Sulfuric acid, H2SO4, is an important industrial chemical, typically synthesized in a multi-step process. What is...
Sulfuric acid, H2SO4, is an important industrial chemical, typically synthesized in a multi-step process. What is the percent yield if a batch of H2SO4 has a theoretical yield of 3.3 kg, and 2.7 kg are obtained at the end of the process?
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Sulfuric acid, H2SO4, is an important industrial chemical,
typically synthesized in a multi-step process. What is...
Question 6 1 pts Suppose you are measuring the mass of a solid sample on a...
Question 6 1 pts Suppose you are measuring the mass of a solid sample on a balance using a weigh boat. You record the data in a table. Mass of weigh boat 3.117 g Mass of weigh boat and sample 9.405 g What is the mass, in grams, of the solid sample? Question 7 2 pts Sulfuric acid, H2SO4, is an important industrial chemical (typically used for fertilizers and making of many other chemicals), typically synthesized in a multi-step process....
12 Sulfuric acid is a very important is a good of its induni ommodity chemical., anod...
12 Sulfuric acid is a very important is a good of its induni ommodity chemical., anod indeed, a nationfr fertl or an array of applications including: detergents. Most of the Sulfuric scid is process used to make sulfuric acid is shown below: (12 th Sulfuric scid is used for fe treatment Step 1 Step 2 1r 42.59 g of Hs . How many moles of which reactant were in excess? was reacted with 56.0 g of O: (7 pts.) O,...
9. Sulfuric acid (H2SO4), the industrial chemical produced in greatest quantity (almost 45 million tons per year in the...
9. Sulfuric acid (H2SO4), the industrial chemical produced in greatest quantity (almost 45 million tons per year in the United States alone), is prepared by the following chemical reaction in the presence of a catalyst 2S (s) + 302 (g) + 2H2O (1) - 2H2SO4 (aq) What volume of Oz (in liters) at 22 ° C and 0. 95 atm is required to produce 454 g of H2SO4?
plesae ASAP The contact process for producing sulfuric acid is: Sg(s) + 8 O2(g) — 2...
plesae ASAP
The contact process for producing sulfuric acid is: Sg(s) + 8 O2(g) — 2 SO2(g) + O2(g) SO3(g) + H2O(l) 8 SO2(g) +2 SO3(g) H2SO4(aq) each step has a percent yield of 77.1%, how many grams of Sg are needed to produce 1.50 kg sulfuric acid? 637 g 1.07*10^3 g 378 9 2.25*10^3 g 0 212 g
Balance the chemical equation for the important industrial process: C2H4 + O2 + HCl → C2H4Cl2...
Balance the chemical equation for the important industrial process: C2H4 + O2 + HCl → C2H4Cl2 + H2O. Given 525.0 kg of hydrochloric acid, calculate how many kg of C2H4Cl2 can be produced.
23. An important intermediate reaction in the industrial production process of nitric acid is shown. What...
23. An important intermediate reaction in the industrial production process of nitric acid is shown. What is the theoretical yield of H2O (18.02 g/mol) if 45.0 kg of NH3 (17.04 g/mol) reacts with excess O2 (32.00 g/mol)? NH3(g) + O2(g) → NO(g) + H2O (1) 24. A 10.00 g sample of a hydrocarbon (which is a compound that contains only carbon and hydrogen) was burned in oxygen, and the carbon dioxide and water produced were carefully collected and weighed. The...
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts...
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H2(g)+N2(g)→2NH3(g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. 1.43 g H2 is allowed to react with 9.70 g N2, producing 2.31 g NH3. Part A: What...
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts...
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H2(g)+N2(g)→2NH3(g)3H2(g)+N2(g)→2NH3(g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. 1.36 g H2 is allowed to react with 9.75 g N2, producing 1.75 g NH3 What is the...
The Haber-Bosch process is a very important industrial process. In the Haber Process, hydrogen gas reacts...
The Haber-Bosch process is a very important industrial process. In the Haber Process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H2(g) + N2(g) ---> 2NH3(g) The ammonia produced in the Haber process has a wide range of uses from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation. 1.57 g H2 is allowed to react with 9.87 g N2, producing 1.69 g Nh3....
Nitric acid is produced commercially by a multi-step process, starting from the oxidation of ammonia. If...
Nitric acid is produced commercially by a multi-step process, starting from the oxidation of ammonia. If the % yield of each step is as shown (Step 1.) 4NH3(g) + 502(g)-→ 4N0(g) + 6H20(1) 94.9% yield Step 272NO(g) +02(g) 2NO2(g) 85.6% yield Step 3*) 3NO2(g) + H20(I)-> 2 HNO3(l) + NO(g) 80.4%yield How much ammonia (in kg) of ammonia must be input at the start of the reaction to produce 7.0kg of nitric acid.
Question 6 1 pts Suppose you are measuring the mass of a solid sample on a balance using a weigh boat. You record the data in a table. Mass of weigh boat 3.117 g Mass of weigh boat and sample 9.405 g What is the mass, in grams, of the solid sample? Question 7 2 pts Sulfuric acid, H2SO4, is an important industrial chemical (typically used for fertilizers and making of many other chemicals), typically synthesized in a multi-step process....
12 Sulfuric acid is a very important is a good of its induni ommodity chemical., anod indeed, a nationfr fertl or an array of applications including: detergents. Most of the Sulfuric scid is process used to make sulfuric acid is shown below: (12 th Sulfuric scid is used for fe treatment Step 1 Step 2 1r 42.59 g of Hs . How many moles of which reactant were in excess? was reacted with 56.0 g of O: (7 pts.) O,...
plesae ASAP
The contact process for producing sulfuric acid is: Sg(s) + 8 O2(g) — 2 SO2(g) + O2(g) SO3(g) + H2O(l) 8 SO2(g) +2 SO3(g) H2SO4(aq) each step has a percent yield of 77.1%, how many grams of Sg are needed to produce 1.50 kg sulfuric acid? 637 g 1.07*10^3 g 378 9 2.25*10^3 g 0 212 g
23. An important intermediate reaction in the industrial production process of nitric acid is shown. What is the theoretical yield of H2O (18.02 g/mol) if 45.0 kg of NH3 (17.04 g/mol) reacts with excess O2 (32.00 g/mol)? NH3(g) + O2(g) → NO(g) + H2O (1) 24. A 10.00 g sample of a hydrocarbon (which is a compound that contains only carbon and hydrogen) was burned in oxygen, and the carbon dioxide and water produced were carefully collected and weighed. The...
Nitric acid is produced commercially by a multi-step process, starting from the oxidation of ammonia. If the % yield of each step is as shown (Step 1.) 4NH3(g) + 502(g)-→ 4N0(g) + 6H20(1) 94.9% yield Step 272NO(g) +02(g) 2NO2(g) 85.6% yield Step 3*) 3NO2(g) + H20(I)-> 2 HNO3(l) + NO(g) 80.4%yield How much ammonia (in kg) of ammonia must be input at the start of the reaction to produce 7.0kg of nitric acid.
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