How many liters of He gas can be produced at 0 °C and 100 atm (STP) from 180 g of Zn? Zn(s)+2HCl(aq) ZnCl₂(aq)+H₂(g) Express your answer with the appropriate units.

Ammonia, NH3, can react with oxygen to form nitrogen gas and water. 4 NH3(aq) + 30₂(g) →→→ 2N₂(g) + 6H₂O(1) If 3.85 g NH3 reacts with 5.78 g O₂ and produces 0.950 L N₂, at 295 K and 1.01 bar, which reactant is limiting? NH,(aq) 0₂(g) Calculate the percent yield of the reaction. percent yield:

CHEM 1 Please solve correctly and give the complete solution.

1. Many laboratory gases are sold in steel cylinders with a volume of 43.8 L. If there are x kilograms of argon inside a cylinder whose pressure is 4,592 kPa at 46°C, what the value of x? (1 atm = 101325 Pa) 2. A tank was filled with 18 g of oxygen (O2), 75 g of nitrogen (N2) and 4 g of carbon dioxide(CO2). At 25°C the pressure of the tank was 8.5 atm. If the partial pressure of CO2 in the tank is x atm, what is the value of x? 3. 13 g of an unknown gas in a tank with a volume of 5.53 L has a pressure of 3.83 atm at 28°C. If the molecular weight of the gas is x g/mol, what is the value of x? 4. Ammonia burns in air as follows:NH3(g) + O2(g) → N2(g) + H2O(g) (unbalanced)If x liters of N2(g) are formed by burning 9.8 L of ammonia and 9.8 L of oxygen with all species at the same temperature and pressure, what is the value of x? 5. Methane (CH4) at 48°C and 776 mmHg has a density x g/L. What is the value of x? 6. A 3.50 L sample of neon has a pressure of 1.03 atm at 17°C. If the sample has…

A 7.00 L tank at 15.8 °C is filled with 5.07 g of sulfur tetrafluoride gas and 11.5 g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: x10 sulfur tetrafluoride partial pressure: || atm mole fraction: sulfur hexafluoride partial pressure: atm Total pressure in tank: atm

Consider the following situation:  You have a 50 L tank of compressed air at 15 atm and 100 ºC.  You then pass the compressed air through a "titanium getter" which contains fragments of hot titanium metal.  The purpose of the "getter" is to remove oxygen gas from the sample as Ti reacts with oxygen to form solid TiO2 (known as titania).  Once the purified air is passed through the getter is it cooled back down to  100 ºC and fills another 50 L storage tank.  If air typically contains about 20% oxygen, what could the pressure in the storage tank be?     Question 2 options:   A)  12 atm   B)  15 atm   C)  18 atm   D)  24 atm

An experiment is performed to determine the volume of gas produced by the following reaction: 2HCl(aq) + Mg­(s)                  MgCl2(aq) + H2(g) A.  What is the maximum mass of Mg in g that could be reacted at 20oC temperature and 1.0atm, if the volume of the gas burette is 50mL? (Hint: Find moles of H2 using the ideal gas law; then, convert to g of Mg.)   B. If the experiment were moved to a higher elevation and the pressure was decreased to 0.95 atm would the maximum amount of Mg increase or decrease?   C. If 16mg of Mg were reacted, what is the volume of gas produced in this reaction?   D. What is the solvent for this reaction?   E. Would the HCl(aq) be considered a strong, weak, or non-electrolyte?   F. Would the MgCl2(aq) be considered a strong, weak, or non-electrolyte?

11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b)  The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.

Calculating partial pressure in a gas mixture GHA 0/5 A 8.00 L tank at 24.9 °C is filled with 9.56 g of boron trifluoride gas and 4.99 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: boron trifluoride partial pressure: atm mole fraction: sulfur tetrafluoride partial pressure: atm Total pressure in tank: atm Explanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Cen 42°F Cloudy ENC DELL