A mixture of 1.00 mol NaHCO3(s) and 1.00 mol Na2CO3(s) is introduced into a 2.50 L flask in which the partial presure of CO2 is 2.10 atm and that of H2O (g) is 715 mmHg. When equilibrium is established at 100°C, will the partial pressures of CO2(g) and H2O(g) be greater or less than their initial partial pressures? Explain 2NaHCO3(s)=Na2CO3(s)+CO2(g)+H2O(g) Kp=0.23 at 100 °C

A mixture of 0.471 M H₂O, 0.431 M Cl₂O, and 0.675 M HClO are enclosed in a vessel at 25 °C. H₂O(g) + Cl₂O(g) = 2 HOCI(g) K = 0.0900 at 25°C Calculate the equilibrium concentrations of each gas at 25 °C. [H₂O]= [C!,O]= [HOCI]= MacBook Pro Search or type URL 00 8 A -0 < M M + 11 M del

A mixture of 0.06529 mol of CH4, 0.04045 mol of H2S, 0.06585 mol of CS2, and 0.03325 mol of H2 is placed in a 1.0-L steel pressure vessel at 1304 K. The following equilibrium is established: 1 CH4(g) + 2 H2S(g)  1 CS2(g) + 4 H2(g) At equilibrium 0.01420 mol of H2 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2.Peq(CH4) = ______  .Peq(H2S) =  ______ .Peq(CS2) = ______  .Peq(H2) = _______  .(b) Calculate KP for this reaction.KP = _______  .

Phosphorus pentachloride decomposes according to the chemical equation: PCI (g) = PCI₂(g) + Cl₂(g) Kc = 1.80 at 250.0 °C A 55.0 gram sample of PCI (g) is injected into an empty 5.00-liter reaction vessel held at 250.0 °C. Calculate the pressure, in atm, of the vessel when equilibrium is reached.

A student ran the following reaction in the laboratory at 479 K: PCI3(g) + Cl₂(g) =PC15(g) When she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of PCI3 was 2.13 atm and the initial partial pressure of Cl₂ was 1.34 atm, she found that the equilibrium partial pressure of PCI5 was 1.12 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp Submit Answer Retry Entire Group 8 more group attempts remaining

A mixture of 0.009482 mol of CH4, 0.02708 mol of H2S, 0.02785 mol of CS2, and 0.02860 mol of H2 is placed in a 1.0-L steel pressure vessel at 3918 K. The following equilibrium is established: 1 CH4(g) + 2 H2S(g)  1 CS2(g) + 4 H2(g) At equilibrium 0.001533 mol of CH4 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2.Peq(CH4).Peq(H2S).Peq(CS2).Peq(H2).(b) Calculate KP for this reaction.KP.

please indiciate whether the pressure will decrease, increase, or not change. Also please indicate what the shift in equilibrium will be

The equilibrium constant Kc for the reaction,I2(g) + Br2(g) <-----> 2 IBr(g) is 26 at 425 K. What is the value of Kc for the equilibrium,1/2 I2(g) + 1/2 Br2(g) <-----> IBr(g) at 425 K?

A student ran the following reaction in the laboratory at 588 K: CO(g) + Cl₂(g) —COCI₂(g) When she introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 1.74 atm and the initial partial pressure of Cl2 was 0.951 atm, she found that the equilibrium partial pressure of COCI₂ was 0.685 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр =

Assume that the change in concentration of COCl2 is small enough to be neglected in the following problem. Use an ICE table with the "x is small" approximation. The results might surprise you. You can trust them if you verify the assumption. (a) Calculate the equilibrium concentration of all species in an equilibrium mixture that results from the decomposition of COCl2 with an initial concentration of 0.3166 M. COCl2(g) ⇌ CO(g) + Cl2(g)       Kc=2.200 × 10−10 Enter the equilibrium molar concentration of COCl2 below, with 4 sig figs