A 0.334 g sample of an unknown halogen occupies 109 mL at 398 K and 1.41 atm. What is the identity of the halogen? (Hint: use the ideal gas law to find n (moles). Then divide mass by moles to find molar mass. Which option would be correct? Bromine, Fluorine, Chlorine, Iodine, or Germanium?

Q: The partial pressures of CH4, N2, and O2 in a sample of a gas mixture were found to be 123 mmHg, 505…

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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…

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Q: A steel cylinder contains 150.0 moles of argon gas at a temperature of 25°C and a pressure of 8.93 M…

A: Answer:- This question is answered by using the simple concept of ideal gas equation which involves…

Q: A gas with a mass of 95.14g occupies 48.8L at 659mmHg and 25.3°C. What is its molecular weight? Use…

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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: 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

A: Weight = 14.0 g fluorine gas P1 =  21.0atm at a certain Temperature P2 = 4.30

Q: A sample of an ideal gas at 1.00 atm1.00 atm and a volume of 1.62 L1.62 L was placed in a weighted…

A: Given: Initial Pressure, P1 = 1.00 atm Initial volume, V1 = 1.62 L Final Pressure, P2 = 80.0 atm…

Q: Oxygen is a product of the decomposition of mercury(II) oxide as shown below. 2 HgO(s) → 2 Hg(ℓ) +…

A: The decomposition of mercury(II) oxide provides Oxygen and mercury as the products. 2 HgO(s) → 2…

Q: Consider a gas mixture that contains only helium (He) and neon (Ne). If the partial pressure of He…

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

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Q: For many purposes we can treat ammonia  NH3  as an ideal gas at temperatures above its boiling…

A: Initial Volume = V1 Final Volume = V2  Initial Temperature = T1 = −14.0°C = (−14.0 + 273.15) K =…

Q: Calculate the partial pressure of helium gas for a volume of 1.0 x 10-6 m3 of 222Rn gas after 9…

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Q: In a common Freshman College Laboratory experiment, KClO3 is decomposed by heating to give KCl and…

A: 2 KClO3 ---> 2 KCl + 3O2  Volume of O2 = 0.238 L  Temperature = 28°C  Pressure = 752 mm Hg 760 mm…

Q: A 5.0 × 102 sample of sulfur dioxide, SO2(g), has a volume of 2.37 × 106 L. If the temperature of…

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Q: Use the van der Waals equation and the ideal gas equation to calculate the volume of 1.000 mol of…

A: Given that Number of moles of Neon, n = 1.000 mol Pressure of Neon, P = 500.0 atm Temperature of…

Q: 0.17 moles of hydrogen gas and 0.33 moles of nitrogen gas are created from the reaction 2NH3 (g) →…

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Q: A flask at room temperature contains equal numbers of di-nitrogen molecules and krypton atoms. (a)…

A: The question is based on the concept of gaseous state . we need to identify the gas having higher…

Q: According to our modern understanding of the gas laws, there are four measurable properties…

A: • We need to determine in Boyles's experiment which two variables were held constant.

Q: Hydrogen cyanide is prepared commercially by the reaction of methane CH4(g), ammonia, NH3(g), and…

A: The commercial preparation of hydrogen cyanide is to be expressed.

Q: A student obtained a mass of 0.266 g CO2 during his experiment. The atmospheric pressure was 751.6…

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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.