A 65.0  g piece of gold at 650  K is dropped into 162  g of  H2O(l)  at 298  K  in an insulated container at 1  bar  pressure.  CP,m  for  Au  and  H2O at 298  K  are 25.4 and 75.3  J⋅K−1⋅mol−1, respectively. Calculate the temperature of the system once equilibrium has been reached. Assume that CP,m for Au and H2O are constant at their values for 298 K throughout the temperature range of interest.

For a certain chemical reaction, the standard Gibbs free energy of reaction at 30.0°C is 73.3 kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits.

he decomposition of a generic diatomic element in its standard state is represented by the equation   12X2(g)⟶X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.20 kJ·mol−1 at 2000. K and −53.38 kJ·mol−1 at 3000. K. Determine the value of the thermodynamic equilibrium constant, ?, at each temperature. At 2000. K, Δ?f=4.20 kJ·mol−1. What is ? at that temperature? ? at 2000. K=     At 3000. K, Δ?f=−53.38 kJ·mol−1. What is K at that temperature? ? at 3000. K=

For a certain chemical reaction, the standard Gibbs free energy of reaction is - 104. kJ. Calculate the temperature at which the equilibrium constant K = 7.1 × 10¹8. Round your answer to the nearest degree. T = °C X S

For the reaction X(g)+3Y(g)⇌3Z(g) Kp = 1.95\times 10−2 at a temperature of 81 ∘C . Calculate the value of Kc .

For a certain chemical reaction, the standard Gibbs free energy of reaction is  129.   kJ . Calculate the temperature at which the equilibrium constant K   =   ×6.010−25 .Round your answer to the nearest degree.

For a certain chemical reaction, the equilibrium constant K = 2.8 × 104 at 5.00 °C. Calculate the standard Gibbs free energy of reaction. Round your answer to 2 significant digits. AG° = kJ x10 X Ś

Calculate the value of Kp for the equation C(s) + CO,(g) = 2 CO(g) Kp = ? given that at a certain temperature C(s) + 2 H,O(g) = CO,(g) + 2 H,(g) Ки — 3.15 H,(g) + CO,(g) H,0(g)+CO(g) Kp2 = 0.747 Kp =

Consider the reaction in the Haber process 3H2 (g) + N2 (g) → 2NH3 (g)where delta H° = -91.8 kJ/mol and delta S° = -197 J/(mol*K). What is the value of the equilibrium constant (K) at a temperature of 125°C?

For a certain chemical reaction, the standard Gibbs free energy of reaction is - 149. kJ. Calculate the temperature at which the equilibrium constant K = 1.3 × 1026. Round your answer to the nearest degree. T=