1. Determine the state of each chemical species and obtain its chemical equilibrium equation: Al3 +...
Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after a decrease in pressure or volume. If there is no change in the concentration of the species, leave the box blank. CH 4 ( g ) + 2 H 2 S ( g ) − ⇀ ↽ − CS 2 ( g ) + 4 H 2 ( g ) after decreasing the pressure after decreasing the volume of the reaction vessel
Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after increasing the pressure. $$ \mathbf{N}_{2}(g)+3 \mathbf{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) $$
2. For each of the following species, write a balanced chemical equation for its reaction with warden and calculate K. or ki for its conjugate acid or base from the information given. (a) CO32-, ks = 1.8 x 10-4 (b) NH2OH (hydroxylamine), ks = 1.1 x 10-8 (c) CsHsNH(pyridinium), K. = 5.88 x 10-6 3. Calculate [OH-], [H], por, and pH of a 0.0020 M Ba(OH)2 solution at 25 °C.
what is the overall balanced chemical equation? Al → Al3+ O2 → 2 O2-
Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after a decrease in pressure or volume.
Core Chemistry Skill: Balancing a Chemical Equation 1 of 16 Balance the chemical equation by indicating the number of each species in the appropriate blanks For this exercise, indicate coefficients of 1 explicit Match the numbers in the left column to the appropriate blanks in the chemical equations on the right. Make certain the chemical equation is complete before submitting your answer. View Available Hint(s) Reset Help Fe (s) + H20 (1) ► Fe, O. (s)+ Core Chemistry Skill: Balancing...
Al(OH)3 + 3 H+ <--> Al3+ + 3 H2O You find that the solution pH = 5, and that [Al3+] = 10-2 mol/L. Assuming the activity coefficient = 1 for Al3+, what is the log(Keq) of the Al(OH)3 dissolution written above assuming the system is at equilibrium? If you got stuck on a, assume that log(Al3+)=log(Keq)-3pH + 30.
Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after reactant or product is added. Click in each box to toggle in the relative change in concentration (up = increases, down = decreases, leave the box blank for no charge). 2CO(g) + O_2(g) rlhar 2CO_2(g) a) after increasing the concentration of CO b) after increasing the concentration of CO_2
Al(OH)3(s) → Al3+(aq) + 3OH−(aq) ΔfH∘/kJ⋅mol−1 −1284 −538.4 −230.02 S∘/J⋅mol−1⋅K−1 85.4 −325 -10.9 Part A Compute ΔrS (answer in J⋅mol−1⋅K−1) Part B Compute ΔrG∘ at 298 K (answer in kJ⋅mol−1) Part C Determine the equilibrium constant for the dissolution of Al(OH)3 at 298 K. Part D Determine the Gibbs energy change for the dissolution of Al(OH)3 when the concentrations of Al3+ and OH− are both 2.60×10−7mol⋅L−1.(answer in kJ⋅mol−1) Part E At what temperature will Al(OH)3(s) be at equilibrium with...
Exp 7_C Post-Lab Chemical Equilibrium (10 pts/show all work) Determine if the following salts will be acidic, basic, or neutral. For each salt show the 1. balanced equation for ionization in H20 and Example: NaNO2(aq)> Na (aq)+ NO2 (aq) 2. how the ion products form which determine pH by producing OH or H30 Example: NO2(aq) +H20(1) <>HNO2(aq)+ OH (aq) If the salt is neutral give a brief explanation. a) LiF b) BaBr2 c) NHa d) CaSO3 ?) ???.