States of Matter Test

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States of Matter Test - 53

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Question 1
1 / -0

60 cc of oxygen was added to 24 cc of carbon monoxide and the mixture ignited. Calculate the volume of $$O_2$$ used up and the volume of $$CO_2$$ formed.

A
15 cc, 30 cc

B
12 cc, 24 cc

C
20 cc, 40 cc

D
10 cc, 20 cc

Solution
Question 2
1 / -0

''Total pressure of a gaseous mix is equal to the sum of the partial pressures'', this statement is from :

A
Boyle's law

B
Charles's law

C
Avogadro's principle

D
ideal gas law

E
Dalton's law

Solution

Dalton's law of partial pressures states that the total pressure exerted by a mixture of gases is the sum of partial pressure of each individual gas present. Each gas is assumed to be an ideal gas.
$$P_total = P_1 + P_2 + P_3 + . .$$
Where, $$P_1$$ and $$P_2$$ are the partial pressure of gas 1 and gas 2 in the mixture. Since, each gas behaves independently, the ideal gas law can be used to calculate the pressure of that ga,s if we know the number of moles of the gas, the total volume of the container, and the temperature of the gas.
Question 3
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Statement 1: At the same temperature and pressure, 1 L of hydrogen gas and 1 L of neon gas have the same mass.
Statement 2: Equal volumes of ideal gases at the same temperature and pressure contain the same number of moles.

A
Both statement 1 and statement 2 are correct and statement 2 is the correct explanation of statement 1

B
Both statement 1 and statement 2 are correct but Statement 2 is not the correct explanation of Statement 1

C
Statement 1 is correct but statement 2 is incorrect

D
Statement 1 is incorrect but statement 2 is correct

E
Both the statement 1 and statement 2 are incorrect

Solution

Statement 1: At the same temperature and pressure, 1 L of hydrogen gas and 1 L of neon gas have the same volume.
Statement 2: Equal volumes of ideal gases at the same temperature and pressure contain the same number of moles.
For example, 1 mole of any gas at STP will occupy a volume of 22.4 L.
Hence, statement 1 is not correct but statement 2 is correct.
Question 4
1 / -0

Among the following which one shows that the total pressure of a mixture of gases is equal to the sum of the partial pressure of the component gases.

A
V/T$$=$$k

B
P/T$$=$$k

C
PV$$=$$k

D
$$P_T=P_1+P_2+P_3$$

E
PT$$=$$k

Solution

The total pressure of a mixture of gases is equal to the sum of the partial pressure of the component gases.
$$\displaystyle P_T=P_1+P_2+P_3 $$
$$\displaystyle P_T=$$ total pressure of a mixture of gases.
$$\displaystyle P_1, P_2, P_3 = $$ partial pressures of the component gases.
Question 5
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At constant temperature, the pressure of a gas is __________ to its volume.

A
inversely proportional

B
directly proportional

C
not proportional

D
none of the above

Solution

At constant temperature the pressure of a gas is inversely proportional to its volume. This law is called Boyle's law.
$$P \propto \cfrac { 1 }{ V } $$
So answer is A.
Question 6
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All of the following statements are related to the kinetic molecule theory of gases except:

A
gas molecules have no inter-molecular forces

B
gas particles are in random motion

C
the collisions between gas particles are elastic

D
gas particles have no volume

E
the average kinetic energy is proportional to the celsius temperature of the gas

Solution

The average kinetic energy is proportional to the absolute temperature of the gas.
Absolute temperature is the temperature in kelvin.
Question 7
1 / -0

The vapour pressures of two liquids A and B in their pure states are in the ratio of 1 : 2. A binary solution of A and B contains A and B in the mole proportion of 1 : 2. The mole fraction of A in the vapour phase of the solution will be:

A
$$0.33$$

B
$$0.2$$

C
$$0.25$$

D
$$0.52$$

Solution

$$\dfrac {P^o_A}{P^o_B} = \dfrac{1}{2}$$

$$\dfrac {x_A}{x_B} = \dfrac{1}{2}$$

$$P_T \gamma _A =\ P^o_Ax_A$$

$$\therefore \dfrac{ \gamma _A}{ \gamma _B}= \dfrac {P^o_A}{P^o_B} \dfrac {x_A}{x_B} $$

We know $$\gamma _A + \gamma _B =1$$

$$\therefore \gamma _A = 0.2$$

Hence, the correct option is $$\text{B}$$
Question 8
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Which of the following variables is not included in the ideal gas equation?

