What are the bond angles in BeCl_2? a. 180 degree b. 109 degree c. 120 degree d.

Question

What are the bond angles in BeCl_2? a. 180 degree b. 109 degree c. 120 degree d. 90 degree e. not enough information What is the hybridization of the central atom information What is the hybridization of the central atom in chloroform CHCI_3? a. sp b. sp^2 c. sp^4 d. sp^3 e. not hybridized The boiling point of liquid oxygen is 90.2 K. What is this temperature in Celsius? a. -208.0 degree C b. 363.4 degree C c. 90.2 degree C d. 194.4 degree C e. -183.0 degree C The ideal gas law is used for most applications, but at high pressures the ideal gas law becomes inaccurate and the van der Walls equation is used instead. Why must the van der Walls equation be used at high pressures? a. Because chemical reactions begin to occur between gas molecules b. Because the temperature becomes too difficult to measure c. Because the pressure becomes too difficult to measure d. Because the gas molecules occupy a significant fraction of the volume e. Because the velocity of the gas molecules is too slow at high pressures.

Explanation / Answer

7.

Ans - a) 1800

BeCl2 is linear molecule and have Cl - Be - Cl bond angle is 1800

8.

Ans - d) sp3

in CHCl3 central atom carbon hybridized to form four sp3 hybridized one sp3 hybridized orbital form sigma bond with hydrogen and remained three sp3 hybridized orbital form three sigma bond with three Cl atom.

9.

Ans -

T(0C)   = T(K) - 273.15

T(0C)   = 90.2 - 273.15 = - 182.95 = -1830C

e) - 1830C

10.

Ans - d) Because gas molecule occupy a significant fraction of volume.

At the normal pressure volume occupied by gas particle is negligibly small fraction of total volume of the gas but at high pressure this is no longer true as result real gas are not as compressible at high pressure as an ideal gas. Volume of real gas is therefore larger than expected from the ideal gas equation at high pressure.

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