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Which of the following statements indicates that law of multiple proportion is being followed?
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One of the statements of Dalton’s atomic theory is given below: “Compounds are formed when atoms of different elements combine in a fixed ratio”
Which of the following laws is not related to this statement?
(i) Law of conservation of mass
(ii) Law of definite proportions
(iii) Law of multiple proportions
(iv) Avogadro law
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If two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element, are in whole number ratio.
Is this statement true?
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If two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element, are in whole number ratio.
If yes, according to which law?
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If two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element, are in whole number ratio.
Give one example related to this law.
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Define the law of multiple proportions. Explain it with two examples. How does this law point to the existence of atoms?
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A box contains some identical red coloured balls, labelled as A, each weighing 2 grams. Another box contains identical blue coloured balls, labelled as B, each weighing 5 grams. Consider the combinations AB, AB2, A2B and A2B3 and show that law of multiple proportions is applicable.
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Which of the following options represents the correct bond order?
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Which of the following have identical bond order?
(i) \[\ce{CN-}\]
(ii) \[\ce{NO+}\]
(iii) \[\ce{O^{-}2}\]
(iv) \[\ce{O^{2-}2}\]
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Species having same bond order are:
(i) \[\ce{N2}\]
(ii) \[\ce{N^{-}2}\]
(iii) \[\ce{F^{+}2}\]
(iv) \[\ce{O^{-}2}\]
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Using molecular orbital theory, compare the bond energy and magnetic character of \[\ce{O^{+}2}\] and \[\ce{O^{-}2}\] species.
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What is the effect of the following processes on the bond order in \[\ce{N2}\] and \[\ce{O2}\]?
(i) \[\ce{N2 -> N^{+}2 + e-}\]
(ii) \[\ce{O2 -> O^{+}2 + e-}\]
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Match the species in Column I with the bond order in Column II.
| Column I | Column II |
| (i) \[\ce{NO}\] | (a) 1.5 |
| (ii) \[\ce{CO}\] | (b) 2.0 |
| (iii) \[\ce{O^{-}2}\] | (c) 2.5 |
| (iv) \[\ce{O2}\] | (d) 3.0 |
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Which of the following pair is expected to have the same bond order?
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As the temperature increases, average kinetic energy of molecules increases. What would be the effect of increase of temperature on pressure provided the volume is constant?
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Match the graphs between the following variables with their names:
| Graphs | Names | ||
| (i) | Pressure vs temperature graph at constant molar volume. | (a) | Isotherms |
| (ii) | Pressure vs volume graph at constant temperature. | (b) | Constant temperature curve |
| (iii) | Volume vs temperature graph at constant pressure. | (c) | Isochores |
| (d) | Isobars |
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Assertion (A): The temperature at which vapour pressure of a liquid is equal to the external pressure is called boiling temperature.
Reason (R): At high altitude atmospheric pressure is high.
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How can production of hydrogen from water gas be increased by using water gas shift reaction?
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In which of the following, functional group isomerism is not possible?
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Which of the following pairs are position isomers?
| I. | \[\begin{array}{cc} \phantom{.......................}\ce{O}\\ \phantom{.......................}||\\ \ce{CH3 - CH2 - CH2 - CH2 - C - H} \end{array}\] |
| II. | \[\begin{array}{cc} \phantom{.................}\ce{O}\\ \phantom{.................}||\\ \ce{CH3 - CH2 - CH2 - C - H} \end{array}\] |
| III. | \[\begin{array}{cc} \ce{CH3 - CH2 - C - CH2 - CH3}\\ \phantom{}||\\ \phantom{}\ce{O} \end{array}\] |
| IV. | \[\begin{array}{cc} \ce{CH3 - CH - CH2 - C - H}\\ \phantom{...}|\phantom{............}||\phantom{}\\ \phantom{...}\ce{CH3}\phantom{.........}\ce{O}\phantom{} \end{array}\] |
(i) I and II
(ii) II and III
(iii) II and IV
(iv) III and IV
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