Concept explainers
(a)
Interpretation : The theoretical yield of oxygen gas should be calculated.
Concept Introduction : The actual yield of the product is the amount of product which is formed at the end of reaction experimentally whereas theoretical yield represents the amount of product calculated by expecting that 100 % of reactant changes to product. The percent yield can be shown as:
(b)
Interpretation : The percent yield of the oxygen gas should be calculated.
Concept Introduction : The actual yield of the product is the amount of product which is formed at the end of reaction experimentally whereas theoretical yield represents the amount of product calculated by expecting that 100 % of reactant changes to product. The percent yield can be shown as:
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- Ke lo %24 3. Ss I u b 2 4. #3 5 9. 7. 8. 6. IIO mol NO How many moles of NO are formed from 2.1 moles of N,? Use the balanced equation for the reaction of N, and O, to form NO to answer the question. (6)0 + (6)N Enter your answer in the provided box. → 2 NO(g)arrow_forward5. 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%)arrow_forwardWrite the net ionic equation for the reaction of silver chloride with hydrogen sulfide gas. AgCl(s)+ H2S(g) ⟶ Ag2S(s)+ H+1(aq) + Cl-1(aq) 2AgCl(s)+ H2S(g) ⟶ Ag2S(s)+ 2H+1(aq) + 2Cl-1(aq) 2AgCl(s)+ H2S(g) ⟶ Ag2S(s)+ 2HCl(aq) 2Ag+1(aq)+ S-2(aq) ⟶ Ag2S(s) 2AgCl(s)+ 2H+1(aq) ⟶ 2Ag+1(aq)+ 2HCl(aq)arrow_forward
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- If the yield for the following reaction is 72.0%, how many grams of Al should be used to produce 15.0 g of Al2(SO4)3? [Molar mass of Al2(SO4)3 = 342.17 g/mol] Al(s) + H2SO4(aq) Al2(SO4)3(aq) + H2(g) 11- 11arrow_forwardNitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by réforming of natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N2(9)+3 H,(g)→2NH;(g) In the second step, ammonia and oxygen react to form nitric acid and water: NH;(g)+2O,(9)→HNO,(g)+H,O(g) Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced. Explanation Check O2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility 2:53 PM 4/8/2022 DELL PrtScr Insert Delete PgUp PgDn F7 F8 F9 F10 F11 F12 Esc F1 F2 F3 F4 F5 F6 Fn Num 24 & ( ) Lock Backspace 1 2 6. 7 + II * 00 %#3arrow_forward6.(0-2) Black powder was invented in China in the 9th century. It was used as an explosive with propelling properties. Today it is used in fireworks, model rocket engines, and replica black powder weapons. Black powder consists of potassium nitrate (potassium nitrate, KN03), charcoal and sulfur. A variety of chemical reactions take place when this mixture is exploded. One of these is shown below. 2KNO, +S+ 30 → K, S+N, ↑+3C0, 1 Knowing that carbon makes up 15% of the black powder, calculate the total volume of gases (under normal conditions) released when 0.1 kg of black powder explodes. Assume that only the chemical reaction given above occurs.arrow_forward
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