Consider the equation: 2NO2(g) N2O4(g). Using ONLY the information given by the equation which of the following changes would in
crease the molar concentration at equilibrium of the product N2O4(g)? increase the pressure
increase the temperature
decrease the concentration of NO2(g)
decrease the temperature
decrease the pressure
I believe the correct answer is the first option. To increase the molar concentration of the product N2O4, you should increase the pressure of the system. You cannot determine the effect of changing the temperature since we cannot tell whether it is an endothermic or an exothermic reaction. Also, decreasing the number of NO2 would not increase the product rather it would shift the equilibrium to the left forming more reactants. The only parameter we can change would be the pressure. And, since NO2 takes up more space than the product increasing the pressure would allow the reactant to collide more forming the product.
Answer is: cesium sulfide. Formula for ionic compound is: Cs₂S. Ionic compound <span>electrically </span>neutral, cesium has charge +1 (2· (+1) = +2) and sulfur has charge -2. Cesium sulfide is whide powder, soluble in water, pyrophoric in dry air, reductant.
