Chemistry

sulfuric acid can be prepared by a multistep process summarized as: 2 SO2 + O2 + 2 H2O--> 2 H2SO4 What mass of sulfuric acid could be produced daily by a process using 38 kg per day of sulfuric dioxide with a 70% conversion efficiency ("yield"), assuming that sulfuric dioxide is the limiting reagent

I don't know how to get this answer. someone help!

1. 👍
2. 👎
3. 👁
1. mols SO2 = 38000/molar mass SO2 = ?
mols H2SO4 produced = same as mols SO2 becaue 2 mol SO2 = 2 mol H2SO4.
Then grams H2SO4 = mols H2SO4 x molar mass H2SO4 = ? g, then convert to kg. That's if the process were 100% efficiency. It isn't so that answer x 0.70 = the amount produced at 70% efficiency.

1. 👍
2. 👎

Similar Questions

1. chemistry

In the reaction CaO(s) + SO2(g) ---> CaSO3(s) (Hint: try drawing the Lewis structures of SO2 and SO32-) a. ) Ca2+ acts as a Lewis base, and SO32- acts as a Lewis acid. b. ) SO32- acts as a Lewis base, and SO2 acts as a Lewis acid.

2. Chemistry

Sulfur dioxide (SO2) is an unwelcome result of burning soft coal in power plants. Some of the SO2 ends up as sulfuric acid in acid precipitation. The net reaction is 2 SO2(g) + O2(g) + 2 H2O(ℓ) −→ 2 H2SO4(ℓ) What mass in

3. chemistry

The reaction SO2 + H2O =H2SO4 Is the last step in the commercial production of sulfuric acid . the enthalpy change for this reaction is -227 KJ . In designing a sulfuric acid plant is it necessary to provide for heating or cooling

4. chemistry

What is the mole fraction of sulfuric acid in a solution made by adding 3.4 grams of sulfuric acid to 3500 mL of water?

1. Chemistry

Acid Question!? An unusual category of acids known as superacids, which are defined as any acid stronger than 100% sulfuric acid, can be prepared by seemingly simple reactions similar to the one below. In this example, the

2. Gen Chem 1

A tanker truck carrying 2.01×10^3kg of concentrated sulfuric acid solution tips over and spills its load. The sulfuic acid is 95.0% H2SO4 by mass and has a density of 1.84g/L. Sodium Carbonate (Na2CO3)is used to neutralize the

3. chemistry

Sulfuric acid (H2SO4) is prepared commercially from elemental sulfur using the contact process. In a typical sequence of reactions, the sulfur is ﬁrst burned: S + O2 → SO2 , then it is converted to SO3 using a catalyst: 2 SO2

4. chem

which one of the following statements about sulfuric acid is correct? A. sulfuric acid is a known muriatic acid B. sulfuric acid is a strong oxidizing agent C. sulfuric acid has little effect on metals D. sulfuric acid is

1. Chemistry

Sulfur dioxide is used to make sulfuric acid. one method of producing it is by roasting mineral sulfides, for example, FeS2(s) + O2 (g) ---> SO2(g) + Fe2O3(s) (unbalanced). A production error leads to the sulfide being placed in a

2. Chemistry

In the formation of acid rain, sulfur dioxide reacts with oxygen and water in the air to form sulfuric acid. Write the balanced chemical equation for the reaction. 2 SO2 + 1 O2 + 2 H2O --> 2 H2SO4 If 5.45 g SO2 react with excess

3. chemistry 112

the formation of SO3 from so2 and o2 is an intermediate step in the manufacture of sulfuric acid, and it is also responsible for the acid rain phenomenon. the equilibrium constant Kp for the reaction is 0.13 at 830 degree celcius.

4. chemistry

Sulfuric acid (H2SO4) is prepared commercially from elemental sulfur using the contact process. In a typical sequence of reactions, the sulfur is ﬁrst burned: S + O2 → SO2 , then it is converted to SO3 using a catalyst: 2 SO2