part A Part complete How much heat is required to convert 41.5 gg of ethanol at 21 ∘C∘C to the vapor phase at 78 ∘C∘C? Express your answer using two significant figures. QQ = 40 kJkJ SubmitPrevious...
Ethanol (C2H5OH) melts at -114 degrees C and boils at 78 degrees C. The enthalpy of...
Ethanol (C2H5OH) melts at -114 degrees C and boils at 78 degrees C. The enthalpy of fusion of ehtinal is 5.02 kj/mol, and its enthalpy of vaporization is 38.56 kj/mol. The specific heat of solid nd liquid ethanol are 0.97 and 2.3 J/g-K, repectively. (A) How much heat is required to convert 42.0 g of ethanol at 35 degrees C to the vapor phase at 78 degrees C? (B) How much heat i required to convert the same amount of...
The molar enthalpy of benzene at its normal boiling point (80.09° C) is 30.72 kJ/mol. Assuming...
The molar enthalpy of benzene at its normal boiling point (80.09° C) is 30.72 kJ/mol. Assuming that Δ H of vaporization and Δ S of vaporization stay constant at their values at 80.09° C, calculate the value of ΔG of vaporization at 75.0° C, 80.09° C, and 85.0° C. Interpret these results physically.
A 29.60 g piece of iron and a 28.00 g piece of gold at 100.0 C...
A 29.60 g piece of iron and a 28.00 g piece of gold at 100.0 C were dropped into 880.0mL of water at 17.60 C. The molar heat capacities of iron and gold are 25.19 J/(mol*C) and 25.42 J/(mol*C), respectively. What is the final temperature of the water and pieces of metal?
A 25 g piece of metal is dropped into 100.0 g sample of water. The water...
A 25 g piece of metal is dropped into 100.0 g sample of water. The water temperature drops by 5.0 C. The piece of metal's temperature increases by 85 C. What is the specific heat of this piece of metal? (The specific heat of water is 4.18 J/gC)
A 28.8 g piece of iron and a 27.6 g piece of gold at 100.0°C were...
A 28.8 g piece of iron and a 27.6 g piece of gold at 100.0°C were dropped into 660.0 mL of water at 16.0°C. The molar heat capacities of iron and gold are 25.19 J/(mol·°C) and 25.41 J/(mol·°C), respectively.
When a certain liquid (MM = 49.9 g mol-1) freezes at -8.51°C and 1 atm, its...
When a certain liquid (MM = 49.9 g mol-1) freezes at -8.51°C and 1 atm, its density changes from 0.787 g cm-3 to 0.808 g cm-3. Its enthalpy of fusion is 6.27 kJ mol-1. Find the freezing point of the liquid in °C at 52 MPa.
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT