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V = n ⋅ V molar. For 2 moles of a gas at STP the volume will be. 2 moles ⋅ 22.4 L/mol = 44.8 L. For 0.5 moles the volume will be. 0.5 moles ⋅ 22.4 L/mol = 11.2 L, and so on. The molar volume of a gas is derived from the ideal gas law P V = nRT: P V = nRT → V = nRT P → V n = RT P. Let's say you were given a temperature of 355 K and a ...
2 Answers. Dr. Hayek. May 17, 2016. d = 1.79g ⋅ L−1. Explanation: Assuming that carbon dioxide behaves ideally, then we can use the ideal gas law: P V = nRT. Since we are looking for the density of CO2, we can modify the law as follows: First we replace n by n = m M M where, m is the mass and M M = 40 g mol is the molar mass of CO2.
One mole of which gas has the greatest density at STP? A) CO2 B) Ar C) Kr D) All three gases have the same density. What is the density of oxygen gas at STP? A. 32 g/L B. 22.4 g/L C. 1.43 g/L D. 0.71 g/L; The density of a gas is 3.12 g L-1 at STP. What is the gas? The density of a gas is 1.146 g L-1 at STP. What is the gas?
Density of Gas: Density is defined as the mass of a substance occupy per unit volume. At standard temperature and pressure (STP) conditions, the molar volume of a gas is equal to 22.4 L. To find the density of the gas at STP, we will use the molar mass of the gas as mass and the molar volume (22.4 L) as volume. Answer and Explanation: 1
Calculate the density of SO3(g) at STP conditions. "Dry ice" is the solid form of carbon dioxide. Determine the mass of CO2 gas in grams that are present in 57.7 L of CO2 at STP. What is the density of hydrogen gas at STP? Determine the density of NH3 gas at 435K and 1.00atm. a. 0.321g/L b. 2.24g/L c. 2.10g/L d. 0.477g/L
A) How many hydrogen molecules are in 2.75 L of H2 gas at STP? B) What is the density of nitrogen gas, N2, at STP? C) If the density of an unknown gas is 1.34g/L at STP, what is its molar mass? D) The formula for illegal drug cocaine is C17H21NO4. What is; The volume of a sample of carbon dioxide gas is 880 mL at standard temperature and pressure.
Well, all we can say is that their volumes are dependent on their intermolecular forces of attraction... which lead to different densities. If both gases are at STP, they share the same temperature and system pressure, and if the same number of particles of each gas are in the closed container, then the only variable left is their volumes. The molar volume V/n -= barV is dependent on the ...
Using the Ideal Gas Law, you would find the volume of 1 mole of a gas at Standard Temperature and Pressure (STP). STP = 1 atm of pressure and 273 K for temperature. P = 1 atm V = ??? n = 1 mole R = 0.0821 atm L/mol K K = 273 K. #P V = n R T # solves to #V = (n R T) / P#
What units are normally used to express the density of gases? Calculate the density of C H 4 at STP. Calculate the density of oxygen, O_2, of STP 1.00 atm and 10.0 degrees C. Calculate the mass of gasoline, in grams, that you would add to your cars tank given the density of gasoline is 0.75 g/mL, and the volume is 2.9 liters.
Place the following gases in order of increasing density at STP. a. N_2 b. NH_3 c. N_2O_4 d. Ar; Rank the gases Ar, N_2, CH_4, and C_2H_6 in order of the increasing density at STP. Which of the following arranges the given gases in order of increasing (smallest to largest) density at STP, respectively?