\(P_1V = n_1RT\)
\(P_2V = n_2RT\)
\(⇒ (100 kPa) V = (n_1 + n_2)RT\)
\(⇒n_1+n_2=\frac{(100 kPa)(2000 cm)^3)}{8.3×300}….(1)\)
Also, \(n_1 × 2 + n_2 × 32 = 0.76 ….(2)\)
Solving (1) and (2),
\(n_1 = 0.06\)
\(n_2 = 0.02\)
\(⇒ \frac{n_1}{n_2} = 3\)
Hence, the correct option is (B): \(\frac{3}{1}\)
The temperature at which the rms speed of oxygen molecules is 75\% of the rms speed of nitrogen molecules at a temperature of \( 287^\circ C \) is:
Let \( y = f(x) \) be the solution of the differential equation
\[ \frac{dy}{dx} + 3y \tan^2 x + 3y = \sec^2 x \]
such that \( f(0) = \frac{e^3}{3} + 1 \), then \( f\left( \frac{\pi}{4} \right) \) is equal to:
Find the IUPAC name of the compound.
If \( \lim_{x \to 0} \left( \frac{\tan x}{x} \right)^{\frac{1}{x^2}} = p \), then \( 96 \ln p \) is: 32
The gas laws were developed at the end of the 18th century, when scientists began to realize that relationships between pressure, volume and temperature of a sample of gas could be obtained which would hold to approximation for all gases.