A sample of gas mixture from a neon sign contains 4.95x10^-2 mol Ne and 3.07x10^-2 mol...

A sample of gas mixture from a neon sign contains 4.95x10^-2 mol Ne and 3.07x10^-2 mol Kr . What are the mass percentages of Ne and Kr in the gas mixture?

Mass percentages of Ne = %

Mass percentages of Kr = %

Expert Solution

mass of Ne = no of moles * gram atomic mass

= 4.95*10^-2 * 20.1797 = 0.9988g

mass of Kr = no of moles * gram atomic mass

= 3.07*10^-2 *83.798 = 2.573g

Mass percentages of Ne % = 0.9988*100/0.9988+2.573

= 0.9988*100/3.5718 = 27.96%

Mass percentages of Kr% = 2.573*100/0.9988+2.573

= 2.573*100/3.5718 = 72.04%

queen_honey_blossom answered 2 years ago

Two gas cylinders are identical. One contains the monatomic gas neon (Ne), and the other contains...

Two gas cylinders are identical. One contains the monatomic gas neon (Ne), and the other contains an equal mass of the monatomic gas krypton (Kr). The pressures in the cylinders are the same, but the temperatures are different. Determine the ratio KEAvg,krypton / KEAvg,neon of the average kinetic energy of a krypton atom to the average kinetic energy of a neon atom. KEAvg,krypton / KEAvg,neon = Need equation with numerical answer!! Thanks

A gas cylinder contains 2.30 mol He, 1.35 mol Ne, and 1.75 mol Ar. If the...

A gas cylinder contains 2.30 mol He, 1.35 mol Ne, and 1.75 mol Ar. If the total pressure in the cylinder is 2290 mmHg, what is the partial pressure of each of the components? Assume constant temperature. P(He) = ? P(Ne) = ? P (Ar) = ?

A cylinder of volume 0.240 m3 contains 10.1 mol of neon gas at 21.6°C. Assume neon...

A cylinder of volume 0.240 m3 contains 10.1 mol of neon gas at 21.6°C. Assume neon behaves as an ideal gas (g) Compute ΔU − W. (i) Compute Q, the thermal energy transfer.

A gas mixture contains 0.650 mol of N2, 0.100 mol of H2, and 0.400 mol of...

A gas mixture contains 0.650 mol of N2, 0.100 mol of H2, and 0.400 mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 11.0 L vessel at 27.00°C. 1) Total Pressure: 2.57 atm 2) Pressure of H2: ____ atm 3) Pressure of N2: ____ atm 4) Pressure of CH4: ___ atm

A mixture of neon and nitrogen gases contains neon at a partial pressure of 594 mm...

A mixture of neon and nitrogen gases contains neon at a partial pressure of 594 mm Hg and nitrogen at a partial pressure of 295 mm Hg. What is the mole fraction of each gas in the mixture? XNe = XN2 = A mixture of oxygen and neon gases at a total pressure of 674 mm Hg contains oxygen at a partial pressure of 299 mm Hg. If the gas mixture contains 2.48 grams of oxygen, how many grams of...

A rigid, closed container contains 0.0700 mol of Ne(g) and a sample of the solid, ammonium...

A rigid, closed container contains 0.0700 mol of Ne(g) and a sample of the solid, ammonium nitirite, NH4NO2. Assume that the volumes of solids are negligible compared to the volume of the container. The pressure of the Ne is meausre at 33 degrees celsius and is found to be .409atm. The container is then heated to 333 degrees celsius and all of the ammonium nitrite decomposes according to the reaction. NH4NO2(s) --> N2(g) + 2H2O(g) The Ne is not involved...

a cylinder of volume 0.240 m^3 contains 10.3 mol of neon gas at 19.0 C. assume...

a cylinder of volume 0.240 m^3 contains 10.3 mol of neon gas at 19.0 C. assume neon behaves as an idea gas. a) what is the pressure of the gas b) find the internal energy of the gas c) suppose the gas expands at a constant pressure to a colume of 1.000m^3. how much work is done on the gas? d) what is the temperature of the gas at the new volume e) find the internal energy of the gas...

A sample of gas contains 0.1000 mol of HCl(g) and 5.000×10-2 mol of Br2(g) and occupies...

A sample of gas contains 0.1000 mol of HCl(g) and 5.000×10-2 mol of Br2(g) and occupies a volume of 4.79 L. The following reaction takes place: 2HCl(g) + Br2(g)2HBr(g) + Cl2(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. A sample of gas contains 0.1800 mol of HCl(g) and 9.000×10-2 mol of Br2(g) and occupies a volume of 9.74 L. The following reaction takes place: 2HCl(g) + Br2(g)2HBr(g)...

A gas mixture in a 1.00L reaction vessel at 100ºC contains 4.5 mol of Br(g) and...

A gas mixture in a 1.00L reaction vessel at 100ºC contains 4.5 mol of Br(g) and 33.1 mol F2(g). Compte the mole fraction of each gas in this mixture. When this mixture is heated to 150ºC, Br2(g) and F2(g) react to form BrF5(g) according to the following balanced chemical reaction: Br2(g)+ 5F2(g)---------- 2 BrF5(g). At a certain point, 2.2 mol of BrF5(g) is present in this reaction vessel. Determine the mole fractions of Br2(g), F2(g) and BrF5(g) at this point...

An equilibrium mixture contains 0.6500.650 mol of each of the products (carbon dioxide and hydrogen gas)...

An equilibrium mixture contains 0.6500.650 mol of each of the products (carbon dioxide and hydrogen gas) and 0.2000.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g)+H2O(g)−⇀↽−CO2(g)+H2(g)CO(g)+H2O(g)↽−−⇀CO2(g)+H2(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.3000.300 mol once equilibrium has been reestablished?

Question