escPhosphoric acid, which is commonly used as rust inhibitor, food additive and etching agent for dental and orthopedic use, can besynthesized using a two-step thermal process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide:P₁(1)+50₂(g) 2 P₂O(g)In the second step, diphosphorus pentoxide and water react to form phosphoric acid:P₂O(g) + 3 H₂O(1)-2 H₂PO₂(0)4Write the net chemical equation for the production of phosphoric acid from phosphorus, oxygen and water. Be sure your equation isbalanced.0Continue56°FClearF1JF2@2F3#3Q SearchF4$4F5%5F660-0XF7&007ŚF8© 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | AccessibiMOODELLF9prt scF10homeF11end12F120Submit AssignmentJolo18Arinsert

Balanced chemical equation is the equation in which equal number of atoms of each and every element…

Phosphoric acid, which is commonly used as rust inhibitor, food additive and etching agent for dental and orthopedic use, can be synthesized using a two-step thermal process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P4(1)+5O₂(g) 2 P₂O5(9) In the second step, diphosphorus pentoxide and water react to form phosphoric acid: P₂O5(9)+ 3 H₂O(1)-2H₂PO4(1) Write the net chemical equation for the production of phosphoric acid from phosphorus, oxygen and water. Be sure your equation is balanced.

Phosphoric acid, which is commonly used as rust inhibitor, food additive and etching agent for dental and orthopedic use, can be synthesized using a two-step thermal process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P4(1)+5O₂(g) 2 P₂O5(9) In the second step, diphosphorus pentoxide and water react to form phosphoric acid: P₂O5(9)+ 3 H₂O(1)-2H₂PO4(1) Write the net chemical equation for the production of phosphoric acid from phosphorus, oxygen and water. Be sure your equation is balanced.

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...

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200.0 mL of 0.200 M HNO3 is added to 200.0 mL of 0.200 M KOH in a coffee cup calorimeter. The neutralization reaction that occurs can be described by the chemical equation- HNO3(aq) + KOH(aq) → KNO3(aq) + H₂O(l) Before the solutions are mixed they are both at 23.00 °C. After the mixing of the solutions the temperature increases until it remains constant at 24.39 °C. Assuming no heat lost to the surroundings, how much heat was lost in this reaction? (Assume the specific heats and densities of the solutions is the same as water.)
Phosphoric acid, which is commonly used as rust inhibitor, food additive and etching agent for dental and orthopedic use, can be synthesized using a two-step thermal process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: PĄ()+50,(0)→2P,0;(9) In the second step, diphosphorus pentoxide and water react to form phosphoric acid: P,0,(9)+3 H,O(1)→2 H;PO,(1) Write the net chemical equation for the production of phosphoric acid from phosphorus, oxygen and water. Be sure your equation is balanced.
Consider the reaction, C2H4(g) + H2(g) → C2H6(g), where ΔH = –137 kJ. How many kilojoules are released when 3.5 mol of C2H4 reacts?
Section 5.6 You place 0.0750 g of magnesium chips in a coffee-cup calorimeter and then add 100.0 mL of 1.00 M HCI. The reaction that occurs is: -> Mg (s) + 2 HCI (aq) → H2 (g) + MgCl2 (aq) The temperature of the solution raises from 20.15 °C to 23.29 °C. What is the enthalpy change or the reaction per mole of Mg? Assume that the specific heat capacity of the solution is 4.20 J/g K and the density of the solution is 1.00 g/mL. 412 kJ/mol 428 kJ/mol -412 kJ/mol -428 kJ/mol
Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3 H₂(g) → 2 NH3(g) ΔΗ= - 92. kJ In the second step, ammonia and oxygen react to form nitric acid and water: NH3(g) + 2O₂(g) → HNO3(g) + H₂O(g) ΔΗ= - 330. kJ Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ. ☐ kJ X 3
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2. A small immersion heater was used to heat water in an insulated cup. The heater was placed in 100.0 g of distilled water initially at 21.0°C, and turned on for 60.0 seconds while the water was stirred with a thermometer. The final temperature of the water was measured to be 37.5°C. Assume the specific heat capacity of the water is 4.18 J/g °C. (a) Calculate the total heat energy in joules absorbed by the water and the average power in watts (1 watt = 1 joule/s) delivered by the heater. The heater was used to deliver 3000 joules of energy to 100.0 g of methanol (CH,OH(E)) in the same manner. The temperature of the methanol increased by 11.8 Celsius degrees. (b) Calculate the specific heat capacity of the methanol liquid. (c) (i) Calculate the mass of water (H,O, Co= 4.181 Jgl °C-) at 20.0°C that would be requireć %3D to cool a 30.0-g block of copper (Cu, co0.385 J gl °C-l) from 50.0°C to 25.0°C in an insulated cup. %3D (ii) Which liquid, water or methanol, would be more effective as…
2. Calculate the amount of heat required to raise the temperature of 950.0 mL of a solution from 22.5 °C to 38.0 °C if the solution has a density of 1.04 g mL-l and a heat capacity of 4.08 J K-l g. 3. This reaction: CH4(g) + 202(g) → CO2(g) + 2H2O(1) produces 56.0 kJ of heat when 1.00 g of methane is burned. What is the molar heat of combustion for CH4? 4. In thermodynamics heat is represented by the letter 'q' and q is negative for processes which lose heat to the surroundings (i.e. exothermic processes). What is q for burning one mole of methane? 5. What mass of methane would need to be burned in order to generate the heat required to raise the temperature of the solution in question 2? (Hint: look at question 3 for some relevant data) 6. In this lab class you will measure the enthalpy change for hydrochloric acid reacting with sodium hydroxide. What effect, if any, would using nitric acid instead of hydrochloric acid have on the enthalpy changes measured in this experiment? Why?…
1. 25 g of sodium (Na) is put into 200 mL of water. The reaction between the two produces sodium hydroxide (NaOH) and hydrogen gas, and increases the temperature by 14 °C. (a) Calculate the enthalpy change, AH, of the reaction. (C; = 4.18 JºC•3; d= 1 g/mL) (b) Is this reaction endothermic or exothermic? (c) Based on your calculation, determine what is considered as the surrounding in this experiment.
The Haber process is used to manufacture ammonia from nitrogen and hydrogen in the presence of an iron catalyst. The reaction, shown in this equation, is exothermic: N 2 (g)+3H 2 (g) rightleftharpoons 2N*H_{3}(g) + Heat Which statement correctly describes the chemical reaction? The energy needed to break the chemical bonds of 1 mole of nitrogen and 3 moles of hydrogen is greater than the energy released by the formation of 3 moles of ammonia. The energy needed to break the chemical bonds of 1 mole of nitrogen and 3 moles of hydrogen is less than the energy released by the formation of 3 moles of ammonia. The energy released by breaking the chemical bonds of 1 mole of nitrogen and 3 moles of hydrogen is greater than the energy needed to form 3 moles of ammonia. The energy released by breaking the chemical bonds of 1 mole of nitrogen and 3 moles of hydrogen is less than the energy needed to form 3 moles of ammonia.
Train track rails are joined using an exothermic welding process. A mixture of iron (III) oxide (Fe2O3), and aluminium metal (Al) is employed and the process is described by the following chemical reaction: Fe₂O3(s) + 2Al(s) → Al₂O3(s) + 2Fe(s) AH (kJ mol-1) c(g-¹ K-1) 0 0.451 Fe(s) Fe₂O3(s) -822.3 0.651 0 0.900 Al(s) Al2O3(s) -1669.8 0.753 a) Calculate the heat released by this process. b) Assuming the reaction goes to completion and that all the heat goes into the final mixture, calculate the final temperature of the products before heat has flowed into the surroundings. Comment on whether the calculated temperature is reasonable. c) Calculate the entropy change for the surroundings once the system and surroundings have equilibrated to the surrounding temperature of 25 °C.