Untitled Quiz

<p>Internal pressure of the gas (B)</p> Signup and view all the answers

<p>dw = P × A × dV (C)</p> Signup and view all the answers

<p>Reversible expansion follows a series of intermediate steps. (B)</p> Signup and view all the answers

<p>Work is determined by the type of process (reversible or irreversible). (D)</p> Signup and view all the answers

<p>It is equal in magnitude to the work done during isothermal expansion. (A)</p> Signup and view all the answers

<p>The amount of heat required to raise the temperature of one mole of a substance by one degree. (A)</p> Signup and view all the answers

<p>Heat capacity must specify the process affecting temperature change. (B)</p> Signup and view all the answers

<p>Joules per degree per mole. (C)</p> Signup and view all the answers

<p>The amount of heat required to increase the temperature without performing work. (D)</p> Signup and view all the answers

<p>q = C<del>p</del> (T<del>2</del> - T<del>1</del>) (C)</p> Signup and view all the answers

<p>It increases as absorbed heat equals the change in internal energy. (B)</p> Signup and view all the answers

<p>C<del>p</del> is greater than C<del>v</del> due to work done on expansion. (D)</p> Signup and view all the answers

<p>C<del>p</del> (B)</p> Signup and view all the answers

<p>C_p - C_v = R (B)</p> Signup and view all the answers

<p>q = nC(T_2 - T_1) (B)</p> Signup and view all the answers

<p>18 cal/mol/K (C)</p> Signup and view all the answers

<p>Cooling due to gas expansion from high pressure to low pressure. (D)</p> Signup and view all the answers

<p>750 cals (D)</p> Signup and view all the answers

<p>Restricts the flow of gas during expansion. (A)</p> Signup and view all the answers

<p>To measure the temperature change on gas expansion. (C)</p> Signup and view all the answers

<p>1.987 (C)</p> Signup and view all the answers

<p>The flow of heat and energy into or out of a system (B)</p> Signup and view all the answers

<p>Temperature, pressure, volume, and concentration (C)</p> Signup and view all the answers

<p>First law of thermodynamics (D)</p> Signup and view all the answers

<p>It does not account for microscopic systems of individual atoms or molecules. (D)</p> Signup and view all the answers

<p>The rate of a chemical reaction (C)</p> Signup and view all the answers

<p>They derive all laws of physical chemistry from them. (B)</p> Signup and view all the answers

<p>Zeroth law of thermodynamics (B)</p> Signup and view all the answers

<p>The time factor in processes (D)</p> Signup and view all the answers

<p>It decreases. (D)</p> Signup and view all the answers

<p>No heat exchange occurs between the system and surroundings. (C)</p> Signup and view all the answers

<p>Adiabatic process. (C)</p> Signup and view all the answers

<p>Cp = Cv + R. (A)</p> Signup and view all the answers

<p>It remains constant. (D)</p> Signup and view all the answers

<p>1.67 (A)</p> Signup and view all the answers

<p>In isothermal processes, temperature remains constant, while in adiabatic processes, it changes. (D)</p> Signup and view all the answers

<p>ΔE = w (A)</p> Signup and view all the answers

<p>Difference in enthalpy of reactants and products (D)</p> Signup and view all the answers

<p>Reactions involving solids and liquids only (C)</p> Signup and view all the answers

<p>When the enthalpies of reactants and products are equal (A)</p> Signup and view all the answers

<p>Exothermic reaction (D)</p> Signup and view all the answers

<p>It is significant when reactions occur at constant pressure (B)</p> Signup and view all the answers

<p>ΔH &gt; 0 (D)</p> Signup and view all the answers

<p>ΔH = (H<del>C</del> + H<del>D</del>) - (H<del>A</del> + H<del>B</del>) (B)</p> Signup and view all the answers

<p>They describe the heat exchange with the surroundings (C)</p> Signup and view all the answers

The study of energy flow (heat or other forms) into or out of a system during physical or chemical changes.

A specific part of the universe being studied, separated from the surroundings.

Everything outside the system that can interact with it.

Defined by its properties like temperature, pressure, volume, and concentration.

Transition of a system from one state to another, involving changes in its properties.

The total energy of an isolated system remains constant; energy cannot be created or destroyed, only transferred or transformed.

A system containing a large number of particles, treated as bulk matter.

