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CHXI06:STATES OF MATTER

314063 Statement A :
At constant temperature, $p V$ versus $p$ plot for ideal gas is a straight line.
Statement B :
At high pressure all gases have $Z < 1$ but at intermediate pressure most gases have $Z > 1$ .

1 Statement A is correct but Statement B is incorrect.

2 Statement A is incorrect but Statement B is correct.

3 Both statements are correct.

4 Both Statements are incorrect.

Explanation:

At high pressure, all gases have $Z > 1$ but at intermediate pressure most gases have $Z < 1$ .

CHXI06:STATES OF MATTER

314064 The compressibility factor of a gas is more than unity at STP. Its value of $V_{m}$ is

1 Greater than

22.4 {dm}^{3}

2 Lesser than

22.4 {dm}^{3}

3 Equal to

22.4 {dm}^{3}

4 Dependent on its molecular mass

CHXI06:STATES OF MATTER

314065 Identify the wrong relation for real gases :

1

Z = \frac{V_{ideal}}{V_{real}}

2

p_{ideal} = p_{real} + \frac{a n^{2}}{V^{2}}

3

V_{real} = V_{ideal} - nb

4

(p + \frac{a}{V^{2}}) (V - b) = R T

Explanation:

Compressibility factor, $(Z) = \frac{V_{real}}{V_{ideal}}$

KCET - 2024

CHXI06:STATES OF MATTER

314047 The temperature at which real gases obey the ideal gas laws over a wide range of pressure is called

1 critical temperature

2 inversion temperature

3 Boyles temperature

4 reduced temperature

Explanation:

The temperature at which real gas behaves like ideal gas and obeys the gas laws over a wide range of pressure is called Boyle temperature $(T_{b})$ .
$T_{b} = \frac{a}{R b}$ and where, a and b van der Waals' constant.

CHXI06:STATES OF MATTER

314048 A gas is said to behave like an ideal gas when the relation $PV / T =$ constant. When do you expect a real gas to behave like an ideal gas?

1 when the temperature is low

2 when both the temperature and pressure is low

3 when both the temperature and pressure are high

4 when the temperature is high and pressure is low

Explanation:

$PV = nRT$ is an ideal gas equation, it is allowed when the temperature is high and pressure is low.

CHXI06:STATES OF MATTER

314063 Statement A :
At constant temperature, $p V$ versus $p$ plot for ideal gas is a straight line.
Statement B :
At high pressure all gases have $Z < 1$ but at intermediate pressure most gases have $Z > 1$ .

1 Statement A is correct but Statement B is incorrect.

2 Statement A is incorrect but Statement B is correct.

3 Both statements are correct.

4 Both Statements are incorrect.

Explanation:

At high pressure, all gases have $Z > 1$ but at intermediate pressure most gases have $Z < 1$ .

CHXI06:STATES OF MATTER

314064 The compressibility factor of a gas is more than unity at STP. Its value of $V_{m}$ is

1 Greater than

22.4 {dm}^{3}

2 Lesser than

22.4 {dm}^{3}

3 Equal to

22.4 {dm}^{3}

4 Dependent on its molecular mass

CHXI06:STATES OF MATTER

314065 Identify the wrong relation for real gases :

1

Z = \frac{V_{ideal}}{V_{real}}

2

p_{ideal} = p_{real} + \frac{a n^{2}}{V^{2}}

3

V_{real} = V_{ideal} - nb

4

(p + \frac{a}{V^{2}}) (V - b) = R T

Explanation:

Compressibility factor, $(Z) = \frac{V_{real}}{V_{ideal}}$

KCET - 2024

CHXI06:STATES OF MATTER

314047 The temperature at which real gases obey the ideal gas laws over a wide range of pressure is called

1 critical temperature

2 inversion temperature

3 Boyles temperature

4 reduced temperature

Explanation:

The temperature at which real gas behaves like ideal gas and obeys the gas laws over a wide range of pressure is called Boyle temperature $(T_{b})$ .
$T_{b} = \frac{a}{R b}$ and where, a and b van der Waals' constant.

CHXI06:STATES OF MATTER

314048 A gas is said to behave like an ideal gas when the relation $PV / T =$ constant. When do you expect a real gas to behave like an ideal gas?

1 when the temperature is low

2 when both the temperature and pressure is low

3 when both the temperature and pressure are high

4 when the temperature is high and pressure is low

Explanation:

$PV = nRT$ is an ideal gas equation, it is allowed when the temperature is high and pressure is low.

CHXI06:STATES OF MATTER

314063 Statement A :
At constant temperature, $p V$ versus $p$ plot for ideal gas is a straight line.
Statement B :
At high pressure all gases have $Z < 1$ but at intermediate pressure most gases have $Z > 1$ .

1 Statement A is correct but Statement B is incorrect.

2 Statement A is incorrect but Statement B is correct.

3 Both statements are correct.

4 Both Statements are incorrect.

Explanation:

At high pressure, all gases have $Z > 1$ but at intermediate pressure most gases have $Z < 1$ .

