If a mercury barometer reads 846 mm Hg, what is the pressure in bar?

47 HCl(g) reacts with ammonia gas, NH3(g), to form solid ammonium chloride. If a sample of ammonia occupying 250 mL at 21 C and a pressure of 140 torr is allowed to react with excess HCl, what mass of NH4Cl will form?

A 19.9-mL volume of a hydrochloric acid solution reacts completely with a solid sample of magnesium carbonate, producing 183 mL of CO2 that is collected over water at 24.0C and 738 torr total pressure. The reaction is 2HCl(aq)+MgCO3(s)CO2(g)+H2O(l)+MgCl2(aq) What is the molarity of the HCl solution?

A sample of natural gas is 85.2% methane, CH4, and 14.8% ethane, C2H6, by mass. What is the density of this mixture at 18C and 771 mmHg?

A mixture contained calcium carbonate, CaCO3, and magnesium carbonate, MgCO3. A sample of this mixture weighing 7.85 g was reacted with excess hydrochloric acid. The reactions are CaCO3(g)+2HCL(aq)CaCl2(aq)+H2O(I)+CO2(g)MgCO3(s)+2HCL(aq)MgCl2(aq)+H2O(I)+CO2(g) If the sample reacted completely and produced 1.94 L of carbon dioxide, CO2, at 25C and 785 mmHg, what were the percentages of CaCO3 and MgCO3 in the mixture?

Nitrogen monoxide gas reacts with oxygen gas to produce nitrogen dioxide gas. What volume of nitrogen dioxide is produced from the reaction of 1 L nitrogen monoxide gas with 3 L oxygen gas? What volume, if any, of the reactants will remain after the reaction ends? Assume all volumes are measured at the same pressure and temperature.

109 An ore sample with a mass of 670 kg contains 27.7% magnesium carbonate, MgCO3. If all of the magnesium carbonate in this ore sample is decomposed to form carbon dioxide, describe how to determine what volume of CO2 is evolved during the process. What would have to be measured to predict the needed volume in advance?

Consider the following unbalanced chemical equation: ^Sfr) + O2(g) —? Cu2O(s) + SO2(g) What volume of oxygen gas, measured at 27.5 °C and 0.998 atm. is required to react with 25 g of copper!I) sulfide? What volume of sulfur dioxide gas is produced under the same conditions?

A mixture contained zinc sulfide, ZnS, and lead sulfide, PbS. A sample of the mixture weighing 6.12 g was reacted with an excess of hydrochloric acid. The reactions are ZnS(s)+2HCL(aq)ZnCl2(aq)+H2S(g)PbS(s)+2HCL(aq)PbCl2(aq)+H2S(g) If the sample reacted completely and produced 1.049 L of hydrogen sulfide, H2S, at 23C and 762 mmHg, what were the percentages of ZnS and PbS in the mixture?

A typical barometric pressure in Kansas City is 740 torr. What is this pressure in atmospheres, in millimeters of mercury, and in kilopascals?