States of Matter Test

Result

States of Matter Test - 66

Score
-
out of -
Rank
-
out of -

TIME Taken - -

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.

Weekly Quiz Competition

Question 1
1 / -0

A sample of water gas contains $$42\%$$ by volume of carbon monoxide,If the total pressure is 760 mm. the partial pressure of carbon monoxide is?

A
380 mm

B
319.2 mm

C
38 mm

D
360 mm

Solution
Question 2
1 / -0

At same temperature $$N_2O_4$$ is dissolved to 40% and 50% at total presure $$p_1$$ and $$p_2$$ atm respevtively in $$NO_2$$.Then the ratio of $$P_1$$ &$$P_2$$ is?

A
$$\frac { 4 }{ 5 } $$

B
$$\frac { 7 }{ 4 }$$

C
$$\frac { 4 }{ 7 }$$

D
None of these

Solution
Question 3
1 / -0

For the adiabatic expansion of an ideal gas

A
PV $$^{\gamma}$$= constant

B
TV $$^{\gamma-1}$$ = constant

C
T $$^{\gamma}$$P $$^{1-\gamma}$$ =constant

D
All of these
Question 4
1 / -0

The vapour pressure of pure benzene at a certain temperature is 200 mm Hg. At the same temperature the vapour pressure of a solution containing 2 g of non volatile non electrolyte solid in 78 g of benzene is 195 mm Hg. What is the molecular mass of solid?

A
50

B
70

C
85

D
80

Solution
Question 5
1 / -0

One atmosphere is numerically equal to approximately?

A
$${ 10 }^{ 6 }{ dyne\quad cm }^{ -2 }$$

B
$${ 10 }^{ 2 }{ dyne\quad cm }^{ -2 }$$

C
$${ 10 }^{ 4 }{ dyne\quad cm }^{ -2 }$$

D
$${ 10 }^{ 8 }{ dyne\quad cm }^{ -2 }$$

Solution
Question 6
1 / -0

A spherical balloon of $$21\ cm$$ diameter is to be filled up with $$H_2$$ at $$NTP$$ from a cylinder containing the gas at $$20\ atm$$ at $$27^{\circ}C$$. The cylinder can hold $$2.82$$ litre of water. The number of balloons that can be filled up

A
11

B
10

C
8

D
1

Solution
Question 7
1 / -0

In a gaseous mixture at $$20^o C$$ the partial pressure of the components are:
$${ H }_{ 2 }$$ : 150 Torr $${ CH }_{ 4 }$$ : 300 Torr $${ CO }_{ 2 }$$ : 200 Torr $${ C }_{ 2 }{ H }_{ 4 }$$ : 100 Torr
The volume % of $${ H }_{ 2 }$$ in mixture:

A
26.67

B
73.33

C
80.00

D
20

Solution
Question 8
1 / -0

$$200\ ml$$ of $$He$$ at $$0.66\ atm$$ pressure and $$400\ ml$$ of $${ O }_{ 2 }$$ at $$0.52\ atm$$ pressure are mixed in a $$400\ ml$$ vessel at $${ 25 }^{ \circ }C$$. The partial pressure of $$He$$ and $${ O }_{ 2 }$$ will be:

A
$$0.33\ and\ 0.56$$

B
$$0.33\ and\ 0.52$$

C
$$0.38\ and\ 0.56$$

D
$$0.25\ and\ 0.45$$

Solution

Partial pressure is the pressure of individual gas when it is placed in a required vessel or in final vessel.

Given :- Initially volume of $$He$$ is $$200\ ml$$ at $$0.66\ atm$$ after placing it in a vessel of volume $$400\ ml$$

$$P_{1} V_{1}= P_{2} V_{2}$$

$$.66 \times 200 = P_{2} \times 400$$

$$P_{2}= 0.33\ atm$$ ----------- (Partial pressure of $$He$$)

Initially $$O_{2}$$ is present at $$0.25\ atm$$ in $$ 400\ ml$$ volume and then it is placed in $$400\ ml$$ vessel hence the partial pressure of $$O_{2}$$ is $$0.52\ atm$$

Partial pressure of $$He=0.33\ atm$$
Partial pressure of $$O_{2}= 0.52\ atm$$
Question 9
1 / -0

The reduction potential of hydrogen electrode will be positive if

A
$${P_{{H_2}}} = 2\;atm;\left[ {H^ + } \right] = 1\;M$$

B
$${P_{{H_2}}} = 2.5\;atm;\left[ {H^ + } \right] = 1.5\;M$$

C
$${P_{{H_2}}} = 2.5\;atm;\left[ {H^ + } \right] = 1\;M$$

D
$${P_{{H_2}}} = 1\;atm;\left[ {H^ + } \right] = 2\;M$$

Solution
Question 10
1 / -0

The ratio of densities of a gas at two conditions of temperature and pressure is given by:

A
$$\dfrac{\rho_2}{\rho_1} = \left(\dfrac{p_2}{p_1} \right) \left(\dfrac{T_2}{T_1} \right)$$

B
$$\dfrac{\rho_2}{\rho_1} = \left(\dfrac{p_2}{p_1} \right) \left(\dfrac{T_1}{T_2} \right)$$

C
$$\dfrac{\rho_2}{\rho_1} = \left(\dfrac{p_1}{p_2} \right) \left(\dfrac{T_1}{T_2} \right)$$

D
$$\dfrac{\rho_2}{\rho_1} = \left(\dfrac{p_1}{p_2} \right) \left(\dfrac{T_2}{T_1} \right)$$

Solution

The density $$(S)$$ of an ideal gas is given as
$$S = \frac{ PM }{ RT }$$
Where,
$$P=$$ Pressure
$$T=$$ Temperature
$$R=$$ Universal gas content
$$M=$$ Molar Mass
Here, $$R$$ and $$M$$ are constant for a given gas
Therefore;
(refer image 1)