उपसारणिक और सहखण्डज Minors and Co-Factors || Determinants 12th Maths NCERT Ch 4 L3 By Deepak Sir

Matrix of co-factors of the matrix [[1,2],[ 3, 4]] is

Write the minors and co-factors of each elements of the first column of the matrix A A=[(1,-3,2),(4,-1,2),(3,5,2)]

Find minors and co-factors of the elements of the determinant : |{:(2,-3,5),(6,0,4),(1,5,-7):}| and verify that a_(11)A_(31)+a_(12)A_(32)+a_(13)A_(33)=0

The reaction : CO(g)+3H_2(g)hArr CH_4(g) +H_2O(g) is at equilibrium at 1300 K in a one litre flask. The gaseous equilibrium mixture contains 0.30 mol of CO, 0.10 mol of H_2 and 0.020 mol of H_2O and an unknown amount of CH_4 in the flask. Determine the concentration of CH_4 in the mixture . The equilibrium consant K_c for the reaction at given temperature is 3.90

If lambda and mu are the co factors of 3 and -2 respectively in the determinant |[1,0,-2] , [3,-1,2] , [4,5,6]| then the value of lambda+mu=

The reaction, CO(g)+3H_(2)(g) hArr CH_(4)(g)+H_(2)O(g) is at equilibrium at 1300 K in a 1 L flask. It also contains 0.30 mol of CO, 0.10 mol of H_(2) and 0.02 mol of H_(2)O and an unknown amount of CH_(4) in the flask. Determine the concentration of CH_(4) in the mixture. The equilibrium constant K_(c ) for the reaction at the given temperature us 3.90 .

From the rate expression for the following reactions determines the order of reaction and the dimensions of the rate constant. a) 3NO(g) to N_(2)O(g) + NO_(2)(g) , Rate =k[NO]^(2) b) H_(2)O_(2)(aq) + 3I^(-)(aq) + 2H^(+)(aq) to 2H_(2)O(l) + I_(3)^(-) , Rate = [H_(2)O_(2)][I^(-)] c) CH_(3)CHO(g) to CH_(4)(g) + CO(g) : Rate = k[CH_(3)CHO]^(3//2) d) CHCl_(3)(g) to Cl_(4)(g) + HCl(g) : Rate = k[CHCl_(3)][Cl_(2)]^(1//2) e) C_(2)H_(5)Cl(g) to C_(2)H_(4)(g) + HCl(g) , Rate = k[C_(2)H_(5)Cl]

Write down the co-factors of the elements of the first row of the following determinant and hence evaluate the determinant |{:(1,3,-3),(2,-1,0),(4,-2,5):}|

A certain gas occupies a volume of 0.76 L at a pressure of 1.2 atm and a temperature of 4000 K. It is expanded adiabatically to a volume of 4.3 L. Determine (a) the final pressure and (b) the final temperature, assuming the gas to be an ideal gas for which gamma = 1.4.