H2 and F2 react according to the following equation, forming HF. H2(g) + F2(g) 2HF(g); H° = –271 kJ If H2(g) and F2(g) were mixed in a thermally insulated vessel, the reaction that occurred would be a.
The equation for fermentation of glucose to alcohol and carbon dioxide is C6H12O6= 2C2H5OH + 2CO2 The enthalpy for the reaction is -67kj. Is the reaction endothermic or exothermic? Is the heat energy absorbed or released as the
Method for getting correct answer? Thank you! The reaction below is an endothermic reaction. What would one have to do to shift the equilibrium to the right? SO2Cl2(g)↔SO2(g) + Cl2(g) a. Decrease the temperature b. Increase
Could someone explain the reasoning for this? 6) Which of the following is a false statement about ALL reactions in equilibrium? a) Increasing temperature shifts the reaction toward the products in an endothermic reaction b)
I think I made a mistake with my previous question. I have two solutions potassium thiocyanate (KSCN) and iron (III) chloride (FeCl3). The reaction is Fe+++(aq) + SCN-(aq) <--> FeSCN++(aq) What will happen if the solution is
In an endothermic reaction at equilibrium, what is the effect of raising the temperature? The reaction makes more products the reaction makes more reactants*** the reaction is unchanged the answer cannot be determined
HCl (aq) + NaOH (aq) -> NaCl (aq) + H2O (l) Will the neutralisation reaction be endothermic or exothermic? Hint: think about the net ionic equation. So, taking the hint, I got: OH- + H+ -> H2O Not sure how that helps, and
Refer to the net ionic equation below to answer the following questions: Co(H2O)6^+2 + 4Cl- <==> CoCl^-2 + 6H2O 1. In what direction was the equilibrium shifted by: a. Addition of HCl b. Addition of water c. Addition of