A system consisting of individual atoms or molecules, often studied in detail.

The work done by a system refers to the energy transferred from the system to its surroundings during a process. This energy transfer can occur through various mechanisms, such as expansion against external pressure.

A state function is a property that depends only on the current state of the system, not on how the system reached that state. Examples include internal energy, enthalpy, and entropy.

Unlike state functions, work is a process function. This means the work done by a system depends on the specific path or process taken to reach a final state.

Reversible expansion is a process where the system is always in equilibrium with its surroundings. In a reversible process, the system can be brought back to its original state by reversing the process. This is a theoretical ideal.

Irreversible expansion occurs when the system is not in equilibrium with its surroundings. In this case, the process cannot be reversed to return the system to its original state.

PV work, or pressure-volume work, is the work done by a system during expansion or contraction. It's calculated by the change in volume multiplied by the external pressure.

An isothermal process is one that occurs at a constant temperature. During an isothermal process, heat flow into or out of the system occurs to maintain constant temperature.

The work done during an isothermal reversible expansion of an ideal gas is calculated using the formula: W = -nRT ln(V2/V1). This formula accounts for the change in volume and the constant temperature.

The amount of heat energy required to raise the temperature of a substance by one degree Celsius or Kelvin.

The amount of heat energy required to raise the temperature of one mole of a substance by one degree Celsius or Kelvin.

The heat capacity of a system when the volume is held constant during the temperature change.

The heat capacity of a system when the pressure is held constant during the temperature change.

Because at constant pressure, some of the heat absorbed is used to do work by expanding the system, while at constant volume, all the heat goes into increasing internal energy.

The amount of heat absorbed (and thus the heat capacity) depends on the specific path taken to change the system's temperature, not just the initial and final states.

At constant volume, the heat absorbed (qv) is equal to the change in internal energy (ΔU). This is because no work is done when volume is constant.

qp = Cp * (T2 - T1), where qp is the heat absorbed at constant pressure, Cp is the molar heat capacity at constant pressure, and T2 and T1 are the final and initial temperatures, respectively.

The change in enthalpy of a system, denoted by dH, represents the heat absorbed or released at constant pressure.

For ideal gases, enthalpy (H) can be calculated as the sum of internal energy (E) and the product of pressure (P) and volume (V): H = E + PV.

For ideal gases, the difference between molar heat capacity at constant pressure (Cp) and constant volume (Cv) is equal to the gas constant (R): Cp - Cv = R.

The phenomenon of cooling that occurs when a gas expands adiabatically from a region of high pressure to a region of low pressure.

An experiment devised by Joule and Thomson to measure the temperature change during the adiabatic expansion of a gas.

Derivatives that are calculated when one or more variables are held constant during the change of another.

The difference in enthalpy (ΔH) between products and reactants when a reaction occurs at constant pressure.

The change in internal energy (ΔE) of the system when the reaction occurs at constant volume.

A reaction that releases heat into the surroundings, making the enthalpy of products less than reactants (ΔH < 0).

A reaction that absorbs heat from the surroundings, making the enthalpy of products greater than reactants (ΔH > 0).

The total heat content of a system at constant pressure.

The change in enthalpy (ΔH) is calculated by subtracting the enthalpy of reactants from the enthalpy of products.

No heat is evolved or absorbed in the reaction. The enthalpies of products and reactants are equal.

The change in volume (ΔV) is minimal for reactions involving only solids and liquids. Therefore, the term PΔV, which represents work done against pressure, becomes negligible.

A thermodynamic process where no heat exchange occurs between the system and its surroundings.

The change in internal energy (∆E) is equal to the negative of the work done (w) by the system, as there is no heat transfer (q=0).

The work done by the system during expansion is at the expense of its internal energy, leading to a decrease in temperature.

The temperature below which an ideal gas cools during an adiabatic expansion and above which it heats up.

The relationship between pressure (P) and volume (V) during adiabatic expansion is PV^γ = constant, where γ is the adiabatic index.

The ratio of specific heat capacity at constant pressure (Cp) to specific heat capacity at constant volume (Cv).

In adiabatic expansion, temperature changes due to no heat exchange, while in isothermal expansion, temperature remains constant as heat is exchanged to compensate for work done.

Boyle's law (PV=constant) describes isothermal expansion where temperature is constant, while adiabatic expansion (PV^γ=constant) involves temperature change.