Consider the following equilibrium system. At 445 oC, Kc for the following reaction is 0.020. 2 HI (g) ⇄ H2 (g) + I2 (g) The reaction is at equilibrium. The equilibrium reaction favors the formation of more products. The equilibrium reaction favors the formation of more reactan

Consider the following reaction at equilibrium. 2CO2 (g) 2CO (g) + O2 (g) AH° = -514 kJ Le Châtelier's principle predicts that the production of CO (g) can be maximized by carrying out the reaction

When 1.00 mol of H2O and 1.00 mol of CO are introduced into an empty 1.00 L container at 960 K and allowed to come to equilibrium, the mixture contains 0.422 mol of water vapor. Write the equilibrium expression for the reaction and calculate the value of Kc

Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into 5.00 L flask. The flask is found to contain 8.62 g of CO, 2.60 g of H2, 43.0 g of CH4, and 48.4 g of H:O at 320.0 °C. What are the values of Kc and Kp for this reaction? CH:(g) + H2O(g) = CO(g) + 3 H2(g) 1 2 NEXT > Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms.

Consider the following equilibrium: N2O4(g) 2NO2 (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 2.78 atm of dinitrogen tetroxide (N204) at 710. °C. Answer the following questions about this system: rise x10 fall Under these conditions, will the pressure of N2O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO2? In other words, if you said the pressure of N2O4 will tend to rise, can that be changed to a tendency to fall by adding NO2? Similarly, if you said the pressure of N2O4 will tend to fall, can that be changed to a tendency to rise by adding NO2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm X S

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?

Heating HI(g) at 425 °C causes some of this compound to decompose, forming H2 (g) and I2 (g). Eventually, the amounts of the three species do not change further, the system has reached equilibrium. (At this point, approximately 22% of the HI has decomposed.) What is happening in this system at the molecular level? O H2(g) reacts with I2 (g) to produce HI(g) at the same rate as it decomposes. H2 (g) and I2 (g) molecules collide with HI(g) making the reaction stop. Only part of the HI(g) molecules has enough energy to decompose at this temperature. 5:55 PM FLV 2/22/2020 Type here to search hp ins prt sc delete home f12 f8 f9 f10 f5 f6 f7 14 10 num & backspace lock 23 8. 3 %24

4. Toluene, C;H8(1), is an important organic solvent. It is made industrially from methylcyclohexane, C,H14(g): C,H14(g) + heat ? 2C;H8(1) + 3H2(g) State three different changes to an equilibrium mixture of these reacting gases that would shift the reaction toward greater production of toluene. State and explain each change.

A reaction vessel initially contains 6.30 atm of A and 2.10 atm of B. A reaction occurs according to the equation:2A(g)+B(g)⇆2C(g)2A(g)+B(g)⇆2C(g)When equilibrium is reached, the total pressure is found to be 6.51 atm. What is the equilibrium constant Kp?Please enter your response to three significant figures using decimal notation.

Consider the following reaction:COCl2(g) CO(g) + Cl2(g)If 2.98×10-2 moles of COCl2, 0.206 moles of CO, and 0.304 moles of Cl2 are at equilibrium in a 17.8 L container at 672 K, the value of the equilibrium constant, Kp, is .