Self Studies

States of Matter Test - 12

Result Self Studies

States of Matter Test - 12
  • Score

    -

    out of -
  • Rank

    -

    out of -
TIME Taken - -
Self Studies

SHARING IS CARING

If our Website helped you a little, then kindly spread our voice using Social Networks. Spread our word to your readers, friends, teachers, students & all those close ones who deserve to know what you know now.

Self Studies Self Studies
Weekly Quiz Competition
  • Question 1
    1 / -0
    When two molecules of an ideal gas collide:
    Solution
    According to one of the postulates of kinetic gas theory, the kinetic energy of the gas molecules is not changed into any other form of energy and it remains constant before and after the collision between gas molecules.
  • Question 2
    1 / -0
    Which of the following values is not correct?
    Solution
    The value of R (gas constant) has different values in different units. 
    $$R = 8.314 \ J/K-mol$$
    $$R = 62.36 \ torr/K-mol$$
    $$R = 0.0821 \ L-atm/K-mol$$
    $$R = 2 \ calories/K-mol $$
  • Question 3
    1 / -0
    According to kinetic theory of gases, there are:
    Solution

    Postulates of Kinetic Theory of Gases :

    1) The molecules in a gas are small and very far apart. Most of the volume which a gas occupies is empty space.

    2) Gas molecules are in constant random motion. Just as many molecules are moving in one direction as in any other.

    3) Molecules can collide with each other and with the walls of the container. Collisions with the walls account for the pressure of the gas.

    4) When collisions occur, the molecules lose no kinetic energy; that is, the collisions are said to be perfectly elastic. The total kinetic energy of all the molecules remains constant unless there is some outside interference.

    5) The molecules exert no attractive or repulsive forces on one another except during the process of collision. Between collisions, they move in straight lines.


    Hence, Option "C" is the correct answer.

  • Question 4
    1 / -0
    Which is wrong according to kinetic theory?
    Solution
    K.E. = $$\cfrac {1}{2} mv^2$$ and from Maxwell distribution curve it can be seen that molecules of all the gases have a wide range of speed so they have different kinetic energy.
    Hence option B is correct.
  • Question 5
    1 / -0
    $$V$$ versus $$T$$ curves at constant pressure $$P_{1}$$ and $$P_{2}$$ for an ideal gas are shown in the figure given above. Choose the correct relation.

    Solution
    According to Charles's law, when the pressure on a sample of a dry gas is held constant, the Kelvin temperature and the volume will be directly related.

    This directly proportional relationship can be written as: $$V  \propto  T$$ & $$ P \propto T$$

    For the above case, let us consider at a point volume is constant. We find that the temperature of the gas at pressure $$P_2$$ is greater than that of gas at pressure $$P_1$$.

    $$\therefore$$  $$P_1 < P_2$$

    Hence, Option "B" is the correct answer.
  • Question 6
    1 / -0
    Which is wrong according to kinetic theory of gases?
    Solution
    In kinetic theory of gases pressure is due to the molecules colliding with the walls of the container and not when molecules collide with each other.
  • Question 7
    1 / -0
    Which of the following mixture does not obey Dalton's law of partial pressures?
    Solution
    $$SO_{2}+Cl_{2}\rightarrow SO_2Cl_2$$ 

    $$SO_{2}+Cl_{2}$$ does not obey the Dalton's law of partial pressures because it is valid for non-reacting gases.
  • Question 8
    1 / -0
    Which of the following is a representation of Gay-Lussac's law?          
    Solution
    According to Gay-Lussac's law, at constant volume, the pressure of the gas is proportional to it's absolute temperature.

    So, $$\dfrac{P_{1}}{T_{1}} = \dfrac{P_{2}}{T_{2}}$$

    This gives, $$P_{1}T_{2} = P_{2}T_{1}$$.
  • Question 9
    1 / -0
    The correct gas equation is:

    Solution
    Hint: Use Ideal gas equation

    Explanation:
    Ideal gas equation is stated as;
    $$PV = nRT$$
    Where, $$P$$ is Pressure
                  $$V$$ is Volume
                  $$n$$ is number of moles
                  $$R$$ is Ideal gas constant
                  $$T$$ is Absolute Temperature
    As, $$n$$ and $$R$$ are constant So, relation between $$P,V$$ and $$T$$ shown as;

    Equation of state is $$\dfrac{P_1V_1}{T_1} = \dfrac{P_2V_2}{T_2}$$

    Rearranging the equation we get;
    $$\dfrac{P_1V_1}{P_2V_2} = \dfrac{T_1}{T_2}$$

    Final Answer: Option $$B$$
  • Question 10
    1 / -0
    When an ideal gas undergoes expansion through a porous plug, the gas is expected to exhibit no cooling because ___________.
    Solution
    When an ideal gas undergoes expansion through a porous plug, the gas is expected to exhibit no cooling because according to kinetic theory of gases there exist no molecular forces of attraction.
Self Studies
User
Question Analysis
  • Correct -

  • Wrong -

  • Skipped -

My Perfomance
  • Score

    -

    out of -
  • Rank

    -

    out of -
Re-Attempt Weekly Quiz Competition
Self Studies Get latest Exam Updates
& Study Material Alerts!
No, Thanks
Self Studies
Click on Allow to receive notifications
Allow Notification
Self Studies
Self Studies Self Studies
To enable notifications follow this 2 steps:
  • First Click on Secure Icon Self Studies
  • Second click on the toggle icon
Allow Notification
Get latest Exam Updates & FREE Study Material Alerts!
Self Studies ×
Open Now