A 0.55 g sample of a certain metal reacted with acid to liberate 375.0 mL of hydrogen gas when collected over water at 20.0 degree Celsius and 790.0 torr (corrected room pressure). The vapor pressure of water is 17.535 mm Hg at this temp. Assuming there is no need to account for pressure differences due to water levels, and using the reaction below, what is the molar mass and identity of the metal? 2X + 6HCl --> 3H2 + 2XCl3

Q: The composition of the atmosphere is relatively constant, with the exception of humidity; the amount…

A: (a) Dalton's law states that the total pressure of a mixture of gaseous mixture is the sum of…

Q: Oxygen gas, generated by the reaction is collected over water at 27°C in a 5.87-L vessel at a total…

A: Given : Temperature = 27 oC Total pressure of gas mixture = 1.00 atm = 760 torr Volume of vessel =…

Q: A 4.0 liter rigid, indestructible metal can is filled with nitrogen gas at 45 °C to a pressure of…

A:

Q: Gases produced by a chemical reaction can easily be collected over water. To determine the pressure…

A: Given reaction is :  Mg + 2HCl -> MgCl2 + H2 total pressure of gas = 785.0mm Hg Temperature =…

Q: One of the steps to sweeten sour gas using the Claus process is reacting hydrogen sulfide gas with…

A: the reaction is16 H2S (g) + 8 SO2 (g)  16 H2O (g) + 3 S8 (s)Given,volume of H2S= 8.40 kL = 8.40…

Q: 4. A student observed that 0.234 grams of a metal produced 92.2 mL of wet hydrogen gas measured with…

A:

Q: If 14.5g of calcium carbonate decomposes via the following reaction, how many liters of carbon…

A: Number of moles of Calcium carbonate can be calculated as follows: No. of moles of CaCO3= massmolar…

Q: Hydrogen gas generated from the reaction of aluminum with hydrochloric acid was collected over water…

A:

Q: A 2.16 g sample of phosphorus was burned in a large excess of chlorine, and the phosphorus chloride…

A: To Calculate molar mass , we can use the relation that rate of effusion is inversely proportional to…

Q: A 25.0 mL sample of 0.120 M hydrochloric acid was added to an excess of calcium carbonate. The…

A:

Q: If 27.2 grams of potassium carbonate is reacted with 125 ml of .700 M hydrobromic acid in 3.5 L…

A: K2CO3 + 2 HBr ==> 2 KBr + CO2 + H2O  Given mass of K2CO3 = 27.2 g  Given volume of HBr = 125 ml =…

Q: Phosphorus trichloride is important in the manufacture of insecticides, fuel additives, and flame…

A: To find: (a) What different molecular masses (in amu) can be found for PCl3? (b) Which is the most…

Q: Gas Z was collected over water at 21°C on a day when atmospheric pressure was 757 torr. The volume…

A: The pressure in the collection tube is due to water vapor and the gas Z. Since, the total pressure…

Q: To calculate universal gas constant (R) experimentally, the thermal decomposition reaction of KClO3…

A: The thermal decomposition reaction of KClO3 gives KCl and oxygen. MnO2 is used as catalyst for the…

Q: A flammable gas contains only C, H, N, and Cl. The complete combustion of a 100.0 mg sample of this…

A:

Q: A 4.0-liter rigid metal can is filled with nitrogen gas at 45 °C to a pressure of 1.125 atm. The can…

A:

Q: A 0.6333 g sample of a metal carbonate was reacted with hydrochloric acid. The carbon dioxide gas…

A: Given data, Mass of sample = 0.6333 g temperature = 26.0oC Volume of gas over water = 103.80 kPa…

Q: A sample of 250.9 mL of wet nitrogen gas was collected over water at a total pressure of 753 torr…

A: As per Raoult’s Law,Total Pressure = Partial vapour pressure of water + Partial vapour pressure of…

Q: .:A:2.00-L pocket of air at sea level·has a pressure of 100 kPa. Suppose the air pocket rises and…

A: initial Volume of pocket = V1 = 2 L Initial pressure in pocket = P1 = 100 kPa Final Volume of pocket…

Q: A 250MI stoppered The pressure of the torr. What would the the flask was transfe

A:

Q: If 27.2 grams of potassium carbonate is reacted with 125 ml of .700 M hydrobromic acid in a 3.5 L…