CHXI06:STATES OF MATTER

314064 The compressibility factor of a gas is more than unity at STP. Its value of $V_{m}$ is

1 Greater than

22.4 {dm}^{3}

2 Lesser than

22.4 {dm}^{3}

3 Equal to

22.4 {dm}^{3}

4 Dependent on its molecular mass

CHXI06:STATES OF MATTER

314065 Identify the wrong relation for real gases :

1

Z = \frac{V_{ideal}}{V_{real}}

2

p_{ideal} = p_{real} + \frac{a n^{2}}{V^{2}}

3

V_{real} = V_{ideal} - nb

4

(p + \frac{a}{V^{2}}) (V - b) = R T

Explanation:

Compressibility factor, $(Z) = \frac{V_{real}}{V_{ideal}}$

KCET - 2024

CHXI06:STATES OF MATTER

314047 The temperature at which real gases obey the ideal gas laws over a wide range of pressure is called

1 critical temperature

2 inversion temperature

3 Boyles temperature

4 reduced temperature

Explanation:

The temperature at which real gas behaves like ideal gas and obeys the gas laws over a wide range of pressure is called Boyle temperature $(T_{b})$ .
$T_{b} = \frac{a}{R b}$ and where, a and b van der Waals' constant.

CHXI06:STATES OF MATTER

314048 A gas is said to behave like an ideal gas when the relation $PV / T =$ constant. When do you expect a real gas to behave like an ideal gas?

1 when the temperature is low

2 when both the temperature and pressure is low

3 when both the temperature and pressure are high

4 when the temperature is high and pressure is low

Explanation:

$PV = nRT$ is an ideal gas equation, it is allowed when the temperature is high and pressure is low.

CHXI06:STATES OF MATTER

314063 Statement A :
At constant temperature, $p V$ versus $p$ plot for ideal gas is a straight line.
Statement B :
At high pressure all gases have $Z < 1$ but at intermediate pressure most gases have $Z > 1$ .

1 Statement A is correct but Statement B is incorrect.

2 Statement A is incorrect but Statement B is correct.

3 Both statements are correct.

4 Both Statements are incorrect.

Explanation:

At high pressure, all gases have $Z > 1$ but at intermediate pressure most gases have $Z < 1$ .

CHXI06:STATES OF MATTER

314064 The compressibility factor of a gas is more than unity at STP. Its value of $V_{m}$ is

1 Greater than

22.4 {dm}^{3}

2 Lesser than

22.4 {dm}^{3}

3 Equal to

22.4 {dm}^{3}

4 Dependent on its molecular mass

CHXI06:STATES OF MATTER

314065 Identify the wrong relation for real gases :

1

Z = \frac{V_{ideal}}{V_{real}}

2

p_{ideal} = p_{real} + \frac{a n^{2}}{V^{2}}

3

V_{real} = V_{ideal} - nb

4

(p + \frac{a}{V^{2}}) (V - b) = R T

Explanation:

Compressibility factor, $(Z) = \frac{V_{real}}{V_{ideal}}$

KCET - 2024

CHXI06:STATES OF MATTER

314047 The temperature at which real gases obey the ideal gas laws over a wide range of pressure is called

1 critical temperature

2 inversion temperature

3 Boyles temperature

4 reduced temperature

Explanation:

The temperature at which real gas behaves like ideal gas and obeys the gas laws over a wide range of pressure is called Boyle temperature $(T_{b})$ .
$T_{b} = \frac{a}{R b}$ and where, a and b van der Waals' constant.

CHXI06:STATES OF MATTER

314048 A gas is said to behave like an ideal gas when the relation $PV / T =$ constant. When do you expect a real gas to behave like an ideal gas?

1 when the temperature is low

2 when both the temperature and pressure is low

3 when both the temperature and pressure are high

4 when the temperature is high and pressure is low

Explanation:

$PV = nRT$ is an ideal gas equation, it is allowed when the temperature is high and pressure is low.

CHXI06:STATES OF MATTER

314063 Statement A :
At constant temperature, $p V$ versus $p$ plot for ideal gas is a straight line.
Statement B :
At high pressure all gases have $Z < 1$ but at intermediate pressure most gases have $Z > 1$ .

1 Statement A is correct but Statement B is incorrect.

2 Statement A is incorrect but Statement B is correct.

3 Both statements are correct.

4 Both Statements are incorrect.

Explanation:

At high pressure, all gases have $Z > 1$ but at intermediate pressure most gases have $Z < 1$ .

CHXI06:STATES OF MATTER

314064 The compressibility factor of a gas is more than unity at STP. Its value of $V_{m}$ is

1 Greater than

22.4 {dm}^{3}

2 Lesser than

22.4 {dm}^{3}

3 Equal to

22.4 {dm}^{3}

4 Dependent on its molecular mass

CHXI06:STATES OF MATTER

314065 Identify the wrong relation for real gases :

1

Z = \frac{V_{ideal}}{V_{real}}

2

p_{ideal} = p_{real} + \frac{a n^{2}}{V^{2}}

3

V_{real} = V_{ideal} - nb

4

(p + \frac{a}{V^{2}}) (V - b) = R T

Explanation:

Compressibility factor, $(Z) = \frac{V_{real}}{V_{ideal}}$

KCET - 2024

CHXI06:STATES OF MATTER

314047 The temperature at which real gases obey the ideal gas laws over a wide range of pressure is called

1 critical temperature

2 inversion temperature

3 Boyles temperature

4 reduced temperature

Explanation:

The temperature at which real gas behaves like ideal gas and obeys the gas laws over a wide range of pressure is called Boyle temperature $(T_{b})$ .
$T_{b} = \frac{a}{R b}$ and where, a and b van der Waals' constant.

CHXI06:STATES OF MATTER

314048 A gas is said to behave like an ideal gas when the relation $PV / T =$ constant. When do you expect a real gas to behave like an ideal gas?

1 when the temperature is low

2 when both the temperature and pressure is low

3 when both the temperature and pressure are high

4 when the temperature is high and pressure is low

Explanation:

$PV = nRT$ is an ideal gas equation, it is allowed when the temperature is high and pressure is low.