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Dry ice is ______. - Chemistry

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प्रश्न

Dry ice is ______.

पर्याय

  • Solid NH3

  • Solid SO2

  • Solid CO2

  • Solid N2

MCQ
रिकाम्या जागा भरा
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उत्तर

Dry ice is solid CO2.

Explanation:

Solid CO2 is referred to as dry ice because it is used in laboratories to create an ice bath for organic reactions. It is made by rapidly cooling high-pressure CO2 gas.

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Group 13 Elements - The Boron Family
  या प्रश्नात किंवा उत्तरात काही त्रुटी आहे का?
पाठ 11: The p-block Elements - Multiple Choice Questions (Type - I) [पृष्ठ १३६]

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एनसीईआरटी एक्झांप्लर Chemistry [English] Class 11
पाठ 11 The p-block Elements
Multiple Choice Questions (Type - I) | Q 14 | पृष्ठ १३६

संबंधित प्रश्‍न

If B–Cl bond has a dipole moment, explain why BCl3 molecule has zero dipole moment.


Aluminium trifluoride is insoluble in anhydrous HF but dissolves on the addition of NaF. Aluminium trifluoride precipitates out of the resulting solution when gaseous BF3 is bubbled through. Give reasons.


How would you explain the lower atomic radius of Ga as compared to Al?


Write a balanced equation for B2H6 + NH3 → ?


A compound X, of boron reacts with NH3 on heating to give another compound Y which is called inorganic benzene. The compound X can be prepared by treating BF3 with Lithium aluminium hydride. The compounds X and Y are represented by the formulas.


Cement, the important building material is a mixture of oxides of several elements. Besides calcium, iron and sulphur, oxides of elements of which of the group (s) are present in the mixture?


Which of the following statements are correct. Answer on the basis of Figure.

(i) The two birdged hydrogen atoms and the two boron atoms lie in one plane;

(ii) Out of six B – H bonds two bonds can be described in terms of 3 centre 2-electron bonds.

(iii) Out of six B – H bonds four B – H bonds can be described in terms of 3 centre 2 electron bonds;

(iv) The four-terminal B – H bonds are two centre-two electron regular bonds.


Explain why the following compounds behave as Lewis acids?

BCl3


Explain the following:

Boron does not exist as B3+ ion.


Explain the following:

Electron gain enthalpy of chlorine is more negative as compared to fluorine.


Identify the compounds A, X and Z in the following reactions:

\[\ce{A + 2HCl + 5H2O -> 2NaCl + X}\]


Complete the following chemical equations:

\[\ce{Z + 3 LiAlH4 -> X + 3LiF + 3AlF_3}\]

\[\ce{X + 6H2 -> Y + 6H2}\]

\[\ce{3X + 3O2 ->[Δ] B2O3 + 3H2O}\]


Describe the general trends in the following properties of the elements in Groups 13 and 14.

Atomic size


Describe the general trends in the following properties of the elements in Groups 13 and 14.

Ionisation enthalpy


Describe the general trends in the following properties of the elements in Groups 13 and 14.

Metallic character


Boron compounds behave as Lewis acids because of their ______.


A group 13 element ‘X’ reacts with chlorine gas to produce a compound XCl3. XCl3 is electron deficient and easily reacts with NH3 to form \[\ce{Cl3X –> NH3}\] adduct; however, XCl3 does not dimerize X is ______.


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