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The cooling in refrigerator is due to
The cooling effect in a refrigerator is primarily due to the expansion of the refrigerant gas. When the gas expands, it absorbs heat from the refrigerator's interior, thereby cooling it.
The process, in which no heat enters or leaves the system, is termed as
An adiabatic process is a process in which no heat is transferred to or from the system. This means that during such a process, the total heat content of the system remains constant. This is in contrast to other types of processes like isochoric (constant volume), isobaric (constant pressure), and isothermal (constant temperature), where heat exchange can occur.
Warming ammonium chloride with sodium hydroxide in a test tube is an example of :
Warming ammonium chloride with sodium hydroxide in a test tube is an example of an open system. In an open system, both matter and energy can be exchanged with the surroundings. In this case, gases like ammonia may escape from the test tube, indicating the exchange of matter with the surroundings.
Out of boiling point (I), entropy (II), pH (III) and e.m.f. of a cell (IV), intensive properties are –
Intensive properties are those properties that do not depend on the amount of substance present. Out of the given options, boiling point (I), pH (III), and e.m.f. of a cell (IV) are intensive properties. Entropy (II), on the other hand, is an extensive property, as it depends on the amount of substance in the system.
A thermodynamic state function is
A thermodynamic state function is a quantity whose value depends only on the state of the system, not on how the system got to that state. Examples include internal energy, enthalpy, and entropy. This means that the value of a state function is determined solely by the current state of the system, irrespective of the path taken to reach that state.
In thermodynamics, a process is called reversible when
In thermodynamics, a process is called reversible when the surroundings are always in equilibrium with the system. This implies that the process can be reversed without leaving any change in either the system or the surroundings. In other words, the system and surroundings can be returned to their initial states with no net change.
Which one of the following statement is false–
Work is not a state function. Work depends on the path taken to reach one state from another, not just the initial and final states. Therefore, it is path-dependent. On the other hand, state functions like temperature, pressure, and volume depend only on the state of the system and not on how that state was achieved.
A mixture of two moles of carbon monoxide and one mole of oxygen, in a closed vessel is ignited to convert the carbon monoxide to carbon dioxide. If OH is the enthalpy change and OE is the change in internal energy, then
In an exothermic reaction like the combustion of carbon monoxide to carbon dioxide, the enthalpy change (ΔH) is typically greater than the change in internal energy (ΔE). This is because ΔH accounts for the heat released to the surroundings at constant pressure, which includes the work done by the system due to volume change. The relationship can be expressed as ΔH = ΔE + PΔV, where PΔV is the work done by the system. Since gases are involved, PΔV is positive, making ΔH greater than ΔE.
At constant T and P, which one of the following statements is correct for the reaction, $ CO_{(g)} + { 1 \over 2 } O_{2(g) } \rightarrow CO_{2(g) } $
For the reaction $CO_{(g)} + {1 ackslash 2} O_{2(g)} ightarrow CO_{2(g)}$, the enthalpy change (ΔH) is greater than the change in internal energy (ΔE) because the reaction involves a change in the number of moles of gas. At constant temperature and pressure, the enthalpy change includes the pressure-volume work done by the system, making ΔH larger than ΔE.
If $ \triangle H $ is the change in enthalpy and the changes in internal energy accompanying a gaseous reaction
The change in enthalpy (ΔH) can be less than the change in internal energy (ΔE) if the number of moles of the products is less than the number of moles of the reactants. This is because ΔH = ΔE + PΔV, and if the volume decreases (fewer moles of gas), then PΔV is negative, making ΔH less than ΔE.
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