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- A piece of metal "X" weighing 0.0382 g was placed in an eudiometer containing dilute aqueous HCI. After the metal fully dissolved ,15.4 mL of hydrogen gas was collected by displacement of water and a 400 mm column of water was observed. The water temperature was 25 degrees Celcius and the barometric pressure was 758.8 mm Hg ( torr). Refer to the introduction and data sheet to solve the following problems.
a) Calculate the volume occupied by the hydrogen gas at STP.
b) How many moles of the metal were consumed in the reaction?
c) What is the molar mass of the metal?
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- A piece of metal weighing 0.713 g was placed in an eudiometer containing aqueous HCI. After the metal fully dissolved ,23.5 mL of hydrogen gas was collected by displacement of water and a 400 mm column of water was observed. The water temperature was 25 degrees Celcius and the barometric pressure was 758.8 mm Hg ( torr). Refer to the introduction and data sheet to solve the following problems. Calculate the pressure of the hydrogen gas above the water in the column. Calculate the volume occupied by the hydrogen gas at STP.How many equivalent weights (#ew) of the metal were consumed in the reaction? What is the equivalent weight of the metal?solve as neatly as possible and show completesolution. Round your final answer to 4 decimal places and box / highlight all final answers. and all values must include proper units with proper conversion if needed in your solution. kindly folllow the format Given,Required,Solution subject physical chemistry 1. Calculate the mass of water vapor present in a room of volume 400 m3 thatcontains air at 290C when the relative humidity is 53.0%. Compute for the vaporpressure of water?Osmotic pressures are often reported in units of atmospheres or mm Hg. The latter impliesthat the height of a column of liquid can be used as a measure of pressure. This is, in fact, thebasis of the torricellian barometer from which the units of “torr” come. The pressure, P, isrelated to the height of the column by:P = ρghwhere ρ is the density of the liquid, g is the acceleration due to gravity and h is the height. Whatwill be the height (in mm) of a column of aqueous solution with a density of 0.9987 g/mL, if theosmotic pressure of the solution at 25 °C is 1.4 mm Hg? The density of mercury at thistemperature is 13.8 g/mL
- Following the irrigation of salted soils, 10,000 L of salty irrigation runoff was filtered by a reverse osmosis (RO) treatment plant generating 7,000 L of pure water for return to a local river. Following RO treatment, the brine (left-over salt solution) concentration was 1.95 M NaCl. What was the hydrostatic pressure (atm) required by the RO plant to filter this volume of the salty irrigation runoff at a temperature of 20.0 oC?You are wanting to apply a soil conditioner to your garden. 10mL of conditioner cover 3m^(2) of your garden. However, before you use it you must dilute the concentrate by placing 10ml of Seasol in a 9L bucket. How many litres of the diluted mixture do you need to cover a garden of 80m^(2).Nitrogen gas under an initial pressure of 5.0×106 Pa at 15 ºC is contained in a cylinder of volume 0.040 m3. After some time, the pressure has fallen to 2.0×106 Pa at the same temperature. How much gas has leaked out?
- What is the mole fraction of magnesium nitrate, Mg(NO3)2, in an aqueous solution that is 5.549 wt % in magnesium nitrate? MW(Mg(NO3)2) = 148.315 g/mol. 5.834e-2 1.721e-1 7.080e-3 9.929e-1Chemistry Given an average carbon dioxide concentration of 400 ppmv, estimate the mole fraction, partial pressure, and density of carbon dioxide at standard temperature and pressure.Q1a-> A sample of hydrogen (H₂) gas was collected over water at 60°C. If the total volume of gas collected was 53.9 mL and the atmospheric pressure was 1.14 bar, what mass (in g) of hydrogen gas was collected above the water? The vapour pressure of water at 60°C is 150 torr. Q1b=> What is the molar mass (in g mol-¹) of a gas which has a density of 1.91 g/L at a pressure of 0.91 bar and temperature 15.3°C? Your answer may not correspond to an actual gas. Do not try to identify the gas.
- 1. What is the apparent hard-sphere diameter of CO2 at 0°C? The viscosity of CO2(g) at 1 atm and 0°C is 139 μP (micropoise). 2. When equal amounts of hydrogen, H2, and iodine, I2, are mixed together at a total pressure of 1 bar, the partial pressure of hydrogen iodide, HI, vapour produced from by the reaction H2(g) + I2(g) ⇌ 2 HI(g) is 22.8 kPa. Calculate the equilibrium constant for the reaction. 3. The equilibrium constant for the reaction 2HCl(g) + O2(g) ⇌ H2O(g) + Cl2(g) is 13300 at 400 K and 429 at 500 K. Use the van't Hoff equation to determine the standard enthalpy of reaction.A 500mL sample of O2 gas at 24 degrees Celsius was prepared by decomposing a 3% aqueous solution of hydrogen peroxide, H2O2, in the presence of a small amount of manganese catalyst by the reaction: 2H2O2(aq) -------> 2H2O(g) + O2(g) The oxygen thus prepared was collected by displacement of water. The total pressure of gas collected was 755 mm Hg. What is the partial pressure of O2 in the mixture? How many moles of O2 are in the mixture? Please note that the vapor pressure of water at 24 degrees Celsius is 23 mm Hg.The vapor pressures of two volatile organic compounds, compound 1 and compound 2, at 20 °C are 79.2 torr and 194.7 torr, respectively. What is the gas phase mole fraction of compound 2 above a solution containing an equimolar mixture of the two compounds?Please enter your response in standard notation to three significant figures.