9.1 Calculate the total mass of the reactants and the products for each of the following equations: a. 2SO₂(g) + O₂(g) →→→2SO3(g) 2P₂O5(s) b. 4P(s) + 50₂(g) TW ho

3. Determine the enthalpy change (AH₂) for the final reaction below. a. CO(g) + ½ O₂(g) → CO₂(g) AH, -67.6 kcal b. N₂(g) + O₂(g) →→→ 2NO(g) AH₂ = 43.2 kcal c. CO(g) + NO(g) →→→ CO₂(g) + ¹½ N₂(g) AH₂ = ?

1)isothermic,exothermic, or endothermic 2)combustion,descombotion,synthesis,acid-base,double replacement,or single replacement

The metal widely used in our civilization is iron (Fe) and it is obtained industrially by the reduction of iron oxide (Fe,0,) with carbon at higher temperatures (over 1000 °C). The equation for the reaction is as follows, Fe,0;(s) + C(s) –Fe(s) + CO2(g) Using the above equation, a. What is the number of moles of Fe? (ensure 3 decimal places for e.g. 0.300) mols b. How much of the product (Fe) can be produced from 10.0g of Fe,O;?(ensure 2 decimal places for e.g. 0.30) c. What is the number of moles for carbon?(ensure only 4 decimal places) (ensure 4 decimal places for e.g. 0.3003) mols bo

9. One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III) hydroxide from a solution containing rhodium(III) sulfate according to the following chemical equation: (Be sure to balance the reaction equation) Rh₂(SO4)3(aq) + NaOH(aq) - Rh(OH)³(s) + Na₂SO4(aq) If 69.28 g of rhodium(III) hydroxide is to be produced, what mass of rhodium(III) sulfate will be needed for the reaction?

5. When 5.0 moles of potassium metal reacts with an excess of H₂0, 3.5 g of H2 are produced. 2 K (s) + 2 H20 (1) 2 KOH (aq) H₂ (g) a. Calculate the number of moles of water needed to react with all of the potassium metal. (Ans: 5 mol) + b. Calculate the theoretical yield of H2, in grams, formed when all 5.0 moles of potassium metal are consumed. (Ans: 5.04 g) c. Calculate the percent yield of the reaction, given 3.5 g (actual yield) are produced. (Ans: 69.4%)

Chlorine is used by textile manufacturers to bleach cloth. Excess chlorine is destroyed by its reaction with sodium thiosulfate, Na2S2O3, as follows:Na2S2O3(aq) + 4Cl2(g) + 5H2O  2NaHSO4(aq) + 8HCl(aq)   Using the concepts established in the previous parts, answer the following questions about the following reaction:The octane in gasoline burns according to the following equation:2C8H18 + 25O2 → 16CO2 + 18H2O(a) How many moles of O2 are needed to react fully with 6.84 mol of octane?   (b) How many moles of CO2 can form from 0.511 mol of octane?   (c) How many moles of water are produced by the combustion of 8.20 mol of octane?   (d) If this reaction is used to synthesize 6.00 mol of CO2, how many moles of oxygen are needed? How many moles of octane are needed?    ? mol O2 ? mol C8H18   Thanks.

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esc 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: 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) 4 Write the net chemical equation for the production of phosphoric acid from phosphorus, oxygen and water. Be sure your equation is balanced. 0 Continue 56°F Clear F1 J F2 @ 2 F3 # 3 Q Search F4 $ 4 F5 % 5 F6 6 0-0 X F7 & 00 7 Ś F8 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibi M OO DELL F9 prt sc F10 home F11 end 12 F12 0 Submit Assignment J olo 18 Ar insert

Consider the following balanced reaction.  How many grams of water are required to form 75.9 g of HNO3?  Assume there is excess NO2 present.  The molar masses are as follows:  H2O = 18.02 g/mol, HNO3 = 63.02 g/mol.                3 NO2 (g) + H2O (l)  ⟶2 HNO3 (aq) + NO (g) Group of answer choices