How can you determine the specific heat of a metal using a calorimeter?

How can you determine the specific heat of a metal using a calorimeter?

Place the metal piece into the water of the calorimeter and measure the highest temperature reached by the water. This is the final temperature of both the metal and the water. The energy change of water is calculated by rearranging the specific heat equation. The specific heat of water is 1.00 calorie/gram°C.

How do you find the specific heat capacity of water experiment?

Method

1. Place one litre (1 kg) of water in the calorimeter.
2. Place the immersion heater into the central hole at the top of the calorimeter.
3. Clamp the thermometer into the smaller hole with the stirrer next to it.
4. Fully insulate the calorimeter by wrapping it loosely with cotton wool.
5. Record the temperature of the water.

What’s the equation for specific latent heat?

The specific latent heat (L) of a material… is a measure of the heat energy (Q) per mass (m) released or absorbed during a phase change. is defined through the formula Q = mL. is often just called the “latent heat” of the material.

What’s the specific heat capacity of water?

The SI unit of specific heat is joule per kelvin and kilogram, J·kg−1·K−1. For example, the heat required to raise the temperature of 1 kg of water by 1 K is 4179. 6 joules so the specific heat capacity of water is 4179.

What is Gamma in ideal gas?

It is sometimes also known as the isentropic expansion factor and is denoted by γ (gamma) for an ideal gas or κ (kappa), the isentropic exponent for a real gas. the molar heat capacity (heat capacity per mole), and c the specific heat capacity (heat capacity per unit mass) of a gas.

How does specific heat of gas vary from 0 to infinity?

Yes, the specific heat of gas will be infinity. Increase in the temperature of gas is zero, for an isothermal process.

What is Delta U in adiabatic process?

According to the definition of an adiabatic process, ΔU=wad. Therefore, ΔU = -96.7 J. Calculate the final temperature, the work done, and the change in internal energy when 0.0400 moles of CO at 25.0oC undergoes a reversible adiabatic expansion from 200. L to 800.

What is Q for an isothermal expansion?

It is also worth noting that for ideal gases, if the temperature is held constant, the internal energy of the system also is constant, and so ΔU = 0. Since the First Law of Thermodynamics states that ΔU = Q + W (IUPAC convention), it follows that Q = −W for the isothermal compression or expansion of ideal gases.

What is non quasi-static process?

In a quasi-static process, the path of the process between A and B can be drawn in a state diagram since all the states that the system goes through are known. In a non-quasi-static process, the states between A and B are not known, and hence no path can be drawn.