2 N2O(g) + O2(g) ↔ 4 NO(g)
At equilibrium, 0.196 moles of NO is present. What is the composition of the equilibrium mixture in terms of moles of each substance present?
C2H6(g) + H2(g) ↔ 2 CH4(g)
At equilibrium, it is found that 0.010 mole of H2 has reacted. What is the composition of the equilibrium mixture in terms of moles of each substance present?
a)
2N2O + O2 <----> 4NO
N2O | O2 | NO | |
Initial | 0.200 mol | 0.100 mol | 0 mol |
Change | -2x | -x | +4x |
Equilibrium | (0.200-2x) mol | (0.100-x) mol | 4x |
Now,
4x = 0.196 moles
x = 0.049 mol
At equilibrium,
[N2O] = 0.200 - 2(0.049) = 0.102 mol
[O2] = 0.100 - 0.049 = 0.051 mol
[NO] = 0.196 mol
b)
C2H6 + H2 <------> 2CH4
C2H6 | H2 | CH4 | |
Initial | 0.178 mol | 0.329 mol | 0 mol |
Change | -x | -x | +2x |
Equilibrium | (0.178-x) mol | (0.329-x) mol | 2x |
Now,
x = 0.010 mol
At equilibrium,
[C2H6] = 0.178 - 0.010 = 0.168 mol
[H2] = 0.329 - 0.010 = 0.319 mol
[CH4] = 2(0.010) = 0.020 mol
A mixture of 0.200 moles of N2O and 0.100 moles of O2 is placed in a...
A mixture of 2.5 moles of H2O and 100g of C are placed in a 50.0L container and allowed to come to equilibrium in the following reaction: C(s) +H2O(g) <-> CO(g) + H2(g) The equilibrium concentration of hydrogen gas is found to be 0.040M. What is the equilibrium concentration of the water vapour?
1- At a certain temperature, 0.820 mol of SO3 is placed in a 2.50-L container. 2SO3(g)---->2SO2(g)+O2(g) At equilibrium, 0.120 mol of O2 is present. Calculate Kc. 2- At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2(g)----->2HI(g) At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium? 3-Carbon disulfide is prepared by heating sulfur and charcoal....
A mixture of 9.22 moles of A, 10.11 moles of B, and 27.83 moles of C is placed in a one-liter container at a certain temperature. The reaction is allowed to reach equilibrium. At equilibrium the number of moles of B is 18.32. Calculate the equilibrium constant for the reaction:  A (g) + 2 B (g)<-> 3 C (g) Answer is supposed to be .0832. How? Also, how do you determine which way the reaction is going? Thanks
At 451 C, .252 moles of CH4 and .484 mole of H2O were placed in a 2.0L container. At equilibrium, the H2 concentration was .2M. what is the equilibrium constant for this reaction? CH4(g) + H2O(g) <---> 2H2(g) + CO(g) please explain each step throughly!
13. Consider the following When 0.600 moles of SO and allowed to reach equi Keq value. 13. Consider the following equilibrium: 2 SO2(g) + O2(g) +2 SO3 (8) smo ) Set up your ICE table When 0.600 moles of SO2 and 0.600 moles of O2 are placed into a 1.00-liter container and allowed to reach equilibrium, the equilibrium (SO3) becomes 0.250 M. Calculate the Keq value = (0.83 a) Set up your ICE table 0.60 Ans: ve for keq. b)...
Carbon monoxide and hydrogen react according to the following equation: CO(g) + 3H_2(g) CH_4(g) + H_2 O (g) When 1.000mol CO and 3.000 moles H_2, are placed in a 10.00-L vessel at 9271 C and allowed to come to equilibrium the mixture is found to contain 0.387 moles of H.O. What is the molar composition of the equilibrium mixture? That is how many moles of cach substancc arc present? Set up the Data Table.
How many moles of HI will be present at equilbrium if 0.6160 mol HI are placed into a 1-L flask and allowed to react at a temperature where for the following reaction takes place: 2HI(g) H2(g) + I2(g) K = 28.3 0.286 mol H2 ___ ? mol HI
How many moles of H2 and HI will be present at equilibrium if 0.8430 mol HI are placed into a 1-L flask and allowed to react at a temperature where for the following reaction takes place: 2HI(g) H2(g) + I2(g) K = 16.5 mol H2? mol HI?
26. A mixture 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr) was 0.233 M. What is the value of Kc for this reaction? COBr2(g) CO(g) + Br2(g) + 5.23 1.22 1.165 0.858 0.191 E.
Lab Exercise #2: Equilibria Problems 1.2S02e) 22S03(e) at 1500 K: If the equilibrium concentrations are [SO2] = 0.424 [ 2. We place 10.0 moles of N20 into a 2.00 L flask at 300 K. At equilibrium 2.20 moles remain. O2]-0.212 [SO3] = 0.076, find the Kc Given the following reaction, what is the Kc and the concentrations of N2 and O2? 3. Indicate whether the reaction will proceed right or left, and which concentrations will decrease or increase: 2HI(g) 근...