4 g of an ideal gas $A$ (molar mass $=M_A$ ) present in a vessel of volume $V$ litre exerted a pressure of 5 atm at 300 K . When 16 g of another ideal gas $B$(molar mass $=M_B$ ) was introduced into this vessel at the same temperature, its pressure increased to 10 atm . What is the correct relationship between $M_A$ and $M_B$ ?
The sum of three values $12.0,19.034$ and 2.0143 is equal to $X$. The number of significant figures in $X$ is
In. Observe the following properties.
- Molar volume
II. Mass
III. Internal energy
IV. Volume
v. Enthalpy
VI. Temperature
VII. Density
The intensive properties in the above list are
229, $\mathrm{At} T(\mathrm{~K}), K_C$ value for the reaction, $\frac{1}{3} \mathrm{~N}_2(g)+\mathrm{H}_2(g) \rightleftharpoons \frac{2}{3} \mathrm{NH}_3(g)$ is 50 . The $K_C$ value for the reaction, $2 \mathrm{NH}_3(g) \rightleftharpoons \mathrm{N}_2(g)+3 \mathrm{H}_2(g)$ at the same temperature is
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