Question

4. An organic thiol compound is 38.66% C, 9.73% H. and 51.61% S by mass. What is the empirical formula of this compound? [3 pts] 5. When heated, lithium reacts with nitrogen to form lithium nitride. Li(s) + N$_2$(g) ? Li$_3$N(s) (i) Balance the equation and calculate the theoretical yield of Li$_3$N in grams when 12.8 g of Li is heated with 34.9 g of N$_2$. [3 pts] (ii) If the actual yield of Li$_3$N is 15.25 g. what is the percent yield of the reaction? [1 pt] Select the single correct answer for 6-14. (1 pt each) 6. An atom of lead (Pb) is how many times heavier than an atom of iron (Fe)? (1) 5.86 (2) 6.99 (3) 11.30 (4) 3.71 7. What is the average mass of 1 mol of Mg atoms? (1) 6.02 x 10$^{23}$ amu (3) 24.31 g (4) 24.31 amu (2) 6.02 x 10$^{23}$ g 8. How many moles of CO$_2$ are there in 77.5 g of carbon dioxide? (1) 1.76 (2) 0.57 (3) 2.87 (4) 1.29 x 10$^{23}$

          4. An organic thiol compound is 38.66% C, 9.73% H. and 51.61% S by mass. What is the empirical
formula of this compound? [3 pts]
5. When heated, lithium reacts with nitrogen to form lithium nitride.
Li(s) + N$_2$(g) ? Li$_3$N(s)
(i) Balance the equation and calculate the theoretical yield of Li$_3$N in grams when 12.8 g of Li is
heated with 34.9 g of N$_2$. [3 pts]
(ii) If the actual yield of Li$_3$N is 15.25 g. what is the percent yield of the reaction? [1 pt]
Select the single correct answer for 6-14. (1 pt each)
6. An atom of lead (Pb) is how many times heavier than an atom of iron (Fe)? (1) 5.86 (2) 6.99
(3) 11.30
(4) 3.71
7. What is the average mass of 1 mol of Mg atoms? (1) 6.02 x 10$^{23}$ amu
(3) 24.31 g
(4) 24.31 amu
(2) 6.02 x 10$^{23}$ g
8. How many moles of CO$_2$ are there in 77.5 g of carbon dioxide? (1) 1.76 (2) 0.57 (3) 2.87
(4) 1.29 x 10$^{23}$

Show more…

4. An organic thiol compound is 38.66% C, 9.73% H. and 51.61% S by mass. What is the empirical
formula of this compound? [3 pts]
5. When heated, lithium reacts with nitrogen to form lithium nitride.
Li(s) + N2(g) ? Li3N(s)
(i) Balance the equation and calculate the theoretical yield of Li3N in grams when 12.8 g of Li is
heated with 34.9 g of N2. [3 pts]
(ii) If the actual yield of Li3N is 15.25 g. what is the percent yield of the reaction? [1 pt]
Select the single correct answer for 6-14. (1 pt each)
6. An atom of lead (Pb) is how many times heavier than an atom of iron (Fe)? (1) 5.86 (2) 6.99
(3) 11.30
(4) 3.71
7. What is the average mass of 1 mol of Mg atoms? (1) 6.02 x 10^23 amu
(3) 24.31 g
(4) 24.31 amu
(2) 6.02 x 10^23 g
8. How many moles of CO2 are there in 77.5 g of carbon dioxide? (1) 1.76 (2) 0.57 (3) 2.87
(4) 1.29 x 10^23

Added by Jessica G.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Ivan Kochetkov

01/07/2022

Step 1

Step 1: Balance the equation The balanced equation for the reaction is: 6Li + N2 -> 2Li3N Show more…

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5. When heated, lithium reacts with nitrogen to form lithium nitride Li + N2 -> Li3N. Balance the equation and calculate the theoretical yield of LiN in grams when 12.8 g of Li is heated with 34.9 g of N. [3 pts] ii. If the actual yield of LiN is 15.25 g, what is the percent yield of the reaction? [1 pt] Select the single correct answer for 6-14. 1 pt each 6. An atom of lead (Pb) is how many times heavier than an atom of iron (Fe)? 15.86, 26.99, 311.30, 43.71 7. What is the average mass of 1 mol of Mg atoms? 16.02 x 10 amu, 26.02 x 10 g, 324.31 g, 424.31 amu 8. How many moles of CO are there in 77.5 g of carbon dioxide? 11.76, 20.57, 32.87, 412.9 x 10

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Transcript

00:01 Here, lithium reacts with nitrogen according to the reaction shown here.

00:04 6 lithium reacts with 1 nitrogen gaze forming 2 solid li3n.

00:17 And lithium is also solid.

00:19 So, in the first question, yeah, prior we moved on to the questions.

00:25 We better calculate molar masses of each reactants.

00:31 So for lithium molar mass is 6 point.

00:37 Oh, no, so it's already given to us.

00:39 So then it's nice.

00:40 We don't even have to calculate the molar masses.

00:43 Okay, in the first question, in question 8, 124 .0 grams of lithium reacts with 98 .2 grams of nitrogen.

01:01 And we have we need to find limiting reagent let's do this so to determine limiting reagent we have to first calculate number of most of lithium in the mixture it equals to a more mass of lithium divided by its molar mass which is 6 .941 grams per mole and for nitrate number and number of most of nitrogen equals to the mass of nitrogen divided by molar mass of nitrate, which is 98 .2 grams divided by 28 .01 grams per mole.

01:58 Let's calculate each number of moles.

02:12 So a number of most of lithium equals to 17 .86 mole, and number of moles of nitrogen equals to 3 .51 mole.

02:38 So let's calculate ratio of number of most of lithium over number of most of nitrogen in the mixture.

02:47 That is 17 .86 mole over 3 .51 mold.

03:01 It equals to 5 .1 mole...

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