70 g of benzene (C6H6) is reacted with extess hydroach to produce tyclohexane (C6H12) according to...

Question

Question

science chemistry

Answer 1

Answer #1

no of moles = mass / molar mass

for C6H6 = 78 g / 78.11 g/mol => 0.99859 moles

C6H6 + 3 H2 -----------------------> C6H12

from the equation

1 mol C6H6 ----------------> 1 mol C6H12

0.99859 mol ------------------->?

=> 0.99859 * 1 / 1

=> 0.99859 moles

theoretical yield = 0.99859 mol * 84.16 g/mol => 84.0414 grams

percent yield = actual yield / theoretical yield * 100

percent yield = 42 / 84.0414 * 100 => 49.975 %

answer => c ) 50%

Add a comment

Answer 2

Similar Homework Help Questions

Cyclohexane is manufactured from the reaction of benzene with hydrogen: C6H6(g) + 3 H2(g) → C6H12(g)...

Cyclohexane is manufactured from the reaction of benzene with hydrogen: C6H6(g) + 3 H2(g) → C6H12(g) If the initial concentration of hydrogen was 1.5 M and 5 minutes later the hydrogen concentration is 0.34 M, what is the average rate of appearance of cyclohexane? 0.39 M/min 7.7 x 10-2M/min 4.6 M/s 3.9 x 10- 2M/hr 2.3 M/min
If 2.73 mol of benzene, C6H6, are reacted with excess oxygen according to 2C6H6+1502- 12CO2 +...

If 2.73 mol of benzene, C6H6, are reacted with excess oxygen according to 2C6H6+1502- 12CO2 + 6H20 How many grams of CO2 are produced? (Enter your answer to the hundredth place.)
When benzene C6H6 reacts with bromine Br2, bromobenzene C6H5Br is obtained: C6H6 + Br2 --> C6H5Br...

When benzene C6H6 reacts with bromine Br2, bromobenzene C6H5Br is obtained: C6H6 + Br2 --> C6H5Br + HBr (balanced already) When 15.0 g of benzene reacts with excess Br2, 0.19 mole of bromobenzene C6H5Br was produced? IF the actual yield was 42.3 g of C6H5Br produced, Calculate the percent yield.

A 31.2 gram sample of C6H6 (benzene) is reacted with excess HNO3 (nitric acid). 36.0 grams...

A 31.2 gram sample of C6H6 (benzene) is reacted with excess HNO3 (nitric acid). 36.0 grams of the desired product, nitrobenzene C6H5NO2, is isolated from this reaction. Water is the by-product. A. Write a balanced chemical equation for this reaction B. What is the percent yield of nitrobenzene?
5.0g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the...

5.0g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below. Which one of the following statements is false? N2 (g) + 3 H2 (g) > 2 NH3 (g) A) 2.8 grams of hydrogen are left over. B) Nitrogen is the limiting reactant C) The theoretical yield of ammonia is 6.1 g D) Hydrogen is the excess reactant
6. Cyclohexane reacts with oxygen to produce carbon dioxide and water by the following balanced chemical...

6. Cyclohexane reacts with oxygen to produce carbon dioxide and water by the following balanced chemical reaction. (3 points for a and c, 4 points for b, 10 ibe points total) w woled eldste ante 591 dl to sa serta s) meri C6H12(e) + 9 O2(g) →6 CO2 (9) + 6 H2O (9) ginged a. If 79.0 grams of O2 is reacted with 41.8 grams of C6H12, which is the limiting reagent? Limiting reagent b. How many grams of H20...

5.00 g CaH2 reacted with 6.00 g H2O in the reaction below. Calculate the % yield...

5.00 g CaH2 reacted with 6.00 g H2O in the reaction below. Calculate the % yield of H2 if a mass of 0.20 grams was collected after the reaction. CaHz(s) + 2H20(1) - Ca(OH)2(aq) + 2H2(g) 30% 42% 60% 84% 240%
6. Cyclohexane reacts with oxygen to produce carbon dioxide and water by the following balanced chemical...

6. Cyclohexane reacts with oxygen to produce carbon dioxide and water by the following balanced chemical reaction. (3 points for a and c, 4 points for b. 10 points total) CoH12(C) + 9 O2 (g) - 6 CO2 (g) + 6 H20 (0)" a. If 79.0 grams of O2 is reacted with 41.8 grams of C6H12, which is the limiting reagent? Limiting reagent b. How many grams of H20 will be produced? Grams C. If 7.2 grams of H20 are...
10 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to...

10 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below. Which one of the following statements is false? N2(g)+3H2(g)-> 2NH3(g) I know the answer is " The theoretical yield of ammonia is 15 g. but I want see the WORK Thank you !

QUESTION 4 When 81.8 g carbon disulfide was reacted with excess sodium hydroxide, according to the...

QUESTION 4 When 81.8 g carbon disulfide was reacted with excess sodium hydroxide, according to the following equation, 93.9 grams of Na2CS3 was produced. What was % yield of Na2CS3? 3 CS2+ NaOH - 2 Na2CS3 + Na2CO3 + 3H20 percent yield =(actual yield/ theoretical yield) x 100