You are provided with 5.05g of SO2 to react with 2.45 gg of O2. Indicate your...

You are provided with 5.05g of SO2 to react with 2.45 gg of O2. Indicate your theoretical yield by completing the following statements.

Match the chemical formulas and amounts in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer.

The limiting reagent in the reaction is?

Regarding the theoretical yield based on the limiting reagent,(---------)mol of SO3 can be formed, which corresponds to a mass of ( --------)

The excess reagent was ( -------) and after the limiting reagent is consumed during the reaction, the mass of excess reagent remaining will be ( ----------)?

Solutions

Expert Solution

Dear student,

Please give positive rating to this answer.

With regards...

queen_honey_blossom answered 11 months ago

Next > < Previous

Related Solutions

Considering the initial reaction above where 2 mole of SO2 react with 1 mole of O2...

Considering the initial reaction above where 2 mole of SO2 react with 1 mole of O2 to produce 2 moles of SO3, if oxygen was introduced into the system after equilibrium is reached, we would expect that (circle one) [more products would form / more reactants would form / the concentrations would not change]. If argon gas was introduced into the system after equilibrium is reached, we would expect that (circle one) [more products would form / more reactants would...

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) Part A If 276.0 mL of SO2 is allowed to react...

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) Part A If 276.0 mL of SO2 is allowed to react with 161.4 mL of O2 (both measured at 327 K and 48.7 mmHg ), what is the limiting reactant? Part B What is the theoretical yield of SO3? nSO3 = Part C If 175.8 mL of SO3 is collected (measured at 327 K and 48.7 mmHg ), what is the percent yield for the reaction? Express your answer using four significant figures.

Consider the unbalanced reaction NiS2(s) + O2(g) --> NiO(s) + SO2(g). When 11.2g of NiS2 react...

Consider the unbalanced reaction NiS2(s) + O2(g) --> NiO(s) + SO2(g). When 11.2g of NiS2 react with 5.43g of O2, 4.86g of NiO are obtained. The theoretical yield of Nio is? The limiting reactant is? The percentage yield is what percent?

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) 290.2 mL of SO2 is allowed to react with 151.8 mL...

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) 290.2 mL of SO2 is allowed to react with 151.8 mL of O2 (both measured at 318 K and 47.9 mmHg ), what is the limiting reactant? What is the theoretical yield of SO3? If 170.7 mL of SO3 is collected (measured at 318 K and 47.9 mmHg ), what is the percent yield for the reaction?

How does limestone react with SO2 to achieve removal of SO2 from exhaust gas stream?

For the following reaction, 2.45 grams of methane (CH4) are allowed to react with 26.8 grams...

For the following reaction, 2.45 grams of methane (CH4) are allowed to react with 26.8 grams of carbon tetrachloride. methane (CH4)(g) + carbon tetrachloride(g) ---> dichloromethane (CH2Cl2)(g) What is the maximum mass of dichloromethane (CH2Cl2) that can be formed? What is the formula for the limiting reagent? What mass of the excess reagent remains after the reaction is complete? in grams

For the balanced equation shown below, if the reaction of 24.3 grams of SO2 react with...

For the balanced equation shown below, if the reaction of 24.3 grams of SO2 react with 42.3 g of H2S producing 4.58 grams of sulfur, what is the percent yield? 2 H2S + SO2 → 3 S + 2 H2O

Sulfuric acid is produced by the following process: FeS2 + O2 → Fe2O3 + SO2...

Sulfuric acid is produced by the following process: FeS2 + O2 → Fe2O3 + SO2 SO2 + O2 → SO3 SO3 + H2O → H2SO4 Balance each reaction and then write a balanced net reaction. How many moles of O2 and H2O will be needed when 10.0 kg of FeS2 reacts completely?

For the system SO3 ( g) ⇔ SO2 (g ) + 1 2 O2 ( g)...

For the system SO3 ( g) ⇔ SO2 (g ) + 1 2 O2 ( g) at 1000 K, K = 0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. what is its partial pressure at equilibrium?

Enter your answer in the provided box. A sample of zinc metal is allowed to react...

Enter your answer in the provided box. A sample of zinc metal is allowed to react completely with an excess of hydrochloric acid: Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g) The hydrogen gas produced is collected over water at 25.0°C. The volume of the gas is 8.45 L, and the atmospheric pressure is 0.951 atm. Calculate the amount of zinc metal in grams consumed in the reaction. (Vapor pressure of water at 25°C = 23.8 mmHg.) ANSWER ____ g...

Subjects