16.37 Consider the decomposition of red mercury(II) oxide under standard state conditions: 2HgO(s, red) 2Hg()+O2(g) Above...
solid mercury (II) oxide decomposes on heating according to the equation: 2HgO(s) <--> 2Hg(g) + O2(g) The total pressure of gases at equilibrium is 5.16x10^4 Pa at 420℃, and 10.8x10^4 Pa at 450℃. Calculate the equilibrium constants at these temperatures and the molar enthalpy of decomposition of mercury (II) oxide.
In the reaction, 2HgO(s)⟶2Hg(s)+O2(g) what mass of mercury(II) oxide, HgO, would be required to produce 919 L of oxygen, O2, measured at STP?
In the reaction, 2HgO(s)⟶2Hg(s)+O2(g) what mass of mercury(II) oxide, HgO, would be required to produce 139 L of oxygen, O2, measured at STP? mass:
Lab Experiments CHM 120 6. Consider the composition of mercury (Il) oxide: 2Hg (l)+O2 (g)- 2HgO (s) When one mole of mercury reacts with one mole of oxygen, how many moles of mercury (II) oxide will form? 1oc
Consider the reaction: 2HgO(s) → 2Hg() + O2(g) Which of the following statements is correct? Mercury is reduced. All of these statements are correct. Oxygen is oxidized, Mercury(II) ion is the oxidizing agent.
A mercury mirror forms inside a test tube as a result of the thermal decomposition of mercury(II) oxide: 2HgO(s)---> 2Hg(l)+O2(g) (delta)Hrxn = 181.6KJ a) How much heat is needed to decompose 341 g of the oxide? b) If 607 kJ of heat is absorbed, how many grams of Hg form?
help asap please Question 8 (1 point) For the decomposition of mercury(II) oxide, Hgo, to mercury and oxygen: 2HgO(s) → 2Hg() + O2(g) What is the standard change in entropy for this reaction? Sº / J-mol-4K-1 HgO(s) 70.29 Hg(1) 76.02 O2(g) 205.14 351.45 J-K-1 58.83 J-K-1 O 216.60 JK-1 210.87 J-K-1 Question 7 (1 point) Which process would be predicted to have AS < 0? O a solid melting O a solution being made a solid compound decomposing to evolve...
The element oxygen was prepared by Joseph Priestley in 1774 by heating mercury(II) oxide: HgO(s) → Hg(l) + ½O2(g) ΔH° = 90.84 kJ/mol. (S values from tables) Will this be spontaneous at 600oC? What about 800oC? In each case, show appropriate calculations to support your assessment.
32. Calcula te Δ Go for the following reaction at 25°C. You will have to look up the thermodynamic data the correct units with your answer 2C:Ho(g) + 7O2(g)--4CO(g) + 6H0(,) 33. The element oxygen was prepared by Joseph Priestley in 1774 by heating mercury() oxide: Ho(r) +ソ202(g), 솨4" " 90.84 kJ/mol. Hg0(s) Estimate the temperature (in °C) at which this reaction will become spontaneous under standard state conditions 10 pts) S (Hg) 76.02 JIK mol S'(On) 205.0 J/K mol...
Substance (kJ/mol) M203 M(s) O2(g) Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. -6.10 M, 03 (S What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? Number kJ/ mol rxn What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? Number What is the equilibrium pressure of O2(g) over M(s) at 298 K? Number atm