11. When 0.941 mol of gaseous HI is sealed in a 1.00-L flask at 225°C, it decomposes until the equilibrium amount o...
4. (10 Pts) A 1.00-L flask was filled with 2.00 mol gaseous SO, and 2.00 mol gaseous NO, and heated. After equilibrium was reached, it was found that 1.30 mol gaseous NO was present. Assume that the reaction: SO2(g) + NO2(g) =SO3(g) + NO(g) occurs under these conditions. Calculate the value of the equilibrium constant, Kc. 5. (12 Pts) At a particular temperature, Kc = 1.00 x 10 for the reaction H2(g) + 12(g) = 2 HI(g) In an experiment,...
An equilibrium mixture contains 0.950 mol HI, 0.490 mol I2, and 0.290 mol H2 in a 1.00-L flask. What is the equilibrium constant for the following reaction? 2HI(g) H2(g) + I2(g) K = How many moles of I2 must be removed in order to double the number of moles of H2 at equilibrium? mol I2
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?
A sealed 1.00 L flask is charged with 0.400 mol of A and 0.800 mol of B. At equilibrium there are 0.600 mol of C present. Using an ICE chart determine [B] in mol/L at equilibrium. A(g) + B(g) = 2 C(9) 0.250 M 0.500 M 0.100 M 0.200 M 0.300 M Next
UTOR Calculate K from Equilibrium Concentrations Some HI is placed in a sealed flask and heated to 775 K. When equilibrium is reached the flask is found to contain HII (0.137 M), H, (3.28X10M), and (23X10M) What is the value of the equilibrium constant for this reaction at 775 K? 2HI(g) H +1 K-L Submit Show Approach Show.tor Steps Try Another Version 9 item attempts Submit Answer
Calculate the concentrations of all substances present in the equilibrium mixture, if 2.35 mol of H2 and 2.35 mol of I2 are placed in a 10.0 L flask and allowed to come to equilibrium, at which time 3.76 mol of HI are present. The reaction is H2(g) + I2(g) --> 2HI (g) What is the value of Kc? What is the value of Kp?
At a certain temperature, the equilibrium constant, ?c, for this reaction is 53.3. H2(g)+I2(g)↽−−⇀2HI(g)?c=53.3 At this temperature, 0.500 mol H2 and 0.500 mol I2 were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium?
Hydrogen iodide decomposes according to the reaction 2 HI(g) = H2(g) +1268) A sealed 1.50-L container initially holds 0.00623 mol of H2, 0.00414 mol of 12, and 0.0244 mol of HI at 703 K. When equilibrium is reached, the concentration of H2(g) is 0.00467 M. What are the concentrations of HI(g) and 12(g)? 112le [HI]
Calculate the number of moles of HI that are at equilibrium with 1.42 mol of H2 and 1.42 mol of I2 in a 3.50 L flask at 450.°C. H2(g) + I2(g) equilibrium reaction arrow 2 HI(g) Kc = 65.7 at 450.°C
14. An industrial chemist introduces 1.1 atm H2 and 1.1 atm CO2 into a 1.00-L container at 25.0°C and then raises the temperature to 700.0°C, at which Keg 0.534: H2(9) + CO2(9) - H2O(g) + CO(9) How many grams of H2 are present after equilibrium is established? Submit Answer Tries 0/99