**Hydrogen Peroxide Decomposition Experiment**When hydrogen peroxide is decomposed in a lab, oxygen gas \((\text{O}_2)\) is collected over water at \(15.0^\circ \text{C}\). The molar masses are provided for reference: - \(\text{H}_2\text{O}_2 = 34.02 \, \text{g/mol}\) - \(\text{H}_2\text{O} = 18.02 \, \text{g/mol}\) - \(\text{O}_2 = 32.00 \, \text{g/mol}\).**Reaction Equation:**\[ 2 \, \text{H}_2\text{O}_2(l) \rightarrow 2 \, \text{H}_2\text{O}(l) + \text{O}_2(g) \]**Problem Statement:**1. **Moles of \(\text{O}_2\) Collected**: - Calculate the moles of \(\text{O}_2(g)\) collected if the total pressure of the gas is \(780 \, \text{mmHg}\) and the volume of gas is \(0.4000 \, \text{L}\). Assume all gases are ideal.2. **Volume of Decomposed \(\text{H}_2\text{O}_2\)**: - What volume of pure hydrogen peroxide \((\text{density} = 1.530 \, \text{g/mL})\) decomposed? Assume that the decomposition reaction is complete. If unable to solve part (a), assume that 1 mole of \(\text{O}_2(g)\) was collected.3. **Gas Effusion Explanation**: - If the collected gas \((\text{H}_2\text{O(g)} + \text{O}_2(g))\) is transferred into a rubber balloon (which contains tiny pores), determine which gas will effuse out more quickly. Briefly explain why your answer makes physical sense. Ignore the difference in partial pressures for this problem.**Vapor Pressure Data from Table 10.2**:The table provides the vapor pressures of water at various temperatures:- At \(15^\circ \text{C}\), the vapor pressure is \(12.8 \,

The chemical equation for the decomposition of H2O2 is: 2H2O2(l) ----> 2H2O(l) + O2(g)…

Hydrogen peroxide is decomposed in a lab and the produced O2 (g) is collected over water at 15.0 °C. Molar masses: H2O2 = 34.02 g/mol, H2O = 18.02 g/mol, O2 = 32.00 g/mol. 2 H2O2 () → 2 H20 () + O2 (g) a) Calculate the moles of O2 (g) collected if the total pressure of the gas is 780. mmHg and the volume of gas is 0.4000 L. Assume all gases are ideal. b) What volume of pure hydrogen peroxide (density = 1.530 g/mL) decomposed? Assume that the decomposition reaction is complete. If you were unable to answer part (a), assume that 1 mol of O2 (g) was collected. c) If the collected gas (H2O (g) + O2 (g)) is transferred into a rubber balloon (which contains tiny pores), which gas will effuse out more quickly? Briefly explain (in about 1 sentence) why your answer makes physical sense. You can ignore the difference in partial pressures for this problem. TABLE 10.2 VAPOR PRESSURE OF WATER TEMPERATURE ("C) PRESSURE (mm Hg) TEMPERATURE ("c) PRESSURE (mm Hg) 6.5 55 118.0 10 9.2 60 149.4 15 12.8 65 187.5 20 17.5 70 233.7 25 23.8 75 289.1 30 31.8 80 355.1 35 41.2 85 433.6 40 55.3 90 525.8 45 71.9 95 633.9

Hydrogen peroxide is decomposed in a lab and the produced O2 (g) is collected over water at 15.0 °C. Molar masses: H2O2 = 34.02 g/mol, H2O = 18.02 g/mol, O2 = 32.00 g/mol. 2 H2O2 () → 2 H20 () + O2 (g) a) Calculate the moles of O2 (g) collected if the total pressure of the gas is 780. mmHg and the volume of gas is 0.4000 L. Assume all gases are ideal. b) What volume of pure hydrogen peroxide (density = 1.530 g/mL) decomposed? Assume that the decomposition reaction is complete. If you were unable to answer part (a), assume that 1 mol of O2 (g) was collected. c) If the collected gas (H2O (g) + O2 (g)) is transferred into a rubber balloon (which contains tiny pores), which gas will effuse out more quickly? Briefly explain (in about 1 sentence) why your answer makes physical sense. You can ignore the difference in partial pressures for this problem. TABLE 10.2 VAPOR PRESSURE OF WATER TEMPERATURE ("C) PRESSURE (mm Hg) TEMPERATURE ("c) PRESSURE (mm Hg) 6.5 55 118.0 10 9.2 60 149.4 15 12.8 65 187.5 20 17.5 70 233.7 25 23.8 75 289.1 30 31.8 80 355.1 35 41.2 85 433.6 40 55.3 90 525.8 45 71.9 95 633.9

