Thermochemistry
If you mix equimolar amounts of methane (CH4) and chlorine gas (Cl2) at room temperature without initiating combustion, which potential product's formation entails an assessment based on both kinetics and thermodynamics?
Which of the following reactions would be expected to have a positive and likely be non-spontaneous at room temperature?
In a chemical equation representing an element in its standard state, how would it appear?
Which change would NOT affect the rate of a chemical reaction already at equilibrium?
What does a negative value for the standard enthalpy of formation indicate about a compound?
Given that the standard enthalpy change for a reaction can be calculated using standard enthalpies of formation, which equation represents the most appropriate method for determining ΔH°rxn for the combustion of propane?
If the enthalpy change () for a reaction at constant pressure is negative, what type of reaction has occurred?
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When KCl dissolves into and ions in water under standard conditions, which statement correctly describes how its enthalpy change ( ) can be calculated?
In a coffee cup calorimeter experiment, if mixing two solutions results in an increase in temperature, what type of reaction has likely occurred?
How does an increase in pressure affect a gaseous reaction at equilibrium with more moles on the reactant side than product side?