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-stepthermal process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide:PĄ(1)+50,(9)→2P,03(9)In the second step, diphosphorus pentoxide and water react to form phosphoric acid:P2O3(9)+3 H,O(1)→2H;PO,()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: PĄ(1)+50,(9)→2P2Og(9) In the second step, diphosphorus pentoxide and water react to form phosphoric acid: P,0,(9)+3 H,O(1)→2H,PO,(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: PĄ(1)+50,(9)→2P2Og(9) In the second step, diphosphorus pentoxide and water react to form phosphoric acid: P,0,(9)+3 H,O(1)→2H,PO,(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...

See similar textbooks

Similar questions

Energy for recycling Cu: ________ kJ
Calculate the standard enthalpy of reaction, deltaxnHo , at 25 oC for the formation of glucose from carbon dioxide and water (shown below). 6CO2 (g) + 6H2O(l) -> C6H12O6 (s) + 6O2 (g)
2 ·als NaOH, H ethanol heat
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.
22) Given the following reactions 2NO → N2 + 02 2NO+O2 → 2NO2 the enthalpy of the reaction of nitrogen with oxygen to produce nitrogen dioxide N2+202 → 2NO2 is A. -68 B. 68 C. -292 D.) 292 AH = -180 kJ AH = -112 kJ kJ.
The process of flambéing involves pouring liqueur on food for flavor. This addition to desserts adds tons of flavor, (C₂H5OH), which combusts in the presence of immense heat. You may have noticed this in restaurants, chemical equation for the combustion of ethanol as a reference in this assessment. C₂H₂OH (1) +30, (g) 2 CO₂ (g) + 3 H₂0 (g) Use the graph above to explain if the combustion of ethanol is exothermic or endothermic
Consider the combustion of liquid C₅H₈ in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of C₅H₈ is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.634 °C. What quantity in moles of C₅H₈ were burned?
How much heat is released when an excess of Fe reacts with 48 g of 02 (M = 32 g/mol), according to the following reaction: 4Fe(s) + 302(8) → 2Fe,O3(s) AH = -1652 kJ 826 kJ O 1041 kJ O 2478 kJ O 1652 KJ
If AH for the reaction 2 HgO → 2 Hg (1) + O2 (g) is 181.66 kJ, (s) then AH for the reaction + ½ O2 (g) → HgO Hg (1) (s) is:
4. When 1.00 L of 1.05 M Ba(NO3)2 solution is mixed with 1.00 L of 1.10 M NazSO4 solution at 25.0°C in a coffee-cup calorimeter. The reaction is Ba(NOs)2(aq) + NazSO4(aq) → BaSO4(s) + 2NANO:(aq). The final temperature of the mixture increases to 28.1°C. Calculate the enthalpy change per mole for this process. (Assuming C=4.18 J °C' g' and density of the final solution is 1.05 g/ml).
6) A block of rhenium metal (specific heat =0.0329 cal/ gC) is heated to 88.2C and then dropped into 100.0 g of water initially at 26.4 C. The final temperature of the mixture is 32.4C. What was the mass of the block of rhenium?
The heat of reaction for the reaction A + 2B → 2C is 1200. kJ.The heat of reaction for the reaction B + D → C is 150. kJ.Using Hess's Law, calculate the heat of reaction for the reaction A → 2D.