uestion 38 2HgO(s) + heat 2Hg(1) + O₂(g) AH+43.4 kcal Solid HgO, liquid Hg, and gaseous O₂ are placed in a glass bulb and are allowed to reach equilibrium at a given emperature. The mass of HgO in the bulb could be increased by (A) removing some Hg. (C) reducing the volume of the bulb. (B) removing some 02. (D) increasing the temperature.

Q3. At 298 K, F3SSF(g) decomposes partially to SF2(g). At equilibrium, the partial pressure of SF2(g) is 1.1X10-4 atm and the partial pressure of F3SSF is 0.0484 atm. (a) Write a balanced equilibrium equation to represent this reaction. (b) Compute the equilibrium constant corresponding to the equation you wrote. (c) Some SF2 (at a partial pressure of 2.3X10-4 atm) is placed in a closed container at 298 K with some F3SSF (at a partial pressure of 0.0484 atm). Enough argon is added to raise the total pressure to 1.000 atm. Calculate the initial reaction quotient for the decomposition of F3SSF to SF2.

Steam reforming of methane ( CH,) produces "synthesls gas," a mixture of carbon monoxlde gas and hydrogen gas, which Is the starting polnt for many 4 Important industrial chemical syntheses. An Industrial chemist studying this reaction fills a 2.0 L flask with 4.7 atm of methane gas and 2.3 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 4.1 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K = || Check Explanation 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessib M 9 hp Ce

For which of these reactions will there be no effect on the relative amounts of the substances present at equilibrium when the pressure of the system is increased at constant temperature? O 2 sO, (g) + 0,(g) = 2 SO, (g) + heat heat + CO, (g) + NO(g) =CO(g) + NO, (g) heat + 2 Cl, (g) + 2 H,O(g) = 4 HCI(g) + 0, (g) N, (g) + 3 H, (g) = 2 NH, (g) + heat

103 kJ + 2HBr(g) = H₂(g) + Br₂(g) A system at equilibrium contains the following pressures of gases. PHBr 107.7 atm PH₂ = 2.5 x 10-8 atm PBr₂ = 2.5 x 10-8 atm What is the equilibrium constant for the reaction at this temperature? K=[?] x 101 Coefficient (green) Exponent (yellow) Enter

For the reaction below, the thermodynamic equilibrium constant is K= 1.92x103 at 35 °C. NHẠCO2NH2(s) → 2 NH3(g) + CO2(g) Suppose that 0.0046 moles of NHẠCO2NH2, 0.0092 moles of NH3, and 0.0046 moles of CO2 are added to a 3.00 L container at 35 °C. (a) What are Q and A,G for the initial reaction mixture? Your answers must be accurate to 3 significant figures. Q = Number A,G= Number kJ mol-1 (b) Is the spontaneous reaction to the left or to the right? Click for List

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 100. L tank with 9.9 mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.50 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significan digits. K = 0

In an experiment, gaseous C2H4 and H2O, at 25 mmol each, were mixed in a 50-mL flask that contains 2.5 mmol of C2H6. (a) Determine the equilibrium constant if, at equilibrium, 16 mmol of C2H6 was present. C2H4(g) + H2O(g) ⇋ C2H6(g) + O2(g) At one point of the experiment, it was found that 9.7 mmol C2H4, 7.5 mmol H2O, 21.9 mmol C2H6 and 16.4 mmol O2 were present in the flask. (b) At what direction should the reaction proceed to achieve equilibrium? Support your answer with calculations and explain your answer in not more than 3 sentences.

Consider the reaction shown below at room temperature. 2H2(g) + S2(g) ⇋ 2H2S(g) The equilibrium constant, K, is equal to 1.1 x 107. A mixture of reactants and products at room temperature contains 0.25 M H2, 0.15 M S2, and 0.50 M H2S.  (a) Is this reaction at equilibrium? (b) In which direction does the reaction proceed to reach equilibrium? (c) Assuming the reactants remain at the same equilibrium concentrations, what would the concentration of the product have to be in order to establish equilibrium?

The equilibrium system between nitrogen gas, oxygen gas, and nitrogen dioxide gas is given N2(g) + 2O2(g)----->2N2(g) Write the balanced chemical equation for the reverse reaction. Include physical states