Write a balanced net ionic equation for the (equilibrium) formation of the tetrachloridocobaltate(ii) complex. b. based on your observations of color changes in part c, did heating the reaction mixture cause a shift in equilibrium? which direction? explain your answer based on the color changes you observed. c. is the formation of tetrachlorocobaltate(ii) complex ion exothermic or endothermic? explain your answer based on the shifts in equilibrium caused by heating and cooling the reaction mixture. d. what is the effect of an increase in temperature on the value for the equilibrium constant? (increase, decrease or no change)

The two naturally occurring isotopes of chlorine are 35cl (34.969 amu, 75.77%) and 37cl (36.966 amu, 24.23%). the two naturally occurring isotopes of bromine are 79br (78.918 rm amu, 50.69%) and 81br (80.916 amu, 49.31%). chlorine and bromine combine to form bromine monochloride, brcl. 1. how many peaks will be present in a mass spectrum for brcl? the four combinations of molecule possible given these four isotopes are: 81br37cl, 81br35cl, 79br37cl, and 79br35cl. 2. what are the masses of the four different brcl molecules? express the masses using six significant figures, in decreasing numeric order (highest to lowest), separated by commas.

What volume of a 0.0606 m solution of strontium bromide is needed to obtain 0.340 mol of the compound? question 42 options: a)5.61 l b) 3.4 l c) 600 ml d) 1 l e) 178 ml

If 2 molecules of one reactant combine with 3 molecules of another to produce 5 molecules of a product, then what is the representation of the reaction?