All questions of October for NEET Exam

Understanding Vapor Pressure
Vapor pressure is defined as the pressure exerted by a vapor in equilibrium with its liquid or solid phase at a given temperature.
Impact of Temperature on Vapor Pressure
- As temperature increases, the kinetic energy of the molecules in a liquid also increases.
- High-energy molecules are more likely to escape the liquid phase and enter the vapor phase.
Why Vapor Pressure Increases with Temperature
- At higher temperatures, more molecules have enough energy to overcome intermolecular forces that keep them in the liquid state.
- This leads to an increase in the number of molecules in the vapor phase, thus raising the vapor pressure.
Key Points to Remember
- The relationship between temperature and vapor pressure is typically represented by the Clausius-Clapeyron equation.
- This equation illustrates how the vapor pressure of a substance changes with temperature, confirming that vapor pressure is directly proportional to temperature.
Conclusion
In summary, option 'C' is correct: vapor pressure increases with increasing temperature. Understanding this principle is crucial for various applications in chemistry and related fields, including understanding phase changes and designing processes in chemical engineering.

Compounds with branched or straight chains are known as acyclic compounds, also called aliphatic compounds. They do not form closed rings.

Raoult's law describes the relationship between the total vapour pressure of a solution and the mole fraction of its individual components. It provides insight into how the presence of different components affects the overall vapour pressure of a solution.

Function of Glucocorticoids
Glucocorticoids are steroid hormones produced by the adrenal cortex, with cortisol being the most significant in humans. Their primary functions involve metabolism regulation and stress response.
Key Effects of Cortisol
- Gluconeogenesis: Cortisol stimulates the liver to produce glucose from non-carbohydrate sources, which is essential during fasting or stress situations.
- Lipolysis: It promotes the breakdown of fats, releasing fatty acids into the bloodstream for energy utilization.
- Proteolysis: Cortisol enhances the breakdown of proteins into amino acids, which can be used for energy or to produce glucose.
- Immune Suppression: It suppresses the immune response, which is beneficial in managing inflammation and autoimmune conditions but can make the body more susceptible to infections.
Why Other Options Are Incorrect
- Option A: Incorrect because glucocorticoids do not primarily stimulate adipose tissue deposition; instead, they can lead to fat redistribution.
- Option B: Incorrect as cortisol does not primarily reabsorb sodium and water; that function is mainly associated with mineralocorticoids like aldosterone. High cortisol levels can actually lead to increased potassium levels.
- Option D: Incorrect because while the adrenal cortex does produce androgens, cortisol itself does not stimulate their synthesis. Androgens are produced in the zona reticularis of the adrenal cortex, separate from the effects of glucocorticoids.
In summary, cortisol's multifaceted role in metabolism and immune response confirms option 'C' as the correct choice, highlighting its importance in maintaining homeostasis during stress.

Organic compounds are primarily based on the element carbon. Carbon forms the backbone of organic molecules and is typically bonded to other carbon and/or hydrogen atoms.

Understanding Carcinogenic Radiation
Radiation can be classified based on its properties and effects on biological tissues. Among the various types, some are known to possess carcinogenic potential, meaning they can lead to cancer development.
Types of Radiation
- Alpha Particles:
- Composed of two protons and two neutrons, alpha particles are heavy and positively charged.
- While they have low penetration ability (can be stopped by paper or skin), they can cause significant damage to cells if ingested or inhaled.
- Beta Particles:
- These are high-energy, high-speed electrons or positrons emitted by certain types of radioactive nuclei.
- They are more penetrating than alpha particles but less damaging on a per-event basis.
- X-rays:
- A form of electromagnetic radiation with high energy.
- X-rays can penetrate soft tissues and are widely used in medical imaging.
- They can cause DNA damage, which may lead to cancer.
- Neutrons:
- Neutrons are neutral particles that can also cause ionization indirectly through collisions with other nuclei.
- They are highly penetrating and can be quite damaging to biological tissues.
Why Alpha Particles are Carcinogenic
- Direct Damage:
- When alpha-emitting radionuclides are inhaled or ingested, they can cause localized damage in tissues.
- This localized radiation exposure can lead to mutations in DNA, increasing the risk of cancer.
- Biological Impact:
- Alpha particles have a high mass and charge, which means they transfer energy more efficiently to nearby cells, causing more ionizations and potential cellular damage.
In summary, while all forms of radiation have the potential to cause cancer under certain conditions, alpha particles (option C) are particularly noteworthy due to their capacity for causing significant localized damage when they interact with biological tissues, thereby increasing cancer risk.

