) Predict the effect of increasing pressure for each of the following equilibriums:
(a) 2H2O (g) + N2 (g) ↔ 2H2 (g) + 2NO (g) ________________________
(b) SiO2 (s) + 4HF (g) ↔ SiF4 (g) + 2H2O (g) ________________________
(c) CO (g) + H2 (g) ↔ C(s) + H2O (g) __
) Predict the effect of increasing pressure for each of the following equilibriums: (a) 2H2O (g)...
Predict the effect of decreasing the volume of the container for each equilibrium and why. a.) 2H2O (g) + N2 (g) <--> 2H2 (g) + 2NO (g) b.) SiO2 (s) + 4HF (g) <--> SiF4 (g) + 2H2O c.) CO (g) +H2 (g) <--> C (s) + H2O (g)
9. Which of the following will have no shift in equilibrium if the volume is decreased? 2H2O(g) + N2(g) + 2H2(g) + 2NO(g) SiO2(g) + 4HF(g) SiF4(g) + 2H2O(g) CO(g) + H2(g) C(g) + H2O(g) C6H1206(s) + 602 6CO2(g) + 6H2O(g) 10. Which of the following will shift this endothermic reaction to the REACTANT side? 302(g) 203(g) Increase the pressure Decrease the O2 gas Increase the temperature Remove the ozone, O3
Calculate delta H rxn for each of the following: (a) SiO2(s) + 4HF(g) > SiF4(g) + 2H2O(l) (b) C2H6(g) + O2(g) > CO2(g) + H2O(g) [unbalanced] 6.54 Calculate AHºrxn for each of the following: (a) SiO2(s) + 4HF(g) → SiF4(g) + 2H20(1) (b) CH6(g) + O2(g) → CO2(g) + H2O(g) [unbalanced]
Hess's Law Practice Find AH° for the following equation: SiO2(s) + 4HF(g) → SiF4(g) + 2H2O(g) Using the following equations: Si(s) + O2(g) → SiO2(s) Si(s) + 2F2(g) → SiF4(g) H2(g) + F2(g) → 2HF(g) H2(g) + 4202(g) → H2O(g) AH = -910.9 kJ/mol rxn AH = -1651 kJ/mol rxn AH = -542 kJ/mol rxn AH = -241.8 kJ/mol rxn
Determine which of the following chemical equations are correctly balanced. Fe2O3(s)+CO(g)→2Fe(s)+CO2(g) Al2S3(s)+H2O(l)→2Al(OH)3(s)+3H2S(g) 2Cr(s)+3O2(g)→Cr2O3(s) SiO2(s)+4HF(aq)→SiF4(g)+2H2O(l)
Consider the following: SiF4 (g) + 2H2O (g) < ---> SiO2 (s) + 4HF (g) Kp=7.44 x 10-3 at 2000 K a) Write the equilibrium expression b) Calculate Kc for the above reaction. Will the reaction go to the right, the left, or is it at equilibrium under the following initial conditions? [HF] = 0.100M Given the above information, calculate the value of Kp for the following reaction at 2000 K: 1/2 SiO2 (s) + 2HF (g) <- ->...
What would be the effect of increasing the temperature on each of the following systems at equilibrium? H2(g) + I2(g) ⇄ 2HI(g) + Δ PCl5(g) + Δ ⇄ PCl3(g) + Cl2(g) 2SO2(g) + O2(g) ⇄ 2SO3(g); ΔH°=-198kJ 2NOCl(g) ⇄ 2NO(g) + Cl2(g); ΔH°=75kJ C(s) + H2O(g) + Δ ⇄ CO(g) + H2(g)
QUESTION 19 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) + N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO]1/2[H2] k[NO]2[H2] k[NO] [H2)2 k[N20][H2] k[NO]2
QUESTION 9 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? k[N2O][H2] k[NO]2[H2] k[NO]2[H2]2 k[NO]1/2[H2] k[NO]2
A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? O k[no]/2[Hz] O k[N20][H2] O k[NO]2 O k[NO]2[Hz] O k[NO]2[H212