At 125 °C, 1 mol O2 and 2 mol H₂ in a chamber have a total pressure of 3 atm. A current is run through the chamber, combining all the molecules into H₂O at constant volume. The pressure of the chamber, in atmospheres, is now:

Here again is the balanced equation for the formation of hydrogen gas (H2(g)) that took place in the test tube when Zn(s) and HCl(aq) were combined: 2 HCl(aq) +  Zn(s)--> H2(g) + ZnCl2(aq) This enthalpy and entropy values for this reaction are Δ H = − 80.7 k J and Δ S = 0.0140 k J K. If you perform this reaction at 25.0 degrees Celsius, what is the free energy change (in kJ) for this reaction? Round your answer to three significant figures

Km.201.

Explain Enthalpy and Entropy ? Show the Difference between them ?

For a certain chemical reaction, the standard Gibbs free energy of reaction at  15.0   °C  is  147.   kJ . Calculate the equilibrium constant  K  for this reaction.Round your answer to  2  significant digits.

Determine the temperature of a reaction if K = 1.20 x 106 when AG° = +22.70 kJ/mol.

18,19 plz

In which of the following reactions is ASº expected to be negative? O L(s)I(g) O 2NH;(g) → N(g) + 3H3(g) O 2H,0(g) → 2H,(g) + O>(g) O CH;OH(g) → CH;OH(I) O AS° is not expected to be negative for any of these.

Ammonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below: N2(g) + 3H2(g) → 2NH3(g) Given that the standard free energy of formation of NH3 (g) is -104 kJ/mol at 298 K, calculate the equilibrium constant, K, at this temperature. To express an answer in exponential notation, use E to indicate the exponent. For example, 3.0 x 103 would be written, 3.0E3.

What is true about the following reaction at 25°C? H₂(g) + 2BrF(g) = 2HBr(g) + F₂(g) \Delta Hr\ deg = 115 kJ mol-¹ \Delta Sr\deg = 11.55 J mol-¹ K-¹ \Delta Gr\deg = 111 kJ mol-¹ i. The reaction is endothermic. ii. As the reaction proceeds heat is transferred from the surroundings to the system.