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: Aluminum and hydrochloric acid were reacted, producing hydrogen gas. The total pressure of the…

A: The temperature, pressure, volume, and mole of the gas are related by the ideal gas equation. The…

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 sample of vapor weighing 0.368 g filled a Florence flask when heated in a water bath at 95.0°C.…

A:

Q: If 0.750 L of argon at 1.50 atm and 177°C is mixed with 0.235 L of sulfur dioxide at 95.0 kPa and…

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: A sample of oxygen is collected over water at 24°C and 757 mm Hg in a 125-mL flask. The vapor…

A: Given : Mass of nitrogen gas, m = 0.0205 g  The molar mass of nitrogen gas, M= 28.02 g/mol Moles =…

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: A 0.55 g sample of a certain metal reacted with acid to liberate 375.0 mL of hydrogen gas when…

A:

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

A:

Q: A sample of CO2 gas at 150.°C has a volume of 350. mL at 760. mm Hg. How many moles of CO2 are…

A: Ideal gases are those gases which follow ideal gas equation. The relation between pressure, volume,…

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: A student collected 26.86 mL of H2 over water at 20.00 °C. The water level inside the collection…

A: Volume of gas V = 26.86 mL = 0.02686 L Temperature T1 = 20.00 °C = 20.00 + 273 K = 293 K  Barometric…

Q: A 0.704-g sample of a colorless liquid was vaporized in an evacuated 250.-mL flask at 121°C to give…

A: Given information: Mass of sample = 0.704 g Pressure (p) = 786 mmHg Volume (V) = 250 mL Temperature…

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: 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 2.000 gram sample containing graphite (carbon) and an inert substance was burned in oxygen and…

A: A 2.000 gram sample containing graphite (carbon) and an inert substance was burned in oxygen and…

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 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 0.0665 g sample of aluminum metal reacts with hydrochloric acid to give 90.5 mL of hydrogen gas at…

A: Stoichiometry relates the amount of reacting with the formed species. As per this concept, the…

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

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: HCl can be made by the direct reaction of H2 and Cl2 in the presence of light. Assume that 3.0 g H2…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

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: What is the volume, in mL, of the dry oxygen gas at STP

A:

Q: oxygen gas from the decomposition of KClO3 was collected by water displacement. the barometric…

A: The objective of this question is to calculate the partial pressure of oxygen collected in an…

Q: A 0.0500-g sample of magnesium is reacted with 25 mL of 3.0 M sulfuric acid as described in the…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

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

A:

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 gaseous arsine in a sealed 500.0 mL flask at 278.0 torr and 223 K is heated to 473 K at…

A: The no of moles of arsine before and after decomposition can be calculated from ideal gas equation.…

Q: A 2.00 L reaction container at 25.0 °C contains CO2 (g) and O2 (g). The total pressure of the gases…

A: The partial pressure (p) of a gas is related to the total pressure (Pt) of the gas by the mole…

Q: A sample contianing 8.12g of solid CO2 is put in an empty sealed 5.4L container at a temperature of…

A: Given, the amount of CO2 =8.12 gvolume of container =5.4 Ltemperature T =250.1 Kgas constant…

Q: Balanced Equation: 2KClO3->3O2+2KCl.  d) How many molecules of oxygen gas were collected? e) What…

A:

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

A:

Q: An empty flask weighs 128.950 g. After vaporization of a sample of volatile liquid at a temperature…

A:

Q: A chemistry student places 5.35 grams of aluminum metal into phosphoric acid.  The reaction gives…

A: Given: The mass of aluminium metal taken = 5.35 grams The percent yield = 78.5% We have to calculate…

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

A:

Q: Heating a 6.589 g sample of an ore containing a metal sulfide, in the presence of excess oxygen,…

A:

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

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.