A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. The vessel is a stainless-steel cylinder that measures 37.0 cm wide and 44.4 cm high. The maximum safe pressure inside the vessel has been measured to be 5.00 MPa. For a certain reaction the vessel may contain up to 2.57 kg of boron trifluoride gas. Calculate the maximum safe operating temperature the engineer should recommend for this reaction. Write your answer in degrees Celsius. Be sure your answer has the correct number of significant digits. temperature: c X EEET D olo

The white powder of LiHCO3 is unstable and when heated the following reaction occurs: 2LiHCO3(s) → Li2CO3(s) + H2O(g) + CO2(g) A student performed a controlled experiment in which he heated 2.3 grams of LiHCO3 powder and collected the gases into a 1.4-liter container. At the end of the reaction the temperature in the tank was 350 ° C 1.a. Calculate how many grams of Li2CO3 were obtained at the end of the reaction. 1. b. Calculate the tank pressure at the end of the reaction. 1.c. Calculate the partial pressure of CO2 in the tank at the end of the reaction. 2. Answer the following questions for the reactants: CO2, H2O, Li2CO3, LiHCO3 a. Determine which of them has the weakest intermolecular forces. b. Determine which of the substances is a molecular substance with a constant dipole. c. Determine the systematic name for the ionic substances.

Consider the equilibrium system described by the chemical reaction below. Calculate the value of Qc for the initial set reaction conditions in a 2.00 L container: 0.0560 g H2, 4.36 g l2, and 1.32 g HI. H:(g) + lz(g) = 2 HI(g) Based on the given data, set up the expression for Qc and then evaluate it. Do not combine or simplify terms. Qc =

A sample of phosgene is sealed in a 250.0-cm³ glass bulb to which a pressure gauge is attached. The bulb is heated to 600 °C, and the gauge shows that the pressure in the bulb rises to 0.973 atm. At this temperature, the COCI₂(g) is partially dissociated into CO(g) and Cl₂(9) according to the equation CoCl₂(g) CO(g) + Cl₂(9) At 600 °C, Kp = 5.00 for this reaction. Assume that the contents of the bulb are at equilibrium and calculate the partial pressure the three different chemical species in the vessel. Pcocl₂ = Pco= Pc₂" atm atm atm

Consider the following reversible reaction at equilibrium: C6H12O6(aq) + 6 O2(g)      6 CO2(g) + 6 H2O(l). Given that this reaction is exothermic, if heat is added to the equilibrium system, how is the stress relieved?

The following system is at equilibrium in a closed vessel: 4 HCl(aq) + MnO2(s) ⇆ MnCl2(aq) + 2 Cl2(g) + 2 H2O(l) Various stresses are applied to the system as illustrated in the chart. Drag the appropriate label from the list below that indicates how the system responds to each stress. Each label can be used more than once.

While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 50 L tank with 15. mol of ethylene gas and 22. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 7.8 mol of ethylene gas and 14.8 mol of water vapor. The engineer then adds another 5.5 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. |mol

1 H,(9) + 2 NO(g) · N,O(g) + H,O(g) k1 2 H2(g) + N,0(g) → N,(9) + H,O(g) k2 Suppose also k, «k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: 2H, (g) + 2NO(g) 2H,0(g) + N, Write the experimentally- observable rate law for the overall chemical reaction. rate = k H,NO2 Note: your answer should not contain the concentrations of intermediates. any Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k1 and k-2 for = K,] 21 the reverse of the two elementary reactions in the mechanism.

Explain your reasoning, please. Thank you.