4. You collect a sample of hydrogen gas in an inverted buret by displacement of water at 29.00 °C. The buret could not be submerged deep enough in the water bath to equilize pressure. The water level in the buret was 14.76 cm above the water level in the water bath. The volume of gas in the buret was determined to be 32.60 mL.

Oxygen gas is generated by the reaction:2KClO3(s) → 2KCl(s) + 3O2(g)and collected over water at 27 °C in a 2.00 L vessel at a total pressure of 760 torr. (vapor pressure of water at this temperature = 26.0 torr) How many moles of KClO3 were consumed in the reaction?     0.0790 moles     0.119 moles     0.0813 moles     0.0527 moles     None of the above,

A gas mixture consists of 0.421 mol hydrogen (H2), 0.664 mol carbon dioxide (CO2), and 1.965 mol nitrogen (N2). If the total pressure of the mixture is 2.48 atm, calculate the partial pressure of each component gas in the mixture.

Zn reacts with hydrochloric acid to give zinc chloride and hydrogen gas. A sample of 5 g of a Zn mineral requires 10 mL of commercial HCl of 37% purity, by weight and density 1.19 g/mL, to react completely. Find: a) The mass of zinc contained in the sample. b) The purity of the zinc mineral. c) The pressure exerted by the hydrogen gas collected in a 2 L container and at a temperature of 20ºC.please use conversion factors and mark the solutions

A sample of hydrogen gas was collected by displacement of water in a large gas buret. The total pressure in the buret was measured as 764.2 torr, the temperature was 23.0 °C, and the buret contained 511 mL of the collected gas. How many moles of hydrogen were collected? (At 23.0 °C, the vapor pressure of water is 21.1 torr.)

Part A Hydrogen can be extracted from natural gas according to the following reaction: CH4 (9) + CO2 (g) = 2 CO (g) + 2 H2 (9) K, = 4.5 × 102 at 825 K An 85.0-L reaction container initially contains 22.3 kg of CH4 and 55.4 kg of CO2 at 825 K. Assuming ideal gas behavior, calculate the mass of H2 (in g) present in the reaction mixture at equilibrium. ΑΣφ Submit Request Answer రం

When solid calcium carbonate is reacted with aqueous hydrochloric acid, the products of the reaction include aqueous calcium chloride, liquid water, and gaseous carbon dioxide. Calculate the volume of CO₂ gas (in L) collected over water at 25.0 °C when 25.1 g of calcium carbonate is added to excess hydrochloric acid if the total pressure is 911.0 mmHg. The vapor pressure of water at 25.0 °C is 23.8 mmHg.

A 0.3 L vessel contains 20 mmol of methane gas at 30 °C. What is the calculated pressure of the gas, using the ideal-gas equation (PV = nRT)? [R = 8.314 L kPa mol–1 K–1. Enter your answer as a numerical value in units of kPa.]

Consider the reaction, 2 Al (s) + 6 HCI (aq) → 2 AICI, (aq) + 3 H, (g). When 40.0 g of Al react with an excess of HCl at 25.0 °C the pressure in a collection flask is measured to be 1.50 atm. What is the volume of the collection flask?

A sample of an ideal gas at 1.00 atm and a volume of 1.90 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 80.0 atm, what was the volume of the sample? Assume that the temperature was held constant. V = L