Question

12.If each symbol represents 1 mole of Mg (s) and 1 mole of N2 (g), and...

12.If each symbol represents 1 mole of Mg (s) and 1 mole of N2 (g), and the the reactants are mixed in the proportions shown, what is the limiting reactant and how many moles of excess reactant remain after the reaction is complete? a) N2 (g), 2 mole Mg (s) b) N2 (g), 3 mole Mg (s) c) Mg (s), 1 mole N2 (g) d) Mg (s), 2 mole N2 (g) e) Mg (s), 0.5 mole N2 (g)

Homework Answers

Answer #1

the reation must be

3Mg + N2 = Mg3N2

then, ratio is 3:1

ratio = Mg/N2 = 3/1 = 3

a)

1 mol of N2, 2 mol of Mg

ratio

Mg/N = 2/1 = 0.5

since 0.5 < 3, then Mg is limiting

1-2/3 = 0.333 mol of Mg left

b)

3/1 = 3

no limiting reactant since ratio = 3, similar as 3

0 mol left,

c)

1:1

clearly, there is not enough Mg to react

1-1/3 = 0.6667 mol of Mg left

d)

1 mol of }MG = 2 mol of N2

Mg is limiting, since 1/2 = 0.5

2-1/3 = 1.666 mol of N2 excess

e)

1 mol of MG = 0.5 mol of N2

1/0.5 = 2

since 2 < 3, there is not enough MG

excess = 0.5 - 1/3 = 0.1667 mol of MG

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The reaction of magnesium with nitrogen produces magnesium nitride, as follows. 3 Mg(s) + N2(g) →...
The reaction of magnesium with nitrogen produces magnesium nitride, as follows. 3 Mg(s) + N2(g) → Mg3N2(s) If the reaction is started with 2.05 mol Mg and 0.891 mol N2, find the following. (a) the limiting reactant (b) the excess reactant (c) the number of moles of magnesium nitride produced
The reaction of magnesium with nitrogen produces magnesium nitride, as follows. 3 Mg(s) + N2(g) →...
The reaction of magnesium with nitrogen produces magnesium nitride, as follows. 3 Mg(s) + N2(g) → Mg3N2(s) If the reaction is started with 2.70 mol Mg and 0.805 mol N2, find the following. What is the the limiting reactant and the number of moles of magnesium nitride produced?
The reaction 6ClO2 (g) + 2BrF3 (l) --> 6ClO2F (s) + Br2 (l) is carried out...
The reaction 6ClO2 (g) + 2BrF3 (l) --> 6ClO2F (s) + Br2 (l) is carried out with 12 mol of ClO2 and 5 mol of BrF3. a) Identify the excess reactant. b) Estimate how many moles of each product will be produced and how many moles of the excess reactant will remain. c