The anterior pituitary produces Prolactin (PRL), Growth Hormone (GH), and Thyroid Stimulating Hormone (TSH). The hormones not produced by the anterior pituitary from the list are Oxytocin, Vasopressin, Somatostatin, and Gonadotrophin Releasing Hormone (GnRH). These four hormones are either secreted by the hypothalamus or the posterior pituitary. Thus, the total number of hormones not produced by the anterior pituitary in the list is four.

The boiling point of a liquid is defined as the temperature at which the vapour pressure of the liquid equals the pressure exerted by the atmosphere. At this temperature, the liquid changes into the vapour phase.

Understanding Ideal Solutions
In an ideal solution, the interactions between different molecules are similar to those between like molecules. When considering the vapor-liquid equilibrium of an ideal solution, the partial pressures of the components play a significant role.
Key Concepts
- Vapor Pressure: The vapor pressure of a component in a solution depends on its mole fraction in the liquid phase.
- Raoult's Law: For an ideal solution, the partial vapor pressure of component A (pA) is given by pA = PA° * (xA), where PA° is the vapor pressure of pure A and xA is its mole fraction in the liquid.
Relation between Mole Fractions
- Given that pA > pB, it indicates that component A has a higher tendency to vaporize than component B.
- In equilibrium, the mole fraction of A in the liquid phase (xA) will be higher than that of B in the vapor phase (xB).
Analyzing the Options
- Option A: (xA)liquid = (xB)vapour
This is incorrect because the mole fractions in the two phases are not equal.
- Option B: (xA)liquid > (xB)vapour
While this might seem plausible, it does not accurately reflect the relationship given that pA > pB.
- Option C: (xA)liquid < (xb)vapour="" />
This is the correct statement. Since A is more volatile, its concentration in the vapor phase will be greater than its concentration in the liquid phase.
- Option D: (xA)liquid and (xB)vapour do not bear any relationship
This is incorrect as there is a direct relationship established by Raoult's Law.
Conclusion
Therefore, the correct interpretation of the relationship in the context of an ideal solution with pA > pB is that the mole fraction of A in the liquid phase is indeed less than that of B in the vapor phase, leading us to conclude that the answer is option C.

Liquids with weaker intermolecular forces, like acetone, tend to have higher vapour pressure at a particular temperature compared to liquids with stronger intermolecular forces, like water.

Evaporation occurs when the liquid is heated, causing an increase in the kinetic energy of its molecules. This increased energy allows molecules to transition from the liquid phase to the vapour phase, leading to evaporation.

The total vapour pressure above a solution increases linearly with the mole fraction of a component. This relationship is described by Raoult's law, which states that the total vapour pressure depends on the mole fractions of the components present in the solution.

Vapour pressure reaches its maximum value when the rate of evaporation equals the rate of condensation, resulting in a state of equilibrium. This equilibrium point is where the pressure exerted by the vapour is defined as the vapour pressure of the liquid.

Vapour pressure is the pressure exerted by the vapour of a liquid in equilibrium with its condensed phases (solid or liquid) in a closed system at a given temperature. It is a measure of the tendency of liquid molecules to escape into the vapour phase and serves as an indicator of the liquid's evaporation rate.

The standard boiling point of a liquid is defined at a pressure of 1 atmosphere (atm) or 101.325 kPa. It is the temperature at which the vapour pressure of the liquid equals the atmospheric pressure.

The Heat of Vaporization is the amount of heat energy required to transform one mole of a liquid into the gaseous state at its boiling point, while keeping the temperature constant.