The equilibrium constant, K, for the following reaction is 5.10×10-6 at 548 K. NH,CI(s) NH3(g) + HCl(g) Calculate the equilibrium concentration of HCI when 0.265 moles of NH,Cl(s) are introduced into a 1.00 L vessel at 548 K. [HCI] = M

excel spreadsheet

Use this balanced equation to solve the following problem: NazCO3 (5) + 2 HCI (ag) - H20 () + CO2 (g) + 2 NaCl (ag) 6.91 grams of sodium carbonate are added to 0.053 moles of hydrochloric acid. How many grams of carbon dioxide will be produced? What is the limiting reactant? (you should select 2 answers) O hydrochloric acid is limiting O sodium carbonate is limiting both reactants are limiting O there is no limiting reactant O 1.17 g carbon dioxide O 2.33 g carbon dioxide O 2.87 g carbon dioxide O 5.74 g carbon dioxide O 1.01 g carbon dioxide O 0.37 g carbon dioxide O 0.41 g carbon dioxide

A solution containing sodium fluoride is mixed with a solution containing cadmium nitrate to form a solution that is 0.0050 M in NaF and O.00250 M in Cd(NO3)2. If the Ksp for CDF2 is 6.44x10-3, then Q > K and a precipitate of CDF2 will form. O Q < K and more CDF2 will precipitate since the solution is not supersaturated. O Q < K and CdF2 does not precipitate. Q = K and the system is at equilibrium.

8.2 L of chlorine gas at 298 K and 3.0 atm is added to a rigid 4.0 L reaction vessel containing 3.2 moles of He gas and 2.4 moles of fluorine gas?  Chlorine and Fluorine gas react according to the following reaction at 298 K.                                                               Cl2 (g)    +    3 F2  (g)    à 2 ClF3 (g)               What is the partial pressure of ClF3 after the reaction is complete?                If the reaction proceeded with a percent yield of 40%, what would be the partial pressure of ClF3?

A batch process is operated with the following sequence. The feed to the batch process consists of a solution of 500 L of ethanol with 120 mole of A and 120 mole of B. If the temperature of the solution is sufficient, A and B will react to form P (the desired product): A (eth) + B (eth) → P (s) DHreact  = − 250 kJ/mol (1)  product P is sparingly soluble in ethanol, which helps facilitate its removal from the reaction solution. It can be assumed that the reaction rate is first-order in both the concentration of A (cA ) and B (cB ), and so second-order overall: -r A = k c A cB  (2) The batch process consists of the following FOUR steps: Initially, the tank is empty. 1. Fill tank with solution (ethanol/A/B). 50°C (1 hour) Increase temperature of the feed from 20°C to 2. Reaction takes place isothermally at 50°C (4 hours, to give conversion of 50%) 3. Filtration of reaction solution to give product P (2 hours) 4. Drying with hot nitrogen gas followed by the removal of powder product (3…

For the following reaction, 20.4 grams of chlorine gas are allowed to react with 4.21 grams of water . chlorine(g) + water(1) hydrochloric acid(aq) + chloric acid (HCIO3)(aq) What is the maximum amount of hydrochloric acid that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams

Nitromethane, CH3NO2 , can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is mainlyCH3NO2(l) + O2(g) → CO2(g) + N2(g) + H2O(g)a. The standard enthalpy change of reaction (ΔH°van ) for the balanced reaction (with lowest whole-number coefficients) is −1288.5 kJ. Calculate ΔHf0 for nitromethane.b. A 15.0-L flask containing a sample of nitromethane is filled with O2 and the flask is heated to 100.°C. At this temperature, and after the reaction is complete, the total pressure of all the gases inside the flask is 950. torr. If the mole fraction of nitrogen (χnitrogen) is 0.134 after the reaction is complete, what mass of nitrogen was produced?

4) Given the same concentrations, the reaction CO(g) + Cl2(g)→ COCI2(g) at 250°C is 1.50 x 10° times as fast as the same reaction at 150°C. Calculate the energy of activation (as kJ/mol) for this reaction. Assume that the frequency factor is constant. (R: 8.314 J/mol.K)

From the standard enthalpy of formation of atomic hydrogen (h). from the standard enthalpies of formation, calculate the delta H rxn for the reaction. C6H12(l) + 9O2(g) = 6CO2(g) + 6H2O(l) For C6H12(l), delta H degrees farenheight= -151.9 kJ/mol