Fuel engineers use the extent of the change from CO and H2O to CO2 and H2 to regulate the proportions of synthetic fuel mixtures. If 0.250 mol of CO and 0.250 mol of H20 are placed in a 125-mL flask at 900K, what is the composition of the equilibrium mixture? At this temperature, Kc is 1.56 for the equation CO(g) + H20(g) = CO2(g) + H2(g)

SO₂ reacts with Cl₂ to form SO₂Cl₂. The equilibrium constant, Kp, for this reaction is 0.417 at 373 K. 4 SO₂(g) + Cl₂(g) =SO₂Cl₂(g) The standard enthalpy change for this reaction (AH°) is -67.2 kJ/mol. (a) Predict the effect on the production of SO₂Cl₂ when the temperature of the equilibrium system is increased. (b) Use the van't Hoff equation to estimate the equilibrium constant for this reaction at 449 K. Kat 449 K =

Consider the following reaction:             2HF(g) ⟷H2(g) + F2(g) (K = 1.00 x10-2) Given 1.00 mole of HF(g), 0.500 mole of H2(g), and 0.750 mole of F2(g) are mixed in a 5.00-L flask, determine the reaction quotient, Q, and the net direction to achieve equilibrium.

The equilibrium system shown below was analyzed and the concentrations of H2(g), I2(g) and HI(g), were found, in mol/L, to be 4.2, 3.8, 1.6 respectively. The equilibrium constant must be? H2(g) + I2(g) <=====> 2HI(g) + 65 kJ

When 0.200 mol of CaCO,(s) and 0.300 mol of CaO(s) are placed in an evacuated, sealed 10.0-L container and heated to 385 K, PCO, = 0.220 atm after equilibrium is established. 2 CACO,(s) = CaO(s) + CO,(g) Additional CO,(g) is pumped into the container to raise the pressure to 0.470 atm. After equilibrium is re-established, what is the total mass (in g) of CaCO, in the container?

Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)

An experimenter places the following concentrations of gases in a closed container: NOBI]=0.245 M, [NO] = 3.29 x 10 M, Br2] = 2.02 x 10- M These %3D gases then react: 2NOB1(g) 2NO(g) + Br2 (g) 4. At the temperature of the reaction, the equilibrium constant K, is 5.85 x 10 * Calculate the reaction quotient, Q, from the initial concentrations and determine whether the concentration of NOBR increases or decreases as the reaction approaches equilibrium. Q.= %D The concentration of NOBR

In a particular experiment 1.0 mole of H2O (g) and 1.0 mole of CO (g) are put into a flask and heated to 350 oC.  In another experiment 1.0 mol of H2 (g) and 1.0 mole of CO2 (g) are put into a different flask with the same volume as the first.  This mixture is also heated to 350 oC.  After equilibrium is reached, will there be any difference in the composition of the mixture in the two flasks?

A student ran the following reaction in the laboratory at 588 K: CO(g) + Cl₂(g) —COCI₂(g) When she introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 1.74 atm and the initial partial pressure of Cl2 was 0.951 atm, she found that the equilibrium partial pressure of COCI₂ was 0.685 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр =

Consider the following equilibrium: 2NO(g) + Cl₂ (g) 2NOCI (g) AG=-41. kJ Now suppose a reaction vessel is filled with 1.55 atm of chlorine (C1₂). about this system: T Under these conditions, will the pressure of NOCI tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOC1 will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if said the pressure of NOCI will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. and 4.77 atm of nitrosyl chloride (NOCI) at 683. °C. Answer the following questions Orise Ofall yes Ono atm O x10 X S