At low pressure, if `RT=2sqrt(a.p),` then the volume occupied by a real gas is :
At low pressure, if `RT=2sqrt(a.p),` then the volume occupied by a real gas is :
A
`(2RT)/(P)`
B
`(2P)/(RT)`
C
`(RT)/(2P)`
D
`(2RT)/(P)`
Text Solution
AI Generated Solution
The correct Answer is:
To solve the problem, we need to find the volume occupied by a real gas at low pressure given the equation \( RT = 2\sqrt{a \cdot p} \).
### Step-by-Step Solution:
1. **Understanding the Given Equation**:
We start with the equation provided:
\[
RT = 2\sqrt{a \cdot p}
\]
This equation relates the gas constant \( R \), temperature \( T \), the pressure \( p \), and a constant \( a \) which is specific to the gas.
2. **Using the Van der Waals Equation**:
For a real gas, we can use the Van der Waals equation:
\[
\left( p + \frac{a}{V^2} \right) (V - b) = RT
\]
At low pressure, we can assume that the volume \( V \) is very large compared to \( b \), allowing us to neglect the term \( b \). Thus, we can simplify the equation to:
\[
p + \frac{a}{V^2} = \frac{RT}{V}
\]
3. **Rearranging the Equation**:
Rearranging gives:
\[
pV + \frac{a}{V} = RT
\]
This can be rewritten as:
\[
pV^2 + a = RTV
\]
4. **Substituting for RT**:
Now, substitute \( RT \) from the first step:
\[
pV^2 + a = 2\sqrt{a \cdot p} \cdot V
\]
Rearranging this gives us a quadratic equation in terms of \( V \):
\[
pV^2 - 2\sqrt{a \cdot p} \cdot V + a = 0
\]
5. **Using the Quadratic Formula**:
We can solve for \( V \) using the quadratic formula:
\[
V = \frac{-b \pm \sqrt{b^2 - 4ac}}{2a}
\]
Here, \( a = p \), \( b = -2\sqrt{a \cdot p} \), and \( c = a \). Thus:
\[
V = \frac{2\sqrt{a \cdot p} \pm \sqrt{(2\sqrt{a \cdot p})^2 - 4 \cdot p \cdot a}}{2p}
\]
6. **Simplifying the Expression**:
Simplifying the term under the square root:
\[
(2\sqrt{a \cdot p})^2 - 4pa = 4ap - 4ap = 0
\]
This means the discriminant is zero, indicating there is one solution:
\[
V = \frac{2\sqrt{a \cdot p}}{2p} = \frac{\sqrt{a \cdot p}}{p}
\]
7. **Final Volume Expression**:
Therefore, the volume occupied by the real gas is:
\[
V = \frac{RT}{2p}
\]
### Final Answer:
The volume occupied by the real gas at low pressure is:
\[
V = \frac{RT}{2p}
\]
To solve the problem, we need to find the volume occupied by a real gas at low pressure given the equation \( RT = 2\sqrt{a \cdot p} \).
### Step-by-Step Solution:
1. **Understanding the Given Equation**:
We start with the equation provided:
\[
RT = 2\sqrt{a \cdot p}
...
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van der Waal's equation for calculating the pressure of a non ideal gas is (P+(an^(2))/(V^(2)))(V-nb)=nRT van der Waal's suggested that the pressure exerted by an ideal gas , P_("ideal") , is related to the experiventally measured pressure, P_("ideal") by the equation P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2)))) Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas . Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows : underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT For non-zero value of force of attraction between gas moleculer at large volume, gas equation will be :
van der Waal's equation for calculating the pressure of a non ideal gas is (P+(an^(2))/(V^(2)))(V-nb)=nRT van der Waal's suggested that the pressure exerted by an ideal gas , P_("ideal") , is related to the experiventally measured pressure, P_("ideal") by the equation P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2)))) Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas . Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows : underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT The van der Waals' constant 'a' for CO_(2) gas is greater than that of H_(2) gas. Its mean that the
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