6. Consider the following reaction C2H4(g) +H2(gCaHo (g) K 0.99 What is the concentration for each...
The reaction between ethene and hydrogen occurs according to the following stoichiometry. C2H4 (g) + H2 (g) → C2H6 (g) Which of the following statements is true? d[C2H4]/dt = +d[H2]/dt = –d[C2H6]/dt d[C2H4]/dt=–d[H2]/dt=+d[C2H6]/dt d[C2H4]/dt=+d[H2]/dt=+d[C2H6]/dt d[C2H4]/dt = –d[H2]/dt = –d[C2H6]/dt None of the above statements are true show working
For the reaction H2 (g) + I2 (g) = 2HI (g); Kc =50.0. Calculate the concentration of HI (g) at equilibrium if the initial concentration of each substance is 0.0600 M and the reaction mixture is allowed to come to equilibrium. (Hint: ICE Table)
Ethene is converted to ethane by the reaction C2H4 (9) + H2(g) - C2H6(g) C2H4 flows into a catalytic reactor at 28.6 atm and 250.ⓇC with a flow rate of 1000. L/min. Hydrogen at 28.6 atm and 250°C flows into the reactor at a flow rate of 1400. L/min. If 14.7 kg C2H6 is collected per minute, what is the percent yield of the reaction? Submit Answer Try Another Version 5 item attempts remaining
C2H2(g) + H2(g) ⇌ C2H4(g) Kp = 19.0 at T = 1273 K Suppose 0.0050 M C2H2, 0.080 M H2, and 0.90 M C2H4 are initially present in a rigid chamber at 1273 K. What is the partial pressure of each gas at equilibrium? Hint: Solve this problem using Kc instead of Kp.
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.150 M CO and 0.150 M H2O. What will be the equilibrium concentration of [CO2]? What will be the equilibrium concentration of [H2]?
Exercise 16.56 Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.135 M CO and 0.135 M H2O. Part A What will be the equilibrium concentration of [CO]? [CO] = M SubmitMy AnswersGive Up Part B What will be the equilibrium concentration of [H2O]? [H2O] = M SubmitMy AnswersGive Up Part C What will be the equilibrium concentration of [CO2]? [CO2] = M SubmitMy AnswersGive Up Part D What will be the equilibrium concentration of [H2]?...
Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) The reaction between CO and H2 is carried out at a specific temperature with initial concentrations of CO = 0.26 M and H2 = 0.52 M. At equilibrium, the concentration of CH3OH is 0.11 M. Find the equilibrium constant at this temperature
Consider this reaction at 721
K:
H2(g) + I2(g)
2HI
(g)
If we start with 1.00 Molar H 2 and 2.00 Molar
I2, what is the equilibrium concentration of HI?
Kc = 50.5 (Hint: need quadratic)
1.87 M
0.157 M
3.83 M
3.50 x 10 -4M
1.04 x 10 -3M
8.67 x 10 -6M
0.604 M
5.80
M
60) A student studied the kinetics of the reaction C2H4(g) C2H2(g) + H2(g) ? by monitoring the C2H4 concentration (in moles/L) as a function of time. The student made a plot of In[C2H4] against t. The plot was a straight line with the equation y =-0.61 8x-1 .427 (where y = In [C2H4] and x = t). What was the initial C2Ha concentration? a) 0.62 moles/L b) 4.17 moles/L c) 0.24 moles/L d) 0.78 moles/L e .62 moles/L
Changes in concentrations of product Consider the reaction H2 (g)+ 12 (g) ← → 2H1 (g) The table below summarizes the effects of a sudden concentra ts tion change on a system at equilibrium IHI (M) 1 0.07 H2 (M) 112 (M) Initial equilibrium mixture Stress (concentration of H2 is doubled) Changed concentrations Final equilibrium concentrations 0.01 0.01 +0.01 0.02 0.01 0.07 0.017 0.007 0.076 When additional H2 was added into the system, was the equilibrium disrupted? Which way did...