{"id":17604,"date":"2022-05-24T07:30:22","date_gmt":"2022-05-24T02:00:22","guid":{"rendered":"https:\/\/mcq-questions.com\/?p=17604"},"modified":"2022-05-16T15:23:36","modified_gmt":"2022-05-16T09:53:36","slug":"mcq-questions-for-class-11-chemistry-chapter-9","status":"publish","type":"post","link":"https:\/\/mcq-questions.com\/mcq-questions-for-class-11-chemistry-chapter-9\/","title":{"rendered":"MCQ Questions for Class 11 Chemistry Chapter 9 Hydrogen with Answers"},"content":{"rendered":"

Students are advised to practice the\u00a0NCERT MCQ Questions for Class 11 Chemistry Chapter 9 Hydrogen with Answers Pdf free download is available here. MCQ Questions for Class 11 Chemistry with Answers<\/a> are prepared as per the Latest Exam Pattern. Students can solve these Hydrogen Class 11 MCQs Questions with Answers and assess their preparation level.<\/p>\n

Hydrogen Class 11 MCQs Questions with Answers<\/h2>\n

Solving the Hydrogen Multiple Choice Questions of Class 11 Chemistry Chapter 9 MCQ can be of extreme help as you will be aware of all the concepts. These MCQ Questions on Hydrogen Class 11 with answers pave for a quick revision of the Chapter thereby helping you to enhance subject knowledge. Have a glance at the MCQ of Chapter 9 Chemistry Class 11 and cross-check your answers during preparation.<\/p>\n

Question 1.
\nWhen water is dropped over sodium peroxide, the colourless gas produced is:
\n(a) DiNitrogen
\n(b) DiOxygen
\n(c) DiHydrogen
\n(d) Hydrogen Peroxide<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) DiOxygen
\nExplanation:
\nWhen sodium peroxide dissolves in water:
\n2Na2<\/sub>O2<\/sub> + 2H2<\/sub>O \u2192 4NaOH + O2<\/sub><\/p>\n<\/details>\n

\n

Question 2.
\nThe atomic weights of isotopes of all element are different due to different number of __________.
\n(a) Protons
\n(b) Electrons
\n(c) Neutrons
\n(d) None of Above<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) Neutrons
\nExplanation:
\nIsotopes are variants of a particular chemical element which differ in neutron number, and consequently in nucleon number. All isotopes of a given element have the same number of protons but different numbers of neutrons in each atom.<\/p>\n<\/details>\n

\n

Question 3.
\nDuring the reaction of natural gas and steam the catalyst used is
\n(a) Fe
\n(b) Zn
\n(c) Ni
\n(d) Cr<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) Ni
\nExplanation:
\nSteam reforming of natural gas is the most common method of producing commercial bulk hydrogen at about 95% of the world production of 500 billion m3 in 1998, or 70 million tonnes by 2018.Hydrogen is used in the industrial synthesis of ammonia and other chemicals. At high temperatures (700 \u2013 1100\u00b0C) and in the presence of a metal-based catalyst (nickel), steam reacts with methane to yield carbon monoxide and hydrogen.
\nCH4<\/sub> + H2<\/sub>O \u21cc CO + 3 H2<\/sub><\/p>\n<\/details>\n

\n

Question 4.
\nCavendish in 766 discovered.
\n(a) Nitrogen
\n(b) Oxygen
\n(c) Hydrogen
\n(d) Helium<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) Hydrogen
\nExplanation:
\nHenry Cavendish FRS was an English natural philosopher, scientist, and an important experimental and theoretical chemist and physicist. He is noted for his discovery of hydrogen, which he termed “inflammable air”. He described the density of inflammable air, which formed water on combustion, in a 1766 paper, On Factitious Airs. Antoine Lavoisier later reproduced Cavendishs experiment and gave the element its name.<\/p>\n<\/details>\n

