2. An important source of hydrogen and oxygen, used as rocket fuels, is the decomposition of water by electrical energy: H20 (1) -> H2 (g) O2 (g) What mass of water is needed to produce 84.56 g of hydrogen? How many grams of oxygen would be produced as a byproduct of the above reaction? How many tons of water would be needed to produce 46.3 tons of hydrogen? (1 ton 2000 lb)

8. Consider the following chemical reaction: 4 HBr(g) + O2(g) → 2 H2O(g) + 2 Br2(g) Identify the substance oxidized (SO), the substance reduced (SR), the oxidizing agent (OA) and the reducing agent (RA). SO: SR: OA: RA: 9. Lead (II) iodide is a bright yellow pigment made from the precipitation reaction between solutions of lead (II) nitrate and sodium iodide. a. Write the balanced equation for the precipitation reaction. b. If 19.6 g of lead (II) nitrate are mixed with 25.3 g of sodium iodide, what is the limiting reactant? Calculate and explain. С. How many grams of precipitate are formed? d. If 35.1 g of product is recovered in lab, what is the percent yield for this reaction?

Ethanol (C,H O) is combusted in air according to the following reaction: C,H,O(1) + O,(g) –→ CO,(g) + H,0(I) How many grams of water would be produced by the complete combustion of 5.07 moles of ethanol in the presence of excess oxygen? + MacBook Pro 888 こニ。 esc & # $ @ 7 2 3 4 R Y Q W E ab F А lock C V option command ontrol cの つ つ エ

???

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

Q5. Saponification is a process in which soap is produced from the chemical reaction between animal fat (triglycerides) and a strong base such as KOH. An example of such a balanced chemical reaction is shown here: C51H98O6 + 3KOH → (Triglycerides ) C3H5(OH)3 + 3C16H31O2K ( Soap) If, during the saponification reaction, 231.5 g of C51H98O6 is mixed with 231.5 g of KOH and 160 g of soap is produced: * a. Calculate the theoretical yield of soap, C16H31O2K, and indicate which is the limiting reactant. (5) (Provide your answer to 2 decimal places) * b. Calculate the percent yield for this reaction (1) (Provide your answer to 1 decimal place) *Show ALL steps and mathematical equations involved in your calculations to help the orgo students. Remember to label all steps clearly and

Answer the questions about the balanced reaction 3A + 2B The molar masses are as follows: A = 10. g B = 20. g How many calories are evolved when 5.71 g of B is consumed? mol B (5.71 g B)(-- t. yes g B u. no mol B)(-- cal mol B Is the relationship between moles of B and calories a direct proportion? a. 0 b. 1 c. 2 d. 3 e. 4 f. 5 h. 7 k. 30 1.70 m. 100 n. 0.143 o. 14.3 S. 5.71 1 C + 100. cal C = 70. g g. 6 p. 0.286 mol B i. 10 9. 0.429 j. 20 r. 4.29 cal

Please balance

Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming of natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3 H₂(g) 2 NH₂ (9) In the second step, ammonia and oxygen react to form nitric acid and water: NH₂(g)+20₂(g) →HNO3(9)+H₂O(g) Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced. 0 Explanation Check 0-0 00 7² X S MacBook Air © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center

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