What would be the volume in liters of an ideal gas, if a 0.111 mole sample of the gas had a temperature of 1130 degrees celsius at a pressure of 5.45 atmospheres? (the ideal gas constant is 0.0821 l•atm/mol•k.)

0.43 liters

1.43 liters

1.89 liters

2.35 liters

Option (d) is the correct answer.

Explanation:

The given data is as follows.

      n = 0.111 mole,           T = 1130 degrees Celsius = 1130 + 273 = 1403 K

       P = 5.45 atm,            V = ?

       R = 0.0821 L atm/mol K

Using the ideal gas equation, we can calculate the volume as follows.

                                    PV = nRT

 or,                                V =

                                         =

                                         =

                                         =  2.346 L

or,                                     = 2.35 L (approx)

Thus, we can conclude that volume of the ideal gas is 2.35 liters.

c is the answer because when something is left after something evaporates that shows the chemical change.

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.