1. The shape of boron trihydride, BH3, is 2. In an exothermic reaction, the potential energy of the products is than the potential energy of the reactants. 3. A system at equilibrium always has forward and reverse reaction rates which are 4. A solution at 25°C with a pOH of 3.45 has a pH of 5. When nitric acid is titrated to an end point by lithium hydroxide, two products are and 6. The standard reduction potential table lists the Evalues of half-cell reactions measured in combination with the standard half-cell.

1. The shape of boron trihydride, BH3, is 2. In an exothermic reaction, the potential energy of the products is than the potential energy of the reactants. 3. A system at equilibrium always has forward and reverse reaction rates which are 4. A solution at 25°C with a pOH of 3.45 has a pH of 5. When nitric acid is titrated to an end point by lithium hydroxide, two products are and 6. The standard reduction potential table lists the Evalues of half-cell reactions measured in combination with the standard half-cell.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Suppose 0.125 mol of SCN-(aq) is added to a 1.00 L beaker containing an unknown concentration of Co2+(aq). These two ions react according to the following equation, with an equilibrium constant of 1.0 x 103.Co2+(aq) + 4 SCN-(aq) ⇌⇌ Co(SCN)42-(aq)If the equilibrium concentration of Co(SCN)42- is measured to be 6.3 x 10-3 mol L-1, what was the initial concentration of Co2+(aq)?
Explain about Rapid acid–base reactions? When it occurs ?
Enter your answer in the provided box. Consider the following reaction at a high temperature. Br2(g) 2Br(g) When 1.30 moles of Br2 are put in a 0.710-L flask, 1.90 percent of the Br2 undergoes dissociation. Calculate the equilibrium constant Ke for the reaction.
Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4(g) + H2O(g) 3H2(g) + CO(g). a. Write the equilibrium constant Kc for this reaction. b. How much hydrogen gas is at equilibrium if Kc = 6.3 and the remaining gases have the following concentrations: CH4 = 0.126 M; H2O = 0.242 M; CO = 0.126 M; at a temperature of 760 °C?
What is the equilibrium concentration of OH‒ ions when 25 grams of Al(OH)3 is added to 2.50 L of water? Molar Mass of Al(OH)3 = 78.00 g/mol and Ksp(Al(OH)3) = 1.3 × 10‒33
[References] The equilibrium constant (K) for the reaction PCI3 (g) + Cl2 (g) PCl; (g) equals 49 at 230°C. If 0.378 mol each of phosphorus trichloride and chlorine are added to a 6.30 L reaction vessel, what is the equilibrium composition of the mixture at 230°C? mol PC13 mol Cl2 mol PCI5
What effects does temperature have on the equilibrium constant (Keq)
TRUE OR FALSE. Write T on the space provided if the statement is true. Write F if the statement is false. _6. Catalysts only affect the rate of a reaction. -7. The rate of the forward reaction in a reversible reaction is sometimes greater than the rate of the reverse reaction. 8. Keq of a gaseous solution can be expressed in terms of Kc. 9. If an inert gas is added to a system at equilibrium, the reaction will shift to the direction of fewer molecules. _10. Pressure and volume affect a gaseous system in equilibrium in the same manner.
After equilibrium is reached in the reaction of 6.30 g H2 with 150. g I2, analysis shows that the 1.00 L flask contains 64.0 g of HI. How many moles of H2, I2, and HI are present in this equilibrium mixture? What is the Keq for this reaction?
Image attached
Help with question 3
What is the equilibrium constant, Keq, if the equilibrium concentrations are as follows: PCl5 is 1.788 M, PCl3 is 0.688 M and Cl2 is 0.549 M? PCl5(g) → PCl3(g) + Cl2(g). Round to two decimal places