What is the equilibrium equation for the reaction? SiCl4 (g) + 2 H2(g) = Si (s)...
What is the equilibrium equation for the reaction? SIC14 (8) + 2 H2(g) Si (s) + 4 HCI (8) OK [Si]+[C] [SIC]2[H2] K [51][HC14 [SiC14][H2) Kc [HC14 [H2)” [Sicla] KC [S1C14][H.] [Si] [#C?*
Consider the following reaction: SiCl4(g) ⇌ Si(s) + 2Cl2(g) The initial partial pressure of SiCl4 is 1.00 atm. At equilibrium, the total pressure is 1.35 atm. Calculate Kp for this reaction. Report your answer to the correct number of significant figures.
20.5)
Calculate ΔGo for the reaction
SiCl4(g) 2Mg(s) 2MgCl2(s) Si(s)
Substance SiCl4 Mg(s) MgCl2(s) Si(s)
ΔGof(kJ/mol) -616.98 0 -591.79 0
a)566.60kJ
b)50.38kJ
c)25.19kJ
d)- 25.19kJ
e)- 566.60kJ
Calculate Delta So for the combustion of propane. C3H8(g) + 5O2(g) rightarrow 3CO2(g)+4H2O(g) Sustance C3H8 O2 CO2 H2O So(J/k.mol) 269.9 205.138 213.74 188.825
What is the correct equilibrium constant expression for this reaction? 2HI(g) = H2(g) + 12(g) Multiple Choice Kc = [H2) (12)(HI) O Kc = [H]2/[Hz] [12] Kc = [HI] /[H2] (12) Kc = [H2] (12/(H12
What is the correct equilibrium constant expression for this reaction? 2HI(g) = H2(g) + 12(g) Multiple Choice Kc = [H2) (12)(HI) O Kc = [H]2/[Hz] [12] Kc = [HI] /[H2] (12) Kc = [H2] (12/(H12
Question 21 (4 points) What is the expression for the equilibrium constant for the following system? 2N@Cl(g) + 2NO(g) + Cl2(g) O Kc = [NO]2[C12]2/[NOCI]2 O Kc = [NO]2[C[2] / [NOCI]2 O Kc = [NO][Cl] /[NOCI] O Kc = [NO]?(C12]2/[NOCI]2 Kc = 2[NO][Cl2] / 2[NOCI] Question 20 (4 points) What is the correct equilibrium expression for the reaction? SiCl4(g) + O2(g) → SiO2(s) + 2Cl2(g) O Kc = [C12]2/[SIC14][02] Kc = 2[C12] / [SIC]4] [O2] Kc = [SiO2][Cl2] / [SiCl4]...
Use the equilibrium below to answer the following questions. H2(g) + Cl2(g) # 2 HCl(g) If the initial concentration of HCl is 0.378 M and the equilibrium constant Kc = 0.223, what is the Cl2 concentration at equilibrium? Answer to 3 decimal places and be sure to include your units. Answer: Use the equilibrium below to answer the following questions. H2(g) + Cl2(g) # 2 HCl(g) If the initial concentration of HCI is 0.378 M and the equilibrium constant Kc...
3. a) Write the equilibrium equation for the following reaction N2(g) + 3 H2(g) <-> 2 NH3(g) b) An equilibrium mixture at 500 K has the following concentrations: [N2] = 3.0 x 10-2 M [H2] = 3.7 x 10-2 M [NH3] = 1.6 x 10-2 M, calculate the equilibrium constant, Kc c) Calculate the Kp for this reaction d) Is the equilibrium mixture mostly reactants or products? e) Does this reaction go to nearly 100% completion? Explain f) If Qc...
-The equilibrium constant, Kc, for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibrium concentration of HCl when 0.452 moles of NH4Cl(s) are introduced into a 1.00 L vessel at 548 K. [HCl] = _________M -The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2(g) + I2(g) 2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.380 moles of H2and 0.380 moles of I2are introduced into a 1.00...
1) For this reaction, SiCl4 (l)+ 2H2O(g) <-> SiO2 (s) + 4HCl (g) DeltaH = -127 KJ Predict the effect increase (i), decrease(d) or no change(nc) that each change has on the QUANTITY for the equilibrium mixture. Assume that each change is applied separately to the system. Change Quantity Effect increase in pressure amount of H2O i, d or nc decrease temp amount of SiCl4 i d or nc increase temp Kc i d or nc increase temp amount of H2O...