The temperature of a 356 g piece of granite is increased from 32.3°C to 55.5°C. What...

The temperature of a 356 g piece of granite is increased from 32.3°C to 55.5°C. What is its change in entropy (J/K)? The specific heat capacity of granite is 0.790 J/g.K.

Expert Solution

queen_honey_blossom answered 2 years ago

A 100 g piece of granite and a 100 g piece of lead are placed in...

A 100 g piece of granite and a 100 g piece of lead are placed in an oven that is at 100°C. The initial temperature of the pieces are 25°C. After a couple of minutes, neither one is at 100°C, but which one is warmer? Which one will reach 100°C first? How much energy will it take for both of the objects to reach 100°C?

A 286.0 g piece of granite, heated to 571.0°C in a campfire, is dropped into 1.15...

A 286.0 g piece of granite, heated to 571.0°C in a campfire, is dropped into 1.15 L water (d = 1.00 g/mL) at 25.0°C. The molar heat capacity of water is cp,water = 75.3 J/(mol ·°C), and the specific heat of granite is cs,granite = 0.790 J/(g ·°C). Calculate the final temperature of the granite in Celcius

A 286.0 g piece of granite, heated to 556.0°C in a campfire, is dropped into 1.50...

A 286.0 g piece of granite, heated to 556.0°C in a campfire, is dropped into 1.50 L water (d = 1.00 g/mL) at 25.0°C. The molar heat capacity of water is cp,water = 75.3 J/(mol ·°C), and the specific heat of granite iscs,granite = 0.790 J/(g ·°C). Calculate the final temperature of the granite.

1. A 5.88 kg piece of granite with a specific heat of 0.803 J g-1 °C-1...

1. A 5.88 kg piece of granite with a specific heat of 0.803 J g-1 °C-1 and a temperature of 85.1 °C is placed into 2.00 L of water at 19.0 °C. When the granite and water come to the same temperature, what will the temperature be? 2. The combustion of methane (the chief component of natural gas) follows the equation: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) ∆H° for this reaction is -802.3 kJ. How many grams of methane...

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 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.

A student heats a piece of 130 g of an unknown greyish metal to a temperature...

A student heats a piece of 130 g of an unknown greyish metal to a temperature of 99.2 celcius. she places the metal in a styrofoam cup that contains 55.7 g of water at a temperature of 23.0 celsius. the hot metal heats up the water in the cup to 31.4 celcius. calculate the specific heat of the metal?

Part A It takes 55.0 J to raise the temperature of an 10.2 g piece of...

Part A It takes 55.0 J to raise the temperature of an 10.2 g piece of unknown metal from 13.0∘C to 25.0 ∘C. What is the specific heat for the metal? Part B The molar heat capacity of silver is 25.35 J/mol⋅∘C. How much energy would it take to raise the temperature of 10.2 g of silver by 15.4 ∘C ? I got 36.9 J for B and its correct Part C What is the specific heat of silver?

Part A It takes 47.0 J to raise the temperature of an 9.50 g piece of...

Part A It takes 47.0 J to raise the temperature of an 9.50 g piece of unknown metal from 13.0∘C to 24.8 ∘C. What is the specific heat for the metal? Express your answer with the appropriate units. Cs= Parts B and C The next two questions pertain to silver. They have nothing to do with unknown metal described in Part A. Part B The molar heat capacity of silver is 25.35 J/mol⋅∘C. How much energy would it take to...

Sulfur (2.56 g) was burned in a constant volume calorimeter with excess O2(g). The temperature increased...

Sulfur (2.56 g) was burned in a constant volume calorimeter with excess O2(g). The temperature increased from 21.25 °C to 26.72 °C. The bomb has a heat capacity of 923 J/K, and the calorimeter contained 815 g of water. Calculate ΔU per mole of SO2 formed for the reaction S8(s) + 8 O2(g) → 8 SO2(g)

Question