Chemistry Section 7

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• The state of matter with the lowest density is gas.
• Solid particles only possess vibrational motion.
• Plotting 1/V on the X-axis and pressure on the Y-axis results in a straight line.
• One mole of an ideal gas at 546.5 K and 2 atm pressure has a volume of 22.414 dm3.
• None of these options represent the partial pressure of oxygen in the lungs.
• The kinetic molecular theory of gases was proposed by Bernoulli.
• Hydrogen effuses four times more rapidly than an unknown gas with a molar mass of 32 gmol-1.
• The processes of effusion and diffusion are best understood through Graham’s law.
• Non-ideal behavior results mainly from intermolecular attractions and finite volume.
• Linds method is employed for the liquefaction of gases.
• Nitric oxide (NO) diffuses more quickly than oxygen.
• Vander Waals force is the weakest intermolecular force among the given options.
• Plasma may be the first state of matter, is a conductor of electricity, and is not a phase transition.
• 5 mole of nitrogen gas and 0.5 mole of carbon monoxide gas at STP have the same mass and number of atoms.
• All gases cannot be liquefied through Linds Method, and not all molecules move with the same speed.
• Matter exists in four forms: solid, liquid, gas, and plasma.
• The most abundant form of matter on Earth is solid.
• When pressure is increased from 2 atm to 6 atm at constant temperature, the volume of a gas should be 1/3 dm3.
• The correct value for the gas constant (R) is 0.0821 atm dm3k-1mol-1.
• The spreading of fragrance or scent in air is due to diffusion.
• The highest temperature at which a substance can exist as a liquid is its critical temperature.
• The process of sudden expansion of plasma is called the Joule-Thomson effect.
• The pressure of 1 mole of an ideal gas at 300 K and 250 cm3 volume is 98.5 atm.
• Vander Waals made volume and pressure corrections to explain deviations of gases from ideal behavior.
• Gases become non-ideal at low temperature and high pressure.
• The pH of 10^-3 mol dm^-3 of an aqueous solution of H2SO4 is 2.7.
• Adding a weak acid and its salt with a strong base creates a basic buffer solution.
• The solubility of AgCl dissolved with conc (2×10^-2) Ksp will be 4 x 10^-4.
• Decreasing the pressure causes the reaction to shift towards the direction where volume increases.
• The abundant form of ozone in the atmosphere is O2.
• Solution having the property of a very little change in pH on adding a small amount of strong acid or base is a buffer solution.
• Ka < 10^-3 indicates a very weak acid.
• Kc and Kp have the same value for the reaction N2 + O2 = 2NO.
• Na2CO3 is an example of a basic aqueous solution.
• The condition for the formation of smog does not include winds.
• Ozone hole occurs during the months of September to November.
• The main product of bacterial action is NO.
• The pH of a buffer solution made from an equimolar mixture of sodium benzoate and benzoic acid with pKa of 2 is 2.
• Equilibrium state is dynamic in nature.
• Rate expression for ammonia synthesis is Kc = 4x^2v^2 / (a-x)(b-3x)^3.
• Addition of a catalyst achieves equilibrium quickly.
• The common ion effect is the substantial depletion of ozone.
• pH and pOH were introduced by Sorenson.
• Ka < 10^-3 indicates a very weak acid.
• Homogeneous mixtures of compounds are called solutions.
• The solution with the maximum concentration of solute at a given temperature is called a saturated solution.
• The number of moles in 1 kg of solvent is molality.
• Azeotropic mixtures are mixtures which distill over without a change in composition.
• The solution of KClO3 has a continuous and rising solubility curve.
• Adding common salt to water increases its boiling point.
• Kc and Kp have the same value in the equilibrium: N2 + O2 = 2NO.
• Not a base: Option D. BF3.
• Buffer formed by: 0.4 mole of NH3 with 0.2 mole of HCI.
• Chemical equilibrium is a dynamic state.
• At the start of the reaction, reactant concentration is high.
• In the case of gases, Kc is replaced by Kp.
• When Kc is very small, product concentration is maximum.
• Idea of pH and pOH by: Option C. Sorenson.
• Ka<10^-3 means: Very weak acid.
• Macronutrient: Option D. carbon.
• Healthy plant growth needs: N P K.
• Residence time of methane in atmosphere: 3 – 7 years.
• Hypochlorous acid disinfects water, producing: all of the above.
• Acid in acid rain: both A and B.
• Smog formation doesn’t require: winds.
• Thickest ozone layer in: stratosphere.
• Ozone layer most affected by: A. CFC.
• Incorrect statement: the amount of ozone layer is greater in the region close to the equator.
• Coagulant in water purification: alum.
• Newspaper can be recycled 5 times.
• Main pollutant in leather tanneries: chromium IV.
• Water disinfectant: KMnO4.
• Bulk of hydrosphere content: oceans.
• Suspended solid waste removed by coagulation: 80%.
• Main product of bacterial action: NO.
• Pollutants adversely affect: Ecosystem.
• Not a heavy industry: paper.
• Macronutrient requirement per acre: 5 to 200 kg.
• Secondary pollutant: carbon dioxide.
• Major cause of SO2 on a global scale: volcanoes.
• Yellow color in photochemical smog due to: nitrogen dioxide.
• Not a primary pollutant: H2SO4.
• Main cause of acid rain: NO2.
• Measures water quality: all of the above.
• One chlorine free radical destroys: 100000 ozone molecules.
• Chlorination harmful if water contains: Ammonia.
• Disinfectants to avoid toxic compounds: both B & C.
• Ozone hole depletion: Sep – Nov.
• Most concentrated solution of H2SO4: 1 Molar solution.
• Liquid in gas solution example: Fog.
• Conditions for colligative properties: All of the above.
• Common salt dissolved in water: Boiling point of water increases.
• Homogeneous mixture of compounds: solution.
• Maximum solute concentration: saturated solution.
• Moles in 1 kg of solvent: molality.
• Partially miscible liquids form: saturated solutions of each liquid.
• Relative lowering of vapor pressure: both B & C.
• Distills over without composition change: azeotropic mixture.
• Solubility of KCIO3: continuous and rising solubility curve.
• Boiling point elevations measured by: Landsbergers method.