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(B) Step $1$: Calculate the cell constant $(G^*)$.$G^* = \kappa 	imes R = (1.29 	imes 10^{-2} \ \Omega^{-1} cm^{-1}) 	imes (85 \ \Omega) = 1.0965 \

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$220.2$

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(B) Step $1$: Calculate the cell constant $(G^*)$.$G^* = \kappa 	imes R = (1.29 	imes 10^{-2} \ \Omega^{-1} cm^{-1}) 	imes (85 \ \Omega) = 1.0965 \ cm^{-1}$.Step $2$: Calculate the specific conductivity $(\kappa)$ of the unknown electrolyte.$\kappa = \frac{G^*}{R} = \frac{1.0965 \ cm^{-1}}{96 \ \Omega} \approx 1.142 	imes 10^{-2} \ \Omega^{-1} cm^{-1}$.Step $3$: Calculate the molar conductivity $(\Lambda_m)$.$\Lambda_m = \frac{\kappa 	imes 1000}{M} = \frac{1.142 	imes 10^{-2} \ \Omega^{-1} cm^{-1} 	imes 1000 \ cm^3 L^{-1}}{0.052 \ mol L^{-1}} \approx 219.6 \ \Omega^{-1} cm^2 mol^{-1}$.Rounding to the nearest provided option,the value is $220.2 \ \Omega^{-1} cm^2 mol^{-1}$.

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