\n

Question 5.
\nDihydrogen gas may be prepared by heating caustic soda on
\n(a) Cu
\n(b) Zn
\n(c) Na
\n(d) Ag<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) Zn
\nExplanation:
\nWhen a base reacts with a metal salt in hydrogen gas is formed. In this reaction metal is zinc & base is Sodium hydroxide. When sodium hydroxide solution is heated with zinc granules then Sodium zincate and hydrogen gas are formed.
\n2NaOH (aq) + Zn(s) \u2192 Na2<\/sub>ZnO2<\/sub> (aq)+ H2<\/sub>(g)
\nThe salt formed by the reaction between a base and a metal, the metal is present as a part of the Negative ion. In the sodium zincate salt (Na2<\/sub>ZnO2<\/sub>) formed by the reaction between Sodium Hydroxide and Zinc metal, the zinc metal is present at a part of a negative ions , zincate ion (ZnO2<\/sub>-2<\/sup> ) All the metals do not react with bases to form salt and hydrogen gas. The main product formed in this reaction is sodium zincate (Na2<\/sub>ZnO2<\/sub>)<\/p>\n<\/details>\n

\n

Question 6.
\nHydrogen set free at the time of its preparation from its compound in atomic form are called _________.
\n(a) Nascent Molecular Hydrogen
\n(b) Nascent Atomic Hydride
\n(c) Both (1) and (2)
\n(d) Nascent Hydrogen<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) Nascent Molecular Hydrogen
\nExplanation:
\nThe hydrogen set free at the time of its preparation from its compounds is also in atom from and is commonly known nascent hydrogen. The newly born hydrogen is in atomic form that is why it is called nascent hydrogen.<\/p>\n<\/details>\n

\n

Question 7.
\nWhich substance does not speed up decomposition of H2<\/sub>O2<\/sub>
\n(a) Glycerol
\n(b) Pt
\n(c) Gold
\n(d) MnO2<\/sub><\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) Pt
\nExplanation:
\nGlycerol, phosphoric acid or acetanilide is added to H2<\/sub>O2<\/sub> to check its decomposition.<\/p>\n<\/details>\n

\n

Question 8.
\nWater shows anomalous behavior between
\n(a) 0 to 4 \u00b0C
\n(b) 0 to 5 \u00b0C
\n(c) 0 to -4 \u00b0C
\n(d) 4 to 0 \u00b0C<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) 0 to 4 \u00b0C
\nExplanation:
\nWater show a wide range of anomalies compared to similar liquids or hydrides of other group 16 elements. One of the most talked-about anomalies is the formation of ice from liquid water and how the density changes when we cool the water.<\/p>\n

O is a small atom and highly electronegative compared to Hydrogen. So O attracts the covalent clouds of O-H towards itself, thus making water a polar molecule. The hydrogen bonding in water molecules causes high boiling point and liquid state compared to other hydrides of group 16.<\/p>\n

When we cool water from higher temperature, the density steadily decreases. At 4 degree C it is the highest. But below 4 degree C, The H-bonds break between the molecules and the molecules get drifted further apart, the volume increases and density decreases. The crystalline form of water is ice. At atmospheric pressure ice crystallises in the hexagonal form, but at very low temperatures it condenses to cubic form leaving gap between the structures, thus increasing the volume again.<\/p>\n

Density of ice is less than that of water. Therefore, an ice cube floats on water. In winter season ice formed on the surface of a lake provides thermal insulation which ensures the survival of the aquatic life.<\/p>\n<\/details>\n

