The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO)gas as shown by the unbalanced equation given here: ?NH3(g)+?O2(g)→?NO(g)+?H2O(g) A) What volume of O2O2 at 722 mmHg and 25∘C is required to synthesize 11.0 mol of NO? B) What volume of H2O(g) is produced by the reaction under the same conditions?

The reaction of carbon monoxide(g) with water(l) to form carbon dioxide(g) and hydrogen(g) proceeds as follows: CO(g) + H2O(l)  ---> CO2(g) + H2(g) When 10.2 grams of CO(g) react with sufficient H2O(l) , 1.02 kJ of energy are absorbed .What is the value of H for the chemical equation given?

Example 3: A vessel content, one mole of carbon dioxide is heated. The carbon dioxide is dissociated 1 as: CO₂ → CO + 0₂. 2 If the equilibrium constant is given as: Kp = 30 ln(T) – 240. After equilibrium occurs, the carbon monoxide mole fraction is 0.098 find the reached temperature of the mixture.

(d) Determine the weight percentage, wt%, of the solid solution and liquid solution of a Cu-Ni alloy with a composition of 21 % Ni 79 % Cu, at a temperature of 1050 °C. Use part of the Thermal Equilibrium Diagram for Copper (Cu)-Nickel (Ni) alloy, as shown in Figure 1. Clearly show all your calculations. Temperature "C Figure 1 Part of the Cu-Ni thermal equilibrium diagram (not to scale) 1050 11 21 29 % Ni

A chemical engineer is studying the following reaction: BF 3(aq)+NH3(aq) → BF ,NH3(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.3. The engineer charges ("fills") three reaction vessels with boron trifluoride and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction expected change in concentration compound concentration vessel BE3 I decrease (no change) 0.48 M f increase NH3 I decrease (no change) 0.55 M f increase A BF,NH3 f increase I decrease (no change) 1.01 M 0.41 M f increase I decrease (no change) BF, NH3 I decrease (no change) 0.48 M f increase В BF,NH3 f increase I decrease (no change) 1.08 M BF3 I decrease (no change) 1.07 M ↑ increase NH3 I decrease (no change) 1.14 M f increase C…

Consider the chemical reaction: C(s) + H2O(g) ------>CO(g) + H2(g)How many liters of hydrogen gas are formed from the complete reaction of 15.7 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 355 K.

The high-pressure synthesis of ammonia is known as the Haber process and can be written as: 3 H2 + N2 = 2 NH3 The reaction is an equilibrium one that results in a mixture of product (NH3) and unreacted reactants (H2 and N2). The production plant includes a splitter that separates perfectly ammonia from unreacted nitrogen and hydrogen. The unreacted N2 and H2 are recycled to the reactor with additional fresh feed. The fresh feed contains N2 and H2 in the stoichiometric ratio. The extent of reaction depends on the operating conditions: at 600 K and 300 bar and when the feed to the reactor is 80 moles/hour, the moles of NH3 generated in the reactor per unit of time are 34.50 moles/hour. A schematic of the process is given below. Determine the fluxes and compositions of all streams (Total molar flow rate (mol/h), Molar flow rate H2 (mol/h), Molar flow rate N2 (mol/h), Molar flow rate NH3 (mol/h)).