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A mixture of oxygen and hydrogen is analyzed by passing it over hot copper oxide and through a drying tube. Hydrogen reduces the CuO according to the reaction
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Thermodynamics, Statistical Thermodynamics, & Kinetics
- What possible uses exist for the natural gas liquids that are removed from natural gas during its processing?arrow_forwardHow does hydraulic fracturing differ from previously used techniques for the recovery of natural gas from the earth?arrow_forwardUse the appropriate tables to calculate H for (a) the reaction between copper(II) oxide and carbon monoxide to give copper metal and carbon dioxide. (b) the decomposition of one mole of methyl alcohol (CH3OH) to methane and oxygen gases.arrow_forward
- Mass of copper before electrolysis 5.621 g Mass of copper after electrolysis 5.487 g Volume of H2 collected 53.6 mL Pressure of H2, PH2 727.0 mm Hg Temperature 21.3 oC 1. Determine and report the pressure of collected hydrogen gas in atmospheres. Report this result to one more digit than allowed by applying the rules of significant figures. (1 atm = 760 mm Hg, an exact conversion factor.) 2. Determine the moles of hydrogen collected by substituting the appropriate quantities into the ideal gas equation and solving. Report this result to one more digit than allowed by applying the rules of significant figures. Notes: the gas temperature is the same as the listed temperature; R = 0.082057 L-atm/mol-K. Be mindful of units. 3. Determine the experimental atomic mass of Cu. Round this result to the correct number of significant figures. 4. Determine the percent relative error (= ????????????−?ℎ????????? ?ℎ????????? ? 100). The molar mass of Cu is 63.546 g/mol.arrow_forward3. Hydrochloric acid is a strong acid that can be used to make sodium chloride and a weak acid, nitrous acid. Write the balanced chemical equation of this reaction. (You can use the information in part b to help you determine states), b. Using the information below determine the AºHrn of the gencration of nitrous acid and sodium chloride. 2NACI (s) + H;O (1) → 2HCI (aq) + Na;O (aq) AH, = 507.1 kJ/mol NO (g) + NO2 (g) → Na;O (aq) + 2NaNO; (aq) AH,n = -427.4 kJ/mol NO (g) + NO2 (g) →N20 (g) + AHrxn = -42.8 kJ/mol (8) 2HNO2 (aq) → N20 (g) + O2 (g) + H2O (I) AHrn = 34.2 kJ/molarrow_forwardA metal cylinder with a capacity of 6.0 L is filled with compressed propane (C3H8). The pressure and temperature of the cylinder when it was initially filled were 120 atm and 75 ◦C, respectively. The molar mass of carbon is 12 g·mol−1 and the molar mass of hydrogen is 1 g·mol−1. a) How many moles of propane are in the cylinder? b) What is the mass of the propane inside the cylinder? c) After some time, the cylinder and its contents cool to 25 ◦C. What is the pressure in the cylinder after it has cooled?arrow_forward
- A 0.3400 g piece of brass is allowed to react with hydrochloric acid at the base of eudiometer. The hydrogen gas generated in the reaction occupies a volume of 48.1 mL and leaves behind a column of acid that is 3.65cm in height. If barometric pressure is measured to be 0.9978 atm, determine the percentages of copper and zinc assuming the temperature of the solution is 22 degrees celsius.arrow_forwardA 0.0665 g sample of aluminum metal reacts with hydrochloric acid to give 90.5 mL of hydrogen gas at 23oC and an atmospheric pressure of 756 mm Hg. The hydrogen gas is collected over water. Write a balanced chemical equation for the reaction between solid aluminum metal and aqueous hydrochloric acid.arrow_forwardGreat Lakes Chemical Company produces bromine, Br2, from bromide salts, such as NaBr, in Arkansas brine by treating the brine with chlorine gas. Write a balanced equation for the reaction of NaBr with Cl2. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.)arrow_forward
- 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.arrow_forward24.00 g of solid calcium carbonate completely decomposes at 579 °C in a 12.000 L sealed vessel. The products of this decomposition are solid calcium oxide and carbon dioxide gas. Note: R = 0.08206 Latm/molK Determine the stoichiometric coefficient of carbon dioxide in the balanced chemical equation. Determine the theoretical yield of carbon dioxide in moles Determine the pressure of carbon dioxide gas produced in this reactionarrow_forwardReferences Use the References to access important values if needed for this question. Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCI(aq) ZnCl2(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 754 mm Hg. If the wet H2 gas formed occupies a volume of 6.46 L, the number of moles of Zn reacted was mol. The vapor pressure of water is 23.8 mm Hg at 25 °C. Submit Answerarrow_forward
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