At 25°C, the equilibrium constant, Kc, for the following reaction is 0.045. 2E(g) F(g) + G(g) A mixture of 0.800 moles of F and 1.200 mole of G in a 2.0-L container is allowed to come to equilibrium. What is the equilibrium concentration of E in molar? Please report 3 decimal places, without units.

The reaction below was allowed to react at 375 degrees Celcius until it formed an equilibrium. At equilibrium, the 16.2 L container was found to contain 1.9 mol SiF4, 1.1 mol H2O, 3.5 mol SiO2, and 2.9 mol HF. What is the Kc of the reaction at this temperature?  SiF4 (g) + 2H2O (g) <--> SiO2 (s) + 4HF(g)

CO2 and H, are allowed to react until an equilibrium is established as follows: CO2 (g) + H, (g)H,0 (g) + CO (g) What will be the effect on the equilibriumn of removing CO from the equilibrium mixture?

A chemical engineer is studying the following reaction: N₂(g) + 3H₂(g) → 2 NH3(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.00014. The engineer charges ("fills") three reaction vessels with nitrogen and hydrogen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B C compound N₂ H₂ NH3 N₂ H₂ NH₂ N₂ H₂ NH₂ pressure 32.70 atm 49.38 atm 23.45 atm 33.09 atm 50.55 atm 22.67 atm 33.10 atm 50.59 atm 22.64 atm expected change in pressure ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase O ↑ increase ↑ increase ↑ increase ↑ increase decrease ↓ decrease ↓ decrease ↓ decrease ↓ decrease decrease ↓ decrease decrease decrease (no change) (no change) (no change) (no change) (no change) O (no change) (no…

The formation of nitrogen monoxide from its elements has an equilibrium which favors reactants: N2 (g) + 02 (g) 2 NO (g) K, = 0.0290 at 2400°C If the initial partíal pressures of both reactant gases are 0.717 atm, what will be the equilibrium partial pressure of nitrogen monoxide? (A certain simplification is valid in solving this problem). 0.112 atm (A) (B) 0.0290 atm (C) 0.688 atm (D) 0.0563 atm (E) 0.0611 atm

The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K.H2 (g) + I2 (g) 2 HI (g)Calculate the equilibrium concentrations of reactants and product when 0.228 moles of H2 and 0.228 moles of I2 are introduced into a 1.00 L vessel at 698 K. [ H2 ] = M [ I2 ] = M [ HI ] = M

A chem ngineer is studying the following reaction: 4 HCl(g)+O,(g) – 2 H,0(g)+2Cl,(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.0040. The engineer charges ("fillsf) four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. He then measures the co mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction compound pressure expected change in pressure vessel HCl 8.71 atm Ot increase O! decrease O (no change) 02 8.13 atm O t increase OI decrease O (no change) H,0 3.63 atm Ot increase OI decrease (no change) I decrease (no change) Cl, 1.91 atm ease I decrease (no change) 7,61 atm t increase HCI I decrease O (no change) 7,86 atm O f increase 0, I decrease O (no change) 4.18 atm t increase H,0 I decrease (no change) t increase 2.46 atm Cl, I decrease O (no…

For the following reaction, K, = 0.262 at 1000°C: C(s) + 2 H2(g) = CH4(g) At equilibrium, Pa, is 1.22 atm and 1.35 g of carbon is present. What is the equilibrium partial pressure of CH4(g)? 0.390 atm 5.68 atm 0.997 atm 0.320 atm 0.624 atm None of these

A chemical engineer is studying the following reaction: H₂(g) + Cl₂(g) → 2 HCl(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.83. The engineer charges ("fills") three reaction vessels with hydrogen and chlorine, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A C compound H₂ Cl₂ HCI H₂ CL₂ HCI H₂ CL₂ HCI pressure 4.00 atm 1.97 atm 3.36 atm 4.27 atm 2.82 m 3.84 atm 1.81 atm 3.69 atm expected change in pressure 1 increase O decrease decrease Of increase Of increase Ⓒ↓ decrease Of increase O decrease decrease O1 increase Ot increase O decrease Of increase O decrease Of increase O decrease decrease Of increase O (no change) (no change) O(no change) (no change) (no change) (no change) (no change) (no…

3 A + 2 B → 1 CCalculate the equilibrium constant (K) for the following reaction at 1000. K, using this information: A and B are placed in a flask and at the beginning of the reaction [A] is 6.87 M and [B] is 6.38 M. After the reaction has reached equilibrium, [C] is 1.47 M. Unfortunately, significant figures cannot be taken into account here, so please ignorethem this time.