An exothermic equilibrium reaction is heated. In which direction does the equilibrium shift?
Answer and explanation
Correct answer: B. Toward the reactants
- Step 1: Treat heat as a product of an exothermic reaction. Step 2. Adding heat shifts the equilibrium to consume it, toward the reactants. Answer: toward the reactants. Why not the others: a temperature change always shifts the equilibrium, and the mole count of gas only matters for pressure changes.
Practise more General and Organic Chemistry.
Free questions with an explanation for every one, and full timed MCAT (Medical College Admission Test) mock tests.
More General and Organic Chemistry questions
- What is the pH of a 0.01 M solution of the strong acid HCl?
- In a buffer made of a weak acid HA and its conjugate base A-, what is the pH when [A-] equals [HA]?
- A buffer contains 0.20 M of a conjugate base and 0.020 M of its weak acid, and the weak acid has a pKa of 4.76. What is the pH?
- Which element has the highest electronegativity?
- How does atomic radius change from left to right across a period of the periodic table?
- For the reaction 2 H2 + O2 gives 2 H2O, how many grams of water form from 4.0 g of H2 with excess oxygen? (H = 1.0, O = 16.0)