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

Butane, C4H10C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l)2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.00 atmatm and 23 ∘C∘C, what is the volume of carbon dioxide formed by the combustion of 2.00 gg of butane?
The Apollo 13 mission astronauts are running out of oxygen and need to get rid of the excess carbon dioxide. You know that sodium hydroxide can remove carbon dioxide from the spacecraft cabin. The filter which they had been using is fully saturated and no longer works. The astronauts have a 5 kg container of sodium hydroxide on the ship. The reaction to neutralize the air, remove carbon dioxide with sodium hydroxide is shown below CO2(g) + 2NaOH(s) ⟶⟶ Na2CO3(aq) + H2O(l) The astronauts have 2 days left before they land on earth. You know that there are three astronauts, and each astronaut emits roughly 500. g of carbon dioxide each day. Is there enough sodium hydroxide in the cabin to cleanse the cabin air of the carbon dioxide, or are the astronauts doomed? Calculate how much sodium hydroxide is required to remove all the carbon dioxide from the three astronauts. Be sure to show all your work!
6. Consider the following chemical reaction: 2 Cr(OH)3(aq) >Cr₂O3(s) + 3H₂0(1) 12.00 moles of chromium (III) hydroxide is decomposed. Calculate moles of the water produced. O 18.00 moles O 1.500 moles O 4.00 moles O 12.00 moles
Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite, involves a two-step process. In the first step, manganese (II) carbonate and oxygen react to form manganese (IV) oxide and carbon dioxide: 2 MnCO3(s) + O₂(g) 2 MnO₂ (s) +2 CO₂(g) In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxide: 3 MnO₂(s) +4 Al(s)-3 Mn(s) +2 Al₂O3(s) Write the net chemical equation for the production of manganese from manganese (II) carbonate, oxygen and aluminum. Be sure your equation is balanced. ol 41
Name: 14. The following reaction occurs and 9.81 x 1025 CO, molecules are produced. C6H12O6 (s) + O₂(g) → CO₂(g) + H₂O(1) How many kilograms of O₂ is required? © 2021 F'21/S'22 NetID: Chemistry I A: 5.21 WORKSH 83
The balanced equation for the decomposition of potassium chlorate is shown below. When carried out in lab, this reaction is found to produce 1.2 g of potassium chloride. For your convenience, the molar mass of each substance is shown below their formulas (in purple). Use this Information to make the requested calculation: 2 KCIO3(s) -> 2 KCI(s) + 3 02(g) 122.551 74.551 32 Determine the percent yield if the reaction consumes 0.50 kg of potassium chlorate:
For the reaction between solid tetraphosphorus trisulfide andoxygen gas to form solid tetraphosphorus decaoxide and sulfurdioxide gas, write a balanced equation. Show the equation in terms of (a) molecules, (b) moles, and (c) grams
Ammonium nitrate has been used as a high explosive because it is unstable and decomposes into several gaseous substances. The rapid expansion of the gaseous substances produces the explosive force. NH,NO3 (8) → N2 (g)+ O2 (g) + H2O(g) Calculate the mass of each product gas if 47.4 g of ammonium nitrate reacts. g N2 g O2 g H2O
Suppose a 500. mL flask is filled with 0.10 mol of CO, 1.3 mol of H₂O and 1.5 mol of H₂. This reaction becomes possible: CO(g) + H₂O(g) → CO₂(g) + H₂(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of CO2. You can leave out the M symbol for molarity. initial change equilibrium CO 0 H₂O 0 CO2 0 X 0 H₂ 0 0/0 X Ś
Suppose a 250. mL flask is filled with 1.0 mol of CO, 0.70 mol of H₂O and 2.0 mol of H₂. This reaction becomes possible: CO(g) + H₂O(g) CO₂(g) + H₂(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of CO₂. You can leave out the M symbol for molarity. initial change equilibrium 2 со 0 H₂O CO₂ X H₂ 0 X 5
15. Citric acid, C6H807 (aq), is often used as an additive to make candies "sour. a. Draw a flowchart that shows how to caloulate the molar mass of citric acid, b. Verify the steps in your flowchart by calculating the molar mass of citric acid.
Silicon tetrachloride (SICI4 ) can be prepared by heating Si in chlorine gas: Si(s) + 2C12(g) -> SiCI4(1) In one reaction, 0.507 mole of SiCI4 is produced. What mass (grams) of molecular chlorine were used in the reaction? Choose the nearest answer. MW SICI4 = 169.9 g/mol; MW Cl = 35.453 g/mol A 63 grams B 27 grams 72 grams D 36 grams