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)
a.) 2H2O (g) + N2 (g) <--> 2H2 (g) + 2NO (g)
decrease in volume shifts the equilibrium position towards that the side which has less number of moles of gas
here , in this equation :
reaction shifts left side because number of moles gases are less .
so
forms more of H2O and N2
and less H2 and NO
b.)
SiO2 (s) + 4HF (g) <--> SiF4 (g) + 2H2O (l)
here equilibrium shifts right side. so
forms more SiF4 and H2O , less SiO2 and HF
c.)
CO (g) +H2 (g) <--> C (s) + H2O (g)
here equilibrium shifts right side.
forms more C and H2O , less CO and H2
Predict the effect of decreasing the volume of the container for each equilibrium and why. a.)...
) 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) __
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]
For each of the following reactions: (a) Write the Equilibrium expression (b) Calculate the Equilibrium Constant, Kc (c) Determine the DIRECTION of the reaction (d) Determine if the reaction is in Equilibrium (e) Determine the effect of INCREASING the temperature (f) Determine the effect of increasing the concentration of ONE of the reactants. (g) Determine the effect of increasing the volume of the container. (h) Determine the effect of increasing the Pressure in the container. Reaction 1: N204(g) 2NO2(g) Reaction...
For each of the following equilibria, use Le Chatelier's principle to predict the direction of reaction when the volume is increased. Drag the appropriate chemical equations to their respective bins. chemical equations: 2H2(g)+ O2 (g) ⇌ 2H2O (g), C (s) + H2O (g) ⇌ CO (g) + H2 (g), 2Fe (s) + 3H2O (g) ⇌ Fe2O3 (s) + 3H2 (g) bins: Reaction will go toward products, Reaction will go toward reagents, Reaction will remain at equilibrium
Part A Would decreasing the volume of the container for each of the following reactions cause the equilibrium to shift in the direction of the products, the reactants, or not change? Drag the appropriate items to their respective bins. Reset Help 302(g) = 203(g) 4NH3(g) +502(g) = 4NO(g) + 6H2O(g) 2NOBr() = 2NO(g) + Br2(g) Shift in the direction of the products Shift in the direction of the reactants Equilibrium does not change
Which of the following reactions is a heterogeneous equilibrium expression? a. 2NO(g) + O2(g) 2NO2(g) b. 2NH3(g) N2(g) + 3H2(g) c. 2H2(g) + O2(g) 2H2O(g) d. 2S(s) + 302(g) 2503(g) e. C2H4(g) + H2(g) C2H6(g)
1. Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. Briefly explain your choice (6 pts) 2503(g) = 2502(g) + O2(g) (endothermic reaction) a) Oxygen gas is added. b) The pressure is increased by decreasing the volume of the reaction container. c) Sulfur trioxide gas is added. d) The temperature is decreased
Struggling with this chemistry problem. Please provide the steps you use to solve this type of problem. --For the reaction, 2NO(g)+2H2(g)→N2(g)+2H2O(g), what direction will the reaction proceed if [NO]=0.010 M, [H2]=0.31 M, [N2]=0.10 M, & [H2O]=0.25 M. (K=650) a: forward b: reverse c: the reaction is at equilibrium d: the reaction has stopped
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)