States of Matter Test

Result

States of Matter Test - 70

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Weekly Quiz Competition

Question 1
1 / -0

Vapour pressure of pure 'A' is 70 mm of Hg at $$25^0C$$ it forms an ideal solution is with 'B' in which mole fraction of A is 0.8. If the vapour pressure of the solution is 84 mm is Hg at $$25^0C$$, the vapour pressure of pure 'B' at $$25^0C$$ is :

A
56 mm Hg

B
70 mm Hg

C
140 mm Hg

D
28 mm Hg
Question 2
1 / -0

A solution is prepared by mixing $${\text{8}}{\text{.5}}\,{\text{g}}$$ of $${\text{C}}{{\text{H}}_{\text{2}}}{\text{C}}{{\text{l}}_2}$$ and $$11.95\,{\text{g}}$$ of $${\text{CHC}}{{\text{l}}_{\text{3}}}$$. If vapour pressure of $${\text{C}}{{\text{H}}_{\text{2}}}{\text{C}}{{\text{l}}_{\text{2}}}$$ and $${\text{CHC}}{{\text{l}}_3}$$ at $${\text{298}}\,{\text{K}}$$ are $$415$$ and $$200\,{\text{mm}}$$ Hg respecetively, then mole fraction of $${\text{CHC}}{{\text{l}}_{\text{3}}}$$ in vapour form is:

A
$$0.162$$

B
$$0.675$$

C
$$0.325$$

D
$$0.486$$

Solution
Question 3
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Two liquids A and B form ideal solution.At 300K,the vapour pressure of solution containing 1 mol of A and 3 mol of B is 550mm Hg.At the same temperature,if one more mole of B is added to this solution,the vapour pressure of the solution increases by 10mm Hg.Determine the vapour pressures of A and B in their pure states.

A
$$563$$ and $$469$$

B
$$500$$ adn $$1250$$

C
$$513$$ and $$494$$

D
$$400$$ and $$600$$

Solution
Question 4
1 / -0

The kinetic energy of $$1\ mole$$ of gas is equal to-

A
$$\dfrac {3}{2}RT$$

B
$$\dfrac {3}{2}KT$$

C
$$\dfrac {RT}{2}$$

D
$$\dfrac {2R}{3}$$

Solution

Kinetic enedy of gaseous molecule is calculaed using following formula.
$$KE= \frac{3}{2}\times nRT$$.
Above formula is given for n moles
So for 1 mole $$n=1$$
$$KE= \frac{3}{2}\times 1\times RT$$.
$$KE= \frac{3}{2}\times RT$$.
Hence option A is correct.
Question 5
1 / -0

Pressure exerted by 2 grams of helium present in a vessel is 1.5 atm. If 4 grams of gas 'X' is introduced into the same vessel keeping the condition constant, the pressure is 2.25 atm. Gas 'x' is

A
hydrogen

B
methane

C
oxygen

D
soldier oxide

Solution
Question 6
1 / -0

The figure shows the graphs of pressure versus density for an ideal gas at two temperatures, $$T_1$$ and $$T_2$$, according to this which is correct?

A
$$T_1 > T_2$$

B
$$T_1 = T_2$$

C
$$T_1 < T_2$$

D
none of the above
Question 7
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The value of gas constant per mole is approximately-

A
1 cal

B
2 cal

C
3 cal

D
4 cal
Question 8
1 / -0

Two gases X and Y have densities, $${d_{(x)}} = 3{d_{(y)}}$$ and molecular masses, $${M_{(x)}} = 0.5{M_{(y)}}$$. Then, the ratio of their pressures, i.e, $${P_x}:{P_y}$$ would be

A
1/4

B
1/6

C
4

D
6

Solution
Question 9
1 / -0

The vapour pressure of water at T(K) is 20 mm Hg. The following solutions are prepared at T(K) :

A
6 g of urea (mol. wt. = 60) is dissolved in 178.2 g of water

B
0.01 mole of glucose is dissolved in 179.82 g of water

C
5.3 g of $$N{a_2}C{O_3}$$ (mol. wt. =106) is dissolved in 179.1 g of water.

D
non of these

Solution
Question 10
1 / -0

Two flasks of equal volume, connected by a narrow tube of negligible volume, contain $$2$$ moles of $$H_2$$ gas at $$1$$ atm pressure and $$300$$ K. Now, one of the flasks are heated to $$400$$ K and the other is maintained at $$300 K$$, then find final pressure:

A
$$\cfrac {8}{5}$$ atm

B
$$\cfrac {5}{3}$$ atm

C
$$\cfrac {7}{5}$$ atm

D
$$\cfrac {8}{7}$$ atm