Detemination of an Equilibrium Constant
1) 5.0 moles of NH3 and 5.0 moles of H2 are introdued into a 2.00 L flask. At equilibrium 1.0 moles of NH3 gas remail. Calculate Kc for this reaction.
3H2(g) + N2(g) = 2NH3(g)
2) The Kc value for the following equilibrium at 500 degrees Celcius is 49.
H2(g) + I2(g) = 2HI(g)
If 1.00 moles of H2 and 2.00 moles of I2 are introduces into a 3.00 L flask at 500 degrees celcius, how many moles of HI are present at equilibrium?
3) What would happen to the values you calculated for Kc in the experiment if the Beer's Law constant (k) value you used was low (e.g. you used 6000 M^-1 when the actual constant had a value of 10,000 M^-1) ? Explain your answer.
4) 1/2N2(g) + O2(g) = NO2(g) Kc = 1.04 x 10^-9
N2(g) + 2O2(g) = N2O4(g) Kc = 7.42 x 10^-18
Calculate Kc for each of the following.
(a) 2NO2(g) = N2(g) +2O2(g)
(b) N2(g) + 2O2(g) = N2O2(g)
(c) 2NO2(g) = N2O4(g)
Detemination of an Equilibrium Constant
1) 5.0 moles of NH3 and 5.0 moles of H2 are introdued into a 2.00 L flask. At equilibrium 1.0 moles of NH3 gas remail. Calculate Kc for this reaction.
3H2(g) + N2(g) = 2NH3(g)
2) The Kc value for the following equilibrium at 500 degrees Celcius is 49.
H2(g) + I2(g) = 2HI(g)
If 1.00 moles of H2 and 2.00 moles of I2 are introduces into a 3.00 L flask at 500 degrees celcius, how many moles of HI are present at equilibrium?
3) What would happen to the values you calculated for Kc in the experiment if the Beer's Law constant (k) value you used was low (e.g. you used 6000 M^-1 when the actual constant had a value of 10,000 M^-1) ? Explain your answer.
4) 1/2N2(g) + O2(g) = NO2(g) Kc = 1.04 x 10^-9
N2(g) + 2O2(g) = N2O4(g) Kc = 7.42 x 10^-18
Calculate Kc for each of the following.
(a) 2NO2(g) = N2(g) +2O2(g)
(b) N2(g) + 2O2(g) = N2O2(g)
(c) 2NO2(g) = N2O4(g)
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Related questions
The answers are below, I just want to know how they are found.
| 1. | Reactant A decomposes into product B according to the equation A(g) ® B(g), for which Kc = 0.156 at 400ºC. 0.550 mol of A was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of A at equilibrium. | |
| D) | 0.238 M | |
| 2. | For the nitrogen fixation reaction 3H2(g) + N2(g) ® 2NH3(g), Kc = 6.0 ´ 10â2 at 500°C. If 0.250 M H2 and 0.050 M NH3 are present at equilibrium, what is the equilibrium concentration of N2? | |
| C) | 2.7 M | |
