For gaseous state, if most probable speed is denoted by C*, average speed by C¯ and root mean square speed by C, then for a large number of molecules the ratios of these speeds are

C* = most probable speed = 2RTMC¯ = average speed = 8RTπMC = Root mean square speed or r.m.s = 3RTMC*<C¯<C C*:C¯:C=1 : 4π : 32=1:1.128:1.225

For gaseous state, if most probable speed is denoted by C*, average speed by C¯ and root mean square speed by C, then for a large number of molecules the ratios of these speeds are

C* = most probable speed = 2RTMC¯ = average speed = 8RTπMC = Root mean square speed or r.m.s = 3RTMC*<C¯<C C*:C¯:C=1 : 4π : 32=1:1.128:1.225

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For gaseous state, if most probable speed is denoted by C*, average speed by $\bar{C}$ and root mean square speed by C, then for a large number of molecules the ratios of these speeds are

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$C^{*} : \overline{C} : C = 1 : 1.225 : 1.128$

$C^{*} : \overline{C} : C = 1.128 : 1.225 : 1$

$C^{*} : \overline{C} : C = 1 : 1.128 : 1.225$

$C^{*} : \overline{C} : C = 1.225 : 1.128 : 1$

answer is C.

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C* = most probable speed = $\sqrt{\frac{2 R T}{M}}$
$\bar{C}$ = average speed = $\sqrt{\frac{8 R T}{π M}}$
C = Root mean square speed or r.m.s = $\sqrt{\frac{3 R T}{M}}$

$C * < \bar{C} < C C * : \bar{C} : C = 1 : \sqrt{\frac{4}{π}} : \sqrt{\frac{3}{2}} = 1 : 1.128 : 1.225$

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For gaseous state, if most probable speed is denoted by C*, average speed by C¯ and root mean square speed by C, then for a large number of molecules the ratios of these speeds are

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For gaseous state, if most probable speed is denoted by C*, average speed by $\bar{C}$ and root mean square speed by C, then for a large number of molecules the ratios of these speeds are