Answer:
d. 37 °C
Explanation:
= mass of lump of metal = 250 g
= specific heat of lump of metal = 0.25 cal/g°C
= Initial temperature of lump of metal = 70 °C
= mass of water = 75 g
= specific heat of water = 1 cal/g°C
= Initial temperature of water = 20 °C
= mass of calorimeter = 500 g
= specific heat of calorimeter = 0.10 cal/g°C
= Initial temperature of calorimeter = 20 °C
= Final equilibrium temperature
Using conservation of heat
Heat lost by lump of metal = heat gained by water + heat gained by calorimeter
Given:
The initial volume of the gas, V₁=3200 ml=3.2×10⁻³ m³
The initial pressure of the gas, P₁=122 kPa
The initial temperature of the gas, T₁=27 °C=300 K
The final temperature, T₂=65 °C=338 K
The final pressure, P₂=112 kPa
To find:
The final volume of xenon gas.
Explanation:
From the combined gas law,
Where V₂ is the volume after it is heated.
On rearranging the above equation,
On substituting the known values,
Final answer:
The volume of the balloon when it is heated is 3.61 m³