\n

Question 9.
\nWhich of the following pair of substance will not evolve H2<\/sub> gas
\n(a) Iron and aqueous H2<\/sub>SO4<\/sub>
\n(b) Copper and HCl(aq)
\n(c) Sodium and Ethanol
\n(d) Iron and Steam<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) Copper and HCl(aq)
\nExplanation:
\nCopper is a noble metal. As it lies below hydrogen in the electrochemical series. Therefore it cant displace hydrogen from dilute HCl. While iron and sodium lie above hydrogen in the electrochemical series. so they can liberate H2<\/sub> either from steam or H2<\/sub>SO4<\/sub> solution.
\nFe + H2SO4<\/sub> \u2194 FeSO4<\/sub> + H2<\/sub>
\n3Fe + 4H2<\/sub>O (steam) \u2194 Fe3<\/sub>O4<\/sub> + 4H2<\/sub>
\nCu + HCl(g) \u2192 No reaction
\n2Na + 2C2<\/sub>H5<\/sub>OH \u2192 2C2<\/sub>H5<\/sub>ONa + H2<\/sub><\/p>\n<\/details>\n

\n

Question 10.
\nTritium __________ radio active isotope.
\n(a) Beta-Emitting
\n(b) Alpha \u2013 Emitting
\n(c) Gamma-Emitting
\n(d) None of the Above<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) Beta-Emitting
\nExplanation:
\nTritium is a beta-emitting radioactive isotope of hydrogen. Its nucleus consists of one proton and two neutrons, making it three times as heavy as a hydrogen nucleus (with its one proton) and one-and-a-half times as heavy as deuterium (which contains one proton and only one neutron).<\/p>\n<\/details>\n

\n

Question 11.
\nThe maximum density of water at 40C is :
\n(a) 1.0 g \/ cm\u00b3
\n(b) 0.998 g \/ cm\u00b3
\n(c) 0.918 g \/ cm\u00b3
\n(d) 1.2 g \/ dm\u00b3<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) 1.0 g \/ cm\u00b3
\nExplanation:
\nWater never has an absolute density because its density varies with temperature. Water has its maximum density of 1 g\/cm\u00b3 at 4 degrees Celsius. When the temperature changes from either greater or less than 4 degrees, the density will become less then 1 g\/cm\u00b3. Water has the maximum density of 1 g\/cm\u00b3 only when it is pure water. Other factors affect waters density such as whether it is tap or fresh water or salt water. These variations of water changes its density because whats in the water has its own density.<\/p>\n<\/details>\n

\n

Question 12.
\nWater gas is mixture of hydrogen H2<\/sub> and
\n(a) CO
\n(b) CO2<\/sub>
\n(c) Cl2<\/sub>
\n(d) SO2<\/sub><\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) CO
\nExplanation:
\nWater gas is a combustion fuel containing carbon monoxide (CO) and hydrogen gas (H2<\/sub>). Water gas is made by passing steam over heated hydrocarbons.<\/p>\n<\/details>\n

\n

Question 13.
\nThe volume of oxygen gas evolved at STP by decomposition of 0.68 g \u201c20 volume\u201d hydrogen peroxide is:
\n(a) 112 ml
\n(b) 224 ml
\n(c) 56 ml
\n(d) 336 ml<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) 224 ml
\nExplanation:
\n2H2<\/sub>O2<\/sub> \u2192 2H2<\/sub>O + O2<\/sub>
\n2 \u00d7 34 g = 22400 ml
\nAs 2 \u00d7 34 g = 68 g of H2<\/sub>O2<\/sub> liberates
\n22400 ml O2<\/sub> at STP
\nTherefore, 0.68 g of H2<\/sub>O2<\/sub> liberates
\n= (0.68 \u00d7 22400)\/(68) = 224 ml<\/p>\n<\/details>\n

\n

Question 14.
\nWhich of the following statements regarding hydrogen peroxide is\/are incorrect?
\n(a) As aerating agent in production of sponge rubber
\n(b) As an antichlor
\n(c) For restoring white colour of blackened lead painting
\n(d) All of the above<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) All of the above
\nExplanation:
\nH2<\/sub>O2<\/sub> show all these properties<\/p>\n<\/details>\n

\n

Question 15.
\n_______ on water decolourises H2<\/sub>O2<\/sub>
\n(a) O3<\/sub>
\n(b) Acidic KMnO4<\/sub> solution
\n(c) Black Suspension of Lead Sulphide( PbS)
\n(d) None of these<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) Black Suspension of Lead Sulphide(PbS)
\nExplanation:
\nLead sulphide (black suspension) on reaction with hydrogen peroxide forms lead sulphate and water. Lead sulphate as well as water are colourless, therefore lead sulphite decolourises on addition of hydrogen peroxide.
\nPbS(s) + 4H2<\/sub>O2<\/sub> (aq) \u2192 PbSO4<\/sub> (s) + 4H2<\/sub>O (aq)<\/p>\n<\/details>\n

\n

Question 16.
\nThe number of electron hydrogen contains in its K shell is
\n(a) 1
\n(b) 2
\n(c) 3
\n(d) 4<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) 1
\nExplanation:
\nThe maximum number of electrons present in a shell is given by the formula 2n\u00b2, where \u201cn\u201d is the orbit number or energy level index, 1, 2, 3 , \u2026… Hence the maximum number of electrons in different shells are as follows:
\nFirst orbit or K-shell will be = 2 \u00d7 12 = 2
\nHydrogen (H), lithium (Li), and sodium (Na), all have one electron in their outermost shells. This means that they can achieve a stable configuration and a filled outer shell by donating or losing an electron.<\/p>\n<\/details>\n

\n

Question 17.
\nOn shaking H2<\/sub>O2<\/sub> with acidified potassium dichromate and ether, ethereal layer becomes:
\n(a) Green
\n(b) Red
\n(c) Blue
\n(d) Brown<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) Blue
\nExplanation:
\nThis is due to the formation of CrO5
\nK2<\/sub>Cr2<\/sub>O7<\/sub> + H2<\/sub>SO4<\/sub> + 4H2<\/sub>O2<\/sub> \u2192 K2<\/sub>SO4<\/sub> + 2CrO5<\/sub> + 5H2<\/sub>O
\nSo it is Blue<\/p>\n<\/details>\n

\n

Question 18.
\nHydrogen atom contains one electron. But, the spectrum of hydrogen contains number of lines.
\n(a) Single
\n(b) Multiple
\n(c) Cannot be determined
\n(d) None of the Above<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) Multiple
\nExplanation:
\nIn a sample of hydrogen gas, the number of hydrogen molecules is present. These molecules dissociate and produce hydrogen atoms when heated. Each hydrogen atom contains one electron. The hydrogen atoms absorb different amounts of energy and go to different excited states. From there, they take different paths and come back to ground state. Since different paths are associated with different energies, different spectral lines are formed in the spectrum.<\/p>\n<\/details>\n

\n

Question 19.
\nH2<\/sub>O2<\/sub> used in rocket has the concentration:
\n(a) 50%
\n(b) 90%
\n(c) 70%
\n(d) 30%<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) 90%
\nExplanation:
\nH2<\/sub>O2<\/sub> is used as an oxidant for rocket fuel. Usually, 90% concentration of H2<\/sub>O2<\/sub> is used.<\/p>\n<\/details>\n

\n

Question 20.
\nHydrogen has isotopes
\n(a) 2
\n(b) 3
\n(c) 4
\n(d) 5<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) 4
\nExplanation:
\nHydrogen has three main isotopes; Protium (1<\/sup>H), deuterium (\u00b2H) and tritium (\u00b3H). These isotopes form naturally in nature. Protium and deuterium are stable. Tritium is radioactive and has a half-life of about 12 years. Scientists have created four other hydrogen isotopes (4H to 7H), but these isotopes are very unstable and do not exist naturally.
\nThe main isotopes of hydrogen are unique because they are the only isotopes that have a name.<\/p>\n<\/details>\n

\n

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Students are advised to practice the\u00a0NCERT MCQ Questions for Class 11 Chemistry Chapter 9 Hydrogen with Answers Pdf free download is available here. MCQ Questions for Class 11 Chemistry with Answers are prepared as per the Latest Exam Pattern. Students can solve these Hydrogen Class 11 MCQs Questions with Answers and assess their preparation level. …<\/p>\n

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