3. Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to the following equation: 2NF3(g) = N(g)+ 3F2(g) When 2.54 mol of NF; is placed in a 6.00-L container and allowed to come to equilibrium at 800 K, the mixture is found to contain 0.0434 molof N. What is the value of K, at this temperature? (R = 0.0821 L atm - mol - K') a. 1.54 x 10 %3D b. 1.91 × 10 c. 1.78 x 10* d. 1.59 x 10 e. 4.43 x 10

Phosphorus pentachloride decomposes according to the chemical equation PC15(g) PC13(g) + Cl₂(g) Kc = 1.80 at 250 °C A 0.1584 mol sample of PC1, (g) is injected into an empty 2.00 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PC13 (g) at equilibrium.

For the chemical equation: SO2(g) + NO2(g) SO3(g) + NO(g) The equilibrium constant at a certain temperature is 8.80. At this temperature, calculate the number of moles of NO2(g) that must be added to 6.20 mol SO2(g) in order to form 4.40 mol SO3(g) at equilibrium.

Consider the following reaction: 2NH3(g) N₂(g) + 3H₂(g) If 1.54x10-3 moles of NH3(g), 0.549 moles of N₂, and 0.352 moles of H₂ are at equilibrium in a 19.7 L container at 792 K, the value of the equilibrium constant, K, is

For the chemical equation 2SO2(g) + NO2(g) 2SO3(g) + NO(g) The equilibrium constant at a certain temperature is 5.50. At this temperature, calculate the number of moles of NO2(g) that must be added to 1.20 mol SO2(g) in order to form 0.80 mol SO3(g) at equilibrium.

Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant k for the following reaction is 9.84 x 101: N,(g) + 0,(g) = 2 NO(g) Use this information to complete the following table. Suppose a 30. L reaction vessel is filled with 0.64 mol of N2 and There will be very little N, and O2. alo 0.64 mol of 0,. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K 2 NO(g) N3(9)+Og(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K = 3 N,(9)+30,(9) 6 NO(g)

A student adds 0.600 mol of methane gas, CH4(g) into a 2.00 L container and the methane forms ethyne, C2H2(g) and hydrogen gas, H2(g). At equilibrium, the container was found to contain 0.045 mol/L C2H2.a) Calculate the initial concentration of CH4. Then complete an ICE Table to organize the initial, change and equilibrium concentrations for this equilibrium system. Show any calculations needed. 2CH4(g) ⇄ C2H2(g) + 3H2(g)b) Calculate the equilibrium constant, Keq, for this equilibrium. Show all work.c) What is the equilibrium concentration of H2(g) ?

Carbon disulfide and chlorine react according to the following equation: CS2(g) + 3Ch(g) =S,Cl½(g) + CC1,(g) When 1.14 mol of CS, and 4.80 mol of Clh are placed in a 2.00-L container and allowed to come to equilibrium, the mixture is found to contain 0.650 mol of CC14. How many moles of Cl are present at on equilibrium? Select one: O a. 0.490 mol O b. 2.85 mol O c. 3.50 mol O d. 0.650 mol O e. 1.43 mol e to search F3 F4 F5 F6 FZ FB F9 F10 F11 F12 Prise %24 E R T G H K B N M 立

For the chemical equation SO, (g) + NO, (g) = So, (g) + NO(g) the equilibrium constant at a certain temperature is 2.70. At this temperature, calculate the number of moles of NO, (g) that must be added to 2.75 mol SO,(g) in order to form 1.10 mol SO, (g) at equilibrium. moles of NO,(g): mol

At a certain temperature, 0.3811 mol of N₂ and 1.761 mol of H₂ are placed in a 4.50 L container according to the following equation: N₂(g) + 3H₂(g) + 2NH3(g) At equilibrium, 0.1001mol of N2 is present. Calculate the equilibrium constant.