334K Z No (9) + Brz (g) = 2 No Br (9) When she introduced 0,124 moles of No (9) and 0.108 moles of Brz (g) into a 1.00 liter Container, she found equilibrum Concentration of brg (g) To be 6.47 x 10-2 M. Calculate Ke -equrlibrum Constant to same equation She introduced 190 moles of No Br (g) into a lo Liter Container She found equilibrium Concentration of Briz (s) to be 1.988 10-2 Calcolate equilibrium consteunt Ke obtained​

In this reaction n2o4(g)→2no2(g) what changes in color would you expect as pressure is increased at a constant temperature

Oxidation-reduction reactions (often called "redox" for short) are reactions that involve the transfer of electrons from one species to another. oxidation states, or oxidation numbers, allow chemists to keep track of these electron transfers. in general, one element will lose electrons (oxidation), with the result that it will increase in oxidation number, and another element will gain electrons (reduction), thereby decreasing in oxidation number. the species that is oxidized is called the reducing agent or reductant. the species that is reduced is called the oxidizing agent or oxidant. to sum up: oxidation = increase in oxidation state = loss of electrons = reducing agent reduction = decrease in oxidation state = gain of electrons = oxidizing agent part a which element is oxidized in this reaction? fe2o3+3co→2fe+3co2 enter the elemental symbol. view available hint(s) is oxidized part b which element is reduced in this reaction? 2hcl+2kmno4+3h2c2o4→6co2+2mno2+2kcl+4h2o enter the elemental symbol. view available hint(s) is reduced

Find the mass in grams of 1.37x1020 particles of h3po4