According to the balanced chemical equation 5 H_2C_2O_4(aq) + 6H^+(aq) rightarro

Question

According to the balanced chemical equation 5 H_2C_2O_4(aq) + 6H^+(aq) rightarrow 10 CO_2(g) + 2 Mn^2+(aq) + 8 H_2O(l) 0.3500 grams of oxalic acid, H_2C_2O_4 will react with moles of permanganate, MnO_4-. 0.001554 0.003887 0.00774 0.009718 What are the possible values of l if n = 5? 5 0,1, 2, 3,or 4 -4,-3,-2,-1,0,+1,+2,+3, or +4 -5 -4,-3,-2,-1,0,+1,+2,+3,+4 or +5 The electronegativity for both sulfur and carbon is 2.5. Therefore the compound CS_2 would be expected to be ionic with C as the anion. be ionic with C as the cation. have nonpolar covalent bonds between C and S have polar covalent bonds between C and S Based on the indicated electronegativities, arrange the following in order of increasing ionic character (from left to right): CsBr, LaBr_3, PBr_3, MgBr_2. CsBr

Explanation / Answer

Dear Student,

36. Given:

5H2C2O4(aq) + 2MnO4(aq) + 6H+(aq) -----> 10CO2(g) + 2Mn2+(aq) + 6H2O(l)

Solution:

Molecular weight of oxalic acid is 90

5 x 90 gr oxalic acid react with 2 mole permanganate, then
0.35 gr oxalic acid react with X mole permanganate

Therefore, 5 x 90 x X = 2 x 0.35

Mole of permanganate = ( 2 x 0.35 ) / (5 x 90 )

Mole of permanganate = 0.7 / 450

Mole of permanganate = 0.00155 moles.

Therefore, option is A = 0.001554.

37. The Orbital Angular Momentum Quantum Number ( l )

The possible values of l If n = 5 are as follows:

Since it can be zero or a positive integer less than (n-1), it can have a value of 0, 1, 2, 3, 4.

Therefore, option is B = 0,1,2,3 or 4.

38. The electronegativity for both sulfur and carbon is 2.5. Therefore the compound CS2 would be expected to have non-polar covalent

Explanation:

In the carbon disulfide case, both sulfur and carbon have the same electronegativity values 2.5. The bond electrons are equally shared and there is no dipole moment on any of the carbon sulfur bonds. Generally, dipole moments are vector quantities and from VSEPR theory, the carbon disulfide molecule is linear and the dipole moments if there were any, would be acting in opposite directions. They would be equal magnitude wise, therefore they would cancel out and there will be no resultant dipole i.e. no net dipole moment. However the bonds are non-polar to start with and the molecule therefore is non-polar.

Therefore, option is C.

39. Based on the indicated electronegativities, the following is in the order of increasing ionic character:

PBr3 > MgBr2 > LaBr3 > CsBr

Therefore, option is D.

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