Answer to Question #173992 in General Chemistry for wrtt

Question

Activity: Adding NH4SCN Prediction: Medium Orange Solution Observation: Dark, blood red Solution

Activity:Adding AgNO3 Prediction:White Solution Observation:Opaque, Cloudy, white Colored Solution

Activity: Increasing Temperature Prediction: Dark Orange bubbling Solution Observation: Less Opaque, pale, light orangish-yellow solution

Activity:Decreasing Temperature Prediction: Pale Orange (Clear) Solution Observation: (Darker orange) Solution

Activity:Moving tube 4 to hot water Prediction: Dark Orange (Cloudy) Observation:Light yellowish-orange Solution

Activity:Moving tube 5 to ice water Prediction: Light Orange (clear ) Observation: Dark Orange Solution

Questions to answer:

• Do your observations indicate that the reaction is exothermic or endothermic? That is, based on your observations, is heat a product or a reactant? How do you know?
• What is the net ionic equation of this reaction with heat included in the equation?
• Are equilibrium shifts reversible? Justify using evidence from the lab.

Answer 1

So if the sum of the enthalpies of the reactants is greater than the products, the reaction will be exothermic. If the products side has a larger enthalpy, the reaction is endothermic.

The net ionic equation is the chemical equation that shows only those elements, compounds, and ions that are directly involved in the chemical reaction. ... As a general rule, if you balance the molecular equation properly, the net ionic equation will end up being balanced by both mass and charge.

There are several ways to stress an equilibrium. One way is to add or remove a product or a reactant in a chemical reaction at equilibrium.