Mustard gas, a chemical weapon used in World War II and more recently in the Middle East hasbeen shown to have a therapeutic index that enables it to be used as an effective agent in the chemotherapy of Hodgkin’s disease. It can be generated according to the reaction: SCl₂₍g₎  + 2C₂H₄₍g₎ ⇋ S(CH₂CH₂Cl)₂₍g₎ An evacuated 2.5-liter flask at 20.0°C is filled with 0.129 mol of SCl2 and 0.296 mol C2H4. After equilibrium is established, 0.01745 mol mustard gas is present. What is the partial pressure of each gas at equilibrium? What is the equilibrium constant K at 20.0oC?

Suppose you have 1.25 moles of gaseous napthalene (C10H8) at T = 292 K. What is the average kinetic energy of one molecule of napthalene? (The molar mass of napthalene is 128 g/mol. You may assume that the gas molecules behave ideally.)

A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.

Ammonia is among the top ten synthesized compounds. Its many uses include the manufacture of ammonium nitrate and other fertilizers. Ammonia decomposes at high temperatures. In an experiment to explore this behavior, 2.00 moles of gaseous NH3 are sealed in a rigid 1-liter vessel. The vessel is heated at 800 K and some of the NH3 decomposes in the following reaction:2NH3​(g)<-->N2​(g)+3H2​(g)   The system eventually reaches equilibrium and is found to contain 1.74 mole of NH3. What is the value of KC for the decomposition reaction at 800 K? What is the value of KP for the decomposition reaction at 800 K?

A 1.00 LL flask is filled with 1.20 gg of argon at 25 ∘C∘C. A sample of ethane vapor is added to the same flask until the total pressure is 1.350 atmatm . part A: What is the partial pressure of argon, PArPAr Part B: What is the partial pressure of ethane, PethanePethane

7. When detern ing the mass of a liquid, ras in a hurry and did not allow enough time for the temperature of the flask to reach the temperature of the boiling water bath. The student recorded the temperature of the gas as 100.0°C when it was only 80.0°C, Is the molar mass calculated by the student higher or lower than the accepted molar mass, or does this error have no effect on the calculated result? Briefly explain your answer # 2/HB Office DEPOTS b) If the student assumed the volume of the flask was 125 mL (as marked by the side of the flask) rather than measuring the volume experimentally, would the unknown's calculated molar mass be too high, too low, or unaffected? Explain. # 2/HB 4

What is kinetic energy of one mole of an ideal gas st 25C?