A
Mass

B
Pressure

C
Volume

D
Number of particles

E
Temperature

Solution

(A) : Mass.
$$pV = nRT$$ , The Ideal gas equation.
Here , P = pressure,
V = volume
n = number of moles of particles.
R = gas constant ( Not variable)
So, here the mass is not included, in Ideal gas equation.
T = temperature,
Question 9
1 / -0

Ideal gases:

A
have forces of attraction between them

B
are always linear in shape

C
never travel with a straight line motion

D
have molecules that are close together

E
have low masses and are spread far apart

Solution

Ideal gas have low masses and are spread far apart.
An ideal gas is defined as one in which all collisions between atoms or molecules are perfectly eleastic and in which there are no intermolecular attractive forces. One can visualize it as a collection of perfectly hard spheres which collide but which otherwise do not interact with each other. In such a gas, all the internal energy is in the form of kinetic energy and any change in internal energy is accompanied by a change in temperature
Question 10
1 / -0

Statement 1 : In the kinetic theory of gases, collisions between gas particles and the walls of the container are considered elastic.
Statement 2 : Gas molecules are considered point like, volume less particles with no inter molecular forces and in constant, random motion.

A
Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

B
Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.

C
Statement 1 is correct but Statement 2 is not correct.

D
Statement 1 is not correct but Statement 2 is correct.

E
Both the Statement 1 and Statement 2 are not correct.

Solution

The following statements are the two separate and independent assumptions of kinetic theory of gases:

1. Gas particles are constantly colliding with each other and the walls of their container. These collisions are elastic; that is, there is no net loss of energy from the collisions

2. Gas particles are small and the total volume occupied by gas molecules is negligible relative to the total volume of their container.

Hence, both the statements are true. However, Statement 2 is not the correct explanation of statement 1

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States of Matter Test - 53

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States of Matter Test - 53

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Question 1

15 cc, 30 cc

12 cc, 24 cc

20 cc, 40 cc

10 cc, 20 cc

Solution

Question 2

Boyle's law

Charles's law

Avogadro's principle

ideal gas law

Dalton's law

Solution

Question 3

Both statement 1 and statement 2 are correct and statement 2 is the correct explanation of statement 1

Both statement 1 and statement 2 are correct but Statement 2 is not the correct explanation of Statement 1

Statement 1 is correct but statement 2 is incorrect

Statement 1 is incorrect but statement 2 is correct

Both the statement 1 and statement 2 are incorrect

Solution

Question 4

V/T$$=$$k

P/T$$=$$k

PV$$=$$k

$$P_T=P_1+P_2+P_3$$

PT$$=$$k

Solution

Question 5

inversely proportional

directly proportional

not proportional

none of the above

Solution

Question 6

gas molecules have no inter-molecular forces

gas particles are in random motion

the collisions between gas particles are elastic

gas particles have no volume

the average kinetic energy is proportional to the celsius temperature of the gas

Solution

Question 7

$$0.33$$

$$0.2$$

$$0.25$$

$$0.52$$

Solution

Question 8

Mass

Pressure

Volume

Number of particles

Temperature

Solution

Question 9

have forces of attraction between them

are always linear in shape

never travel with a straight line motion

have molecules that are close together

have low masses and are spread far apart

Solution

Question 10

Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.

Statement 1 is correct but Statement 2 is not correct.

Statement 1 is not correct but Statement 2 is correct.

Both the Statement 1 and Statement 2 are not correct.

Solution

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