7. 4 Pts) 4.21 moles of S2Cl4 are introduced into a 2.0 L vessel. SzCla(g) 늑25C12(g)...
When she introduced 0.142 moles of NO(g) and 0.112 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.107 M. A student ran the following reaction in the laboratory at 297 K: 2NO(g)+ Br2(g)2NOBr(g) When she introduced 0.142 moles of NO(g) and 0.112 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.107 M. Calculate the equilibrium constant, Kc, she obtained for this reaction....
5 pts Question 4 A mixture of 0.75 moles of H2S. 0.40 moles of H2, and 1.25 moles of S2 are placed in a 10.0L container. Which of the following statements is true if the following reaction has a Ke value of c.40 x 108 at a temperature of 750°C? 2 H25 (8)2H2(g) + S2 (8) The reaction shifts to the right to establish equilibrium The reaction is already at equilibrium The value of K will change as the reaction...
The equilibrium constant, Kfor the following reaction is 1.55x0 at 644 When a sufficientiy large sample of HI(g) is introduced into an evacuated vessel at 644 K, the equilibrium concentration of I2)s found to be 0.303 M Calculate the concentration of HI in the equilibrium mixture. more group attempts remaining Submit Anawer Retry Entire Group Consider the following reaction where K 0.159 at 723 K. A reaction mixture was found to contain 2.07x102 moles of N2), 4.45x10-2 moles of H2)...
Sulfuryl chloride decomposes to sulfur dioxide and chlorine in a 2.0 L container SO2Cl2(g) 2 SO2(g) + Cl2(g) Ke is 0.045 at 648 K. A 0.1466 mol sample is allowed to decompose. Calculate the equilibrium concentrations of each species. (7 pts) ording to the
A student ran the following reaction in the laboratory at 686 K: H2(g) + I2(g) 2HI(g) When she introduced 0.200 moles of H2(g) and 0.230 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.18×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?
A student ran the following reaction in the laboratory at 557 K: CO(g) + Cl2(g) = COCl2(g) When she introduced 1.06 moles of CO(g) and 1.09 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of COCl2(g) to be 1.02 M. Calculate the equilibrium constant. Ko she obtained for this reaction. Ke=
When two moles of Co are introduced into a vessel containing solid sulfur, the final equilibrium pressure is 1.03 atm. Determine k_p for the reaction. S(s) + 2Co(g) leftrightarrow SO_2(g) + 2C(s)
5. (10 pts) A 1.00 L reaction vessel is filled with N204 (g) at a pressure of 0.154 atm. The gas is then allowed to decompose by the following equilibrium process N204(g) ^ 2NO2(g) a) At equilibrium, the total pressure in the container is 0.212 atm. What is the equilibriunm pressure of NO2 (g)? b) What is the Kp (numerical value) for the above equilibrium process?
The equilibrium constant, Ke, for the following reaction is 9.52x102 at 350 K: CH (g) + CCI4(g)=?CH2C\2(g) Calculate the equilibrium concentrations of reactants and product when 0.213 moles of CH4 and 0.213 moles of CCI are introduced into a 1.00 L vessel at 350 K [CH4 [CCL [CH2Ch)- Submit Answer 4 question attempts remaining MMM
Question 25 75.0 g of PCI,(g) is introduced into an evacuated 3.00 L vessel and allowed to reach equilibrium at 250°C. PCI; (g) PCI; (g) + Cl (8) If K. = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium? = 75.0 A) 2.88 atm 30.97+5(35.45 ) B) 2.27 atm = 0,360) mole C) 4.54 atm D) 7.42 atm E) 9.69 atm C HM 201/ Ghada El Zakhem Naous C= 0.360!=(0,120m N