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:P4(1)+5 0,(g)→2P,O;(9)In the second step, diphosphorus pentoxide and water react to form phosphoric acid:P,O;(9)+3 H,O(1)–→2H;PO4(1)Write the net chemical equation for the production of phosphoric acid from phosphorus, oxygen and water. Be sure your equation is balanced.

A chemical reaction can be added or subtracted like an algebraic equation.

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)+5 0,(g)→2P,0;(9) In the second step, diphosphorus pentoxide and water react to form phosphoric acid: P,0;(9)+3 H,O(1)–→2H;PO4(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)+5 0,(g)→2P,0;(9) In the second step, diphosphorus pentoxide and water react to form phosphoric acid: P,0;(9)+3 H,O(1)–→2H;PO4(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

Write a balanced equation and draw an approximate enthalpy diagram for each of the following changes: (a) the combustion of 1 mol of liquid methanol (CH₃OH); (b) the formation of 1 mol of nitrogen dioxide from its elements (heat is absorbed).
Consider the balanced chemical equation:2Al(s) + Fe2O3(s) -> 2Fe(s) + Al2O3(s)heat of reaction = −851.5 kJ (c) What mass of Fe2O3 must react to produce 387 kJ of heat? (d) What mass of Fe is produced at the same time 387 kJ of heat is produced?
A hand warmer packet contains a mixture of powdered iron, carbon, sodium chloride, sawdust, and zeolite, all moistened by a little water. The packet is activated by removing the plastic cover, which exposes the materials in the packet to air. The reaction that occurs is represented by the following equation. 4 Fe (s) + 3 O2(g) —> 2 Fe2O3(s) + 1648.4 kJ When 2.50 g of Fe2O3 (s) is produced in the hand-warmer packet, the energy transferred is (in kJ)___________ (Ans. 12.9 kJ)
on 22 of 22 Using the balanced chemical equation, determine how many moles of NaCl will be produced, if 0.381 mol of BaCl, is allowed to react with an excess of Na₂SO4. 20 moles of NaCl: Using the mole mass of NaCl: Using the moles of NaCl found in a previous question, determine how many formula units of NaCl can be produced. formula units: R F NaCl found in the previous question, determine how many grams of NaCl can be produced. V % 15 T G B ^ 6 MacBook Pro Y H N tv U ►II M MOSISO 9 O command P O Aa V { option [ + = } mol 1 S BAY ? delete
A student decides to find the molar enthalpy for the reaction between phosphoric acid and calcium hydroxide. They have a 0.250 M solution of Ca(OH)2, which they will use; they can only find a 2.9 M stock solution of H3PO4. If they want 200 mL of a 0.31 M solution of H3PO4, how many mL of the stock solution should they use to prepare their solution by diluting the stock? Give your answer to the nearest mL.
TRUE/FALSE: the following reaction is a formation reaction: 2C(s) + 4H2(g) → 2CH4(g)
P4.35
In 2001, Nescafé® launched a self-heating can of coffee, called Hot When You Want. To heat up the coffee, a button was pressed which mixed the heating ingredients in a shell outside the can containing the coffee. The can warmed up 210 cm³ of coffee by 40°C. A single step mixed calcium oxide and water to produce calcium hydroxide and generate heat according to the reaction: CaO (s) + H₂O (1) →→→ Ca(OH)2 (aq) AH = -82 kJ/mol J g-K' a. Assuming that the density and heat capacity for coffee is the same as that of water, 4.18- calculate the energy (in J) needed to warm 210 cm³ of coffee by 40°C. b. Use this value to hence calculate the minimum mass (in g) of CaO in the can for it to function as specified.
Concentrated sulfuric acid is 18.0 M. What volume is needed to prepare 1.0 L of 6.0 M sulfuric acid solution? Report your answer with 2 SF
I need help with 2 and 3
Write a balanced chemical equation for the standard formation reaction of liquid ethanol (C₂H5OH). 0-0 Xx
There are two steps in the usual industrial preparation of acrylic acid, the immediate precursor of several useful plastics. In the first step, calcium carbide and water react to form acetylene and calcium hydroxide: CaC,(s) + 2 H,0(g) → C,H,(9) + Ca(OH),(s) AH=-414. kJ In the second step, acetylene, carbon dioxide and water react to form acrylic acid: 6C,H2(g) + 3 C0,(g) + 4 H,O(g) → 5 CH,CHCO,H(g) AH=132. kJ Calculate the net change in enthalpy for the formation of one mole of acrylic acid from calcium carbide, water and carbon dioxide from these reactions. Round your answer to the nearest kJ. O kJ