A: The reaction stoichiometry plays a major role in the yield of the product. The reaction…

Q: A sample of 257.0 mL of wet nitrogen gas was collected over water at a total pressure of 759 torr…

A:

Q: When 0.681 g of zinc was added to 75.0 mL of 0.3 M hydrochloric acid, hydrogen gas was produced. For…

A:

Q: Hydrogen gas is collected over water at 23.5 °C and an atmospheric pressure of 765 mmHg. Calculate…

A: Hydrogen gas is collected over water at 23.5 °C and an atmospheric pressure of 765 mm Hg. Calculate…

Q: What is the experimental molar mass (that is, calculated from the data given and not taken from the…

A: Mass of magnesium = 0.0294 grams Temperature  of Hydrogen gas = 25.9°C  or 299.05K partial pressure…

Q: A sample of limestone (calcium carbonate, CaCO3) isheated at 950 K until it is completely converted…

A: Given, 8.47 kg of solid Ca(OH)2 T = 950 K P= 0.976atm

Q: 0.0500 grams of zinc metal reacted in excess HCl(aq) in a gas tube and produced hydrogen gas that…

A: Given: The mass of Zn is 0.0500 g. The vapor pressure of water is 23.8 mmHg. Barometric pressure is…

Q: What is the experimental molar mass (that is, calculated from the data given and not taken from the…

A: Given: The volume of hydrogen gas generated = 16.99 mL The mass of magnesium taken = 0.0163 g The…

Q: the pressure of Penguinite gas (MM = 85.1 g/mol) is measured to 800. torr at 35 ° calculate its…

A: Temperature = 35°C = 308.15 K Pressure = 800 Torr Molar mass = 85.1 g/mol Density = ? Ideal gas…

Q: Calculate the volume of 1.62g of Helium gas at 25.670C and 872 mmHg.  (R = 0.0821 atm.L/mol.K

A:

Q: A sample of 222.9 mL of wet nitrogen gas was collected over water at a total pressure of 785 torr…

A:

Q: The vapor of a volatile liquid just fills the entire space in a flask kept at a temperature of 100oC…

A:

Q: Given the reaction: 2 Al (s) + 6 HCI (aq) 2 AICI3 (aq) + 3 H2 (g) A strip of aluminum of unknown…

A: All the required calculations have been done in the following step.

Q: 1.) This reaction occurs in large test tube at 32.0oC: 2 Al (s)  + 3 H2SO4(aq) ---> 6 H2 (g)  +…

A: The balanced reaction taking place is given as, => 2 Al (s) + 3 H2SO4 (aq) -------> 6 H2 (g) +…

Q: In an experiment, a sample of zinc metal was added to excess hydrochloric acid and the evolved…

A:

Q: In deep sea diving the composition of air a diver breathes must be changed in accordance with the…

A: Given that : % of oxygen in the air = 20% The partial pressure of oxygen in air = 0.20 atm Total…

Q: You collected 44.1 mL of hydrogen gas in a eudiometer following the procedure outlined in this…

A:

Q: 0380 of Mg strip reacted completly with 6 M HCL in the gas burret and 35.8 mL of hydrogen gas is…

A:

Q: A 0.3 L vessel contains 100 mmol of argon gas at 170 °C. What is the calculated pressure of the gas,…

A:

Q: A sample of O, with a pressure of 1.31 atm and a volume of 243 mL is allowed to react with excess…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: A 0.516 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H, SO,(aq)…

A: A metal on reacting with acid will result in the production of hydrogen gas as follows:…

Q: Solid lithium hydroxide is used to remove CO2 from the air in submarines. It reacts with the CO2 to…

A:

Q: Elemental analysis is performed on an organic liquid with a fishy odor. Vaporization of 275.0 mg of…

A: Given:Mass of compound = 275.0 mg = 275.0 ×10-3 g.Volume of Solution = 110 mL = 110×10-3…

Q: A sample of 263.0 mL of wet nitrogen gas was collected over water at a total pressure of 756 torr…

A: Introduction :  Molarity is defined as the number of moles of solute dissolved in one litre of the…

Q: in the following reaction, 27.1 mL of o2(g) is collected over water at 23*C and barometric pressure…

A:

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.