`6 xx 10^(-3)` mole `K_2 Cr_2 O_7` reacts completely with `9 xx 10^(-3)` mole `X^(n+)` to given `XO_3^- and Cr^(3+)`. The value of `n` is :

A solution containing 2.68 xx 10^(-3) mol of A^(n+) ions requires 1.61xx10^(-3) mol of MnO_(4)^(-) for the complete oxidation of A^(n+) " to "AO_3^(-) in acidic medium. What is the value of n ?

An element A in a compound AB has oxidation number -n. IT is oxidized by Cr_(2)O_(7)^(2-) in acid medium. In the experiment 1.68xx10^(-3) moles of K_(2)Cr_(2)O_(7) was used for 3.36xx10^(-3) moles of AB. The new oxidation number of A after oxidation is

If m = 3 and n = 2 find the value of 9m^2 - 10n^3

M(OH)_x " has " a K_(sp) " of " 4 xx 10 ^(-9) and its solubility is 10^(-3) M. The value of x is :

Number of moles of K_(2)Cr_(2)O_(7) reduced by one mole of Sn^(2+) ions is

A mixture of H_(2), N_(2) and NH_(3) with molar concentration 5.0xx10^(-3) "mol" L^(-1), 4.0xx10^(-3) "mol" L^(-1) and 2.0xx10^(-3) "mol" L^(-1) respectively was prepared and heated to 500K . The value of K_(c) for the reaction: 3H_(2)(g)+N_(2)(g)hArr2NH_(3)(g) at this temperature is 60. Predict whether ammonia tends to form or decompose at this stage of concenration.

When 5.141 xx 10^(-4) Kg of anthracene is dissolved in 3.5 xx 10^(-3) Kg of chloroform the BP of CHCl_3 is found to be increased by 0.325K. Find the molecular weight of Anthracene. [ K_b = 3.9 "K.Kg mole"^(-1) ]