Question

Given the reaction: N2 (g) + H2 (g) → NH3 (g). If 4.50 moles of hydrogen are reacted with excess nitrogen, how many moles of ammonia will be formed? Given the reaction: C4H8 (g) + O2 (g) → CO2 (g) + H2O (g). How many moles of carbon dioxide will be formed if 75.00 grams of C4H8 react with excess oxygen? A CEM 101 student was carrying out the following reaction for a lab experiment. K2CO3 (aq) + CaCl2 (aq) → 2 KCl (aq) + CaCO3 (s) Using the amount of potassium carbonate that they reacted with excess calcium chloride, they calculated 44.25 grams CaCO3 should be formed. They actually collected 38.68 grams of CaCO3. Calculate the student's percent yield and complete the results table below. (Theoretical yield, Actual yield, Percent yield) Given the reaction: Silver nitrate (aq) and potassium chloride (aq) yield silver chloride (s) and potassium nitrate (aq) a. Translate and balance the reaction b. If 84.95 grams of silver nitrate are reacted with excess potassium chloride, what is the theoretical yield of silver chloride? c. If 62.37 grams of silver chloride were actually produced, what was the percent yield? Name AgNO3

          Given the reaction: N2 (g) + H2 (g) → NH3 (g). If 4.50 moles of hydrogen are reacted with excess nitrogen, how many moles of ammonia will be formed?

Given the reaction: C4H8 (g) + O2 (g) → CO2 (g) + H2O (g). How many moles of carbon dioxide will be formed if 75.00 grams of C4H8 react with excess oxygen?

A CEM 101 student was carrying out the following reaction for a lab experiment. K2CO3 (aq) + CaCl2 (aq) → 2 KCl (aq) + CaCO3 (s) Using the amount of potassium carbonate that they reacted with excess calcium chloride, they calculated 44.25 grams CaCO3 should be formed. They actually collected 38.68 grams of CaCO3. Calculate the student's percent yield and complete the results table below. (Theoretical yield, Actual yield, Percent yield)

Given the reaction: Silver nitrate (aq) and potassium chloride (aq) yield silver chloride (s) and potassium nitrate (aq)
a. Translate and balance the reaction
b. If 84.95 grams of silver nitrate are reacted with excess potassium chloride, what is the theoretical yield of silver chloride?
c. If 62.37 grams of silver chloride were actually produced, what was the percent yield?

Name AgNO3

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Added by Deborah W.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Suman K

06/29/2022

Step 1

Since 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3, we can calculate the number of moles of NH3 produced when 4.50 moles of H2 are reacted. Since H2 is the limiting reagent, 4.50 moles of H2 will produce 4.50/3 = 1.50 moles of NH3. Show more…

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Given the reaction: N2 (g) + H2 (g) → NH3 (g). If 4.50 moles of hydrogen are reacted with excess nitrogen, how many moles of ammonia will be formed? Given the reaction: C4H8 (g) + O2 (g) → CO2 (g) + H2O (g). How many moles of carbon dioxide will be formed if 75.00 grams of C4H8 react with excess oxygen? A CEM 101 student was carrying out the following reaction for a lab experiment. K2CO3 (aq) + CaCl2 (aq) → 2 KCl (aq) + CaCO3 (s) Using the amount of potassium carbonate that they reacted with excess calcium chloride, they calculated 44.25 grams CaCO3 should be formed. They actually collected 38.68 grams of CaCO3. Calculate the student's percent yield and complete the results table below. (Theoretical yield, Actual yield, Percent yield) Given the reaction: Silver nitrate (aq) and potassium chloride (aq) yield silver chloride (s) and potassium nitrate (aq) a. Translate and balance the reaction b. If 84.95 grams of silver nitrate are reacted with excess potassium chloride, what is the theoretical yield of silver chloride? c. If 62.37 grams of silver chloride were actually produced, what was the percent yield? Name AgNO3

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Transcript

00:01 So in the first part, the balanced chemical reaction is n2 gaseous state plus 3h2 gaseous state give rise to 2 nh3 gaseous state.

00:28 Now, to understand, 1 mole of n2 reacts with the 3 moles of hydrogen to produce 2 moles of nh3.

00:38 It is given that 4 .5 moles of h2 react with excess nitrogen.

00:45 Thus, here h2 is a limited reagent.

00:50 1 mole of h2 produces 2 by 3rd mole of nh3.

00:54 So, here we are given that 4 .5 moles of h2, which produce 2 by 3 into 4 .5 moles.

01:13 So there will be 3 moles of nh3 will be formed.

01:31 I hope you understand the first part.

01:36 Now in the second part, the balanced chemical reaction will be c4h8 gaseouset plus 602 gase state will give rise to 4 c4c2.

01:55 Co2 gaseousate plus 4h2o gaseousate.

02:04 Now, thus 1 mole of c4h8 reacts with 6 moles of o2 to produce 4 moles of co2.

02:14 It is given that 75 gram moles of c4h8 react with the excess oxygen.

02:25 Thus here, o2 is a limited reagent.

02:29 One mole of c4h8 contains 56 gram per mole.

02:36 So now, the number of moles in 75 gram of c4h8 is 75 upon 56 moles.

03:05 Which is equal to 1 .34 mole.

03:12 Now, number of moles of co2.

03:27 This will be 4 into 1 .34 mole 5 .36 mole will be there.

03:52 I hope you understand the second part.

03:56 In the third part, we have the reaction which is this is third part.

04:04 We have the reaction k2, k2 co3, aqs, plus cacl2, echus, which give rise to caco3 plus 2 kcl...

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