A gas mixture contains 14.8 mol of Br2 and 66.5 mol of F2.(a) Compute the mole fraction of Br2 in the mixture.XBr2 = (b) The mixture is then heated, and the Br2 starts to react with the F2 to give BrF5: Br2(g) + 5F2(g) -> 2BrF5(g) At a certain point in the reaction, 7.70 mol of BrF5 is present. Determine the mole fraction of Br2 in the new mixture. XBr2 =

4. At 5°C and 1 atm, x L of O2 gas is required to react with 0.51 g of glucose, what is the value of x? The unbalanced reaction is shown below: C6H12O6 (s) + O2(g) → CO2(g) + H2O(l)

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?