3. The reaction, MnO:(s) + 4 HCl(aq) → MnCl:(aq) + Cl:(g) + H;O(1) was being studied. 12.2 g of MnO; were reacted with 70.0 ml of 2.50 M HCl solution. The chlorine produced was collected in a vessel. The pressure measured 0.971 atm at a temperature of 78.2 °C. Determine the volume of chlorine produced if the theoretical yield was obtained.

3. The reaction, MnO:(s) + 4 HCl(aq) → MnCl:(aq) + Cl:(g) + H;O(1) was being studied. 12.2 g of MnO; were reacted with 70.0 ml of 2.50 M HCl solution. The chlorine produced was collected in a vessel. The pressure measured 0.971 atm at a temperature of 78.2 °C. Determine the volume of chlorine produced if the theoretical yield was obtained.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

If 8g of ammonium hydroxide is completely decomposed by the reaction below in a closed container with a total volume of 5.00L and at 25°C, what will be the partial pressure of the ammonia gas liberated, in atmospheres? Assume the volume of the liquid is negligible. NH4OH(aq) --> H2O(l)+NH3(g)
+7 (A) 15.2 L B) 0 C) +3 D) -2 19. 68.1 g solid CaCO3 is mixed with excess HC1. What is the volume of CO2 will be collected at 0.0 °C, and 1 atm. (Molar mass CaCO3 = 100.08 g/mol, CO₂ = 44.1 g/mol CaCO3 (s) + 2 HCl(aq) → H₂O (1) +CaCl2 (aq) + CO₂(g) C) OL B) 29.9 L C D) 155 L 20. A gas sample has an initial volume of 0.500 L and initial pressure of 1.0 atm. Wha the volume when the pressure of the sample is decreased to 0.50 atm? Assume the temperature and number of moles of the gas are constant. P₁V₁ = P₂1 A) .0 L B) 0.025 L
Mg(s) + 2 HCl(aq) → MgCl2(g) + H2(g) PV = nRT R = 0.082061. 2. The volume of hydrogen gas produced was not at standard temperature and pressure. Convert the volume at the pressure and temperature of the experiment to a volume at standard temperature and pressure: STP (T = 273.15K and P = 1.00 atm). Mass of flask/stopper/5 mL H2O=112.794 g Mass of flask/stopper/filled flask of H2O=250.302 g Volume of gas space in flask (the difference between the above two measurements converted to L) =0.137508 L Trial 1: mass of Mg (g) =0.013 g pressure= 1.0104 atm temperature= 298.35 K moles of H2 =0.00054 mol
(c) A halothane-oxygen gas mixture is placed in an enclosed container. The partial pressure of halothane and oxygen are 170 kPa and C, respectively. The mole fraction of oxygen gas is 0.458. (i) Calculate the total pressure of halothane-oxygen mixture. (ii) Determine the partial pressure of oxygen, C.
A 9.00 L tank at 4.22 °C is filled with 3.83 g of sulfur tetrafluoride gas and 7.58 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. Be sure your answers have the correct number of significant digits. mole fraction: sulfur tetrafluoride partial pressure: || atm mole fraction: sulfur hexafluoride partial pressure: atm Total pressure in tank: atm
A gas mixture contains 4.5 mol Br, and 33.1 mol F,. (a) Compute the mole fraction of Br, in the mixture. (b) The mixture is heated above 150°C and starts to react to give BrFs: Br2(g) + 5 F2(g) –→ 2 BrF;(g) At a certain point in the reaction, 2.2 mol BrF5 is present. Determine the mole fraction of Br2 in the mixture at that point.
A vessel of a certain volume contains two ideal gases, let's call them A(g) and B(g). The mole fraction of gas A is ??=0.32. At a certain temperature the pressure in the vessel, P1, is measured. Then three additional moles of one of these gases are added while keeping the temperature fixed and the new pressure, P2, is measured. The ratio of the two pressures is found to be: ?2/?1=2.15. How many moles of A(g) and B(g) were originally in the vessel?
A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. The vessel is a stainless-steel cylinder that measures 13.0cm wide and 15.6cm high. The maximum safe pressure inside the vessel has been measured to be 3.60MPa. For a certain reaction the vessel may contain up to 0.0457kg of carbon dioxide gas. Calculate the maximum safe operating temperature the engineer should recommend for this reaction. Write your answer in degrees Celsius. Be sure your answer has the correct number of significant digits.
1) a) Sulfuric acid, the industrial chemical produced in the greatest quantity each year, is prepared by the reaction of sulfur in the presence of oxygen and water as described in the balanced chemical equation below. Calculate the volume, in ml, of 18.0 M sulfuric acid solution that can be prepared from the reaction of 1850 g of sulfur with 6.50E4ML oxygen gas at 25°C and 0.965atm and plenty of water. 25(solid) + 302 (gas) + 2H20(liquid) > 2H:SO4(aqueous) b. Which substance is the limiting reactant? Explain how you know.
A 0.516 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H,SO,(aq) MSO,(aq) + H,(g) A volume of 223 ml. of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 "C. The vapor pressure of water at 25 "C is 23.8 Torr. Calculate the molar mass of the metal. g/mol molar mass:
A certain gas mixture is at a pressure of 3500 kPa and is composed of 18.0 g of O2 and 28.0 g of CO2. Determine the partial pressure of O2 gas in the mixture.
Calculate the mole fraction and partial pressure of each gas as well as the total pressure in the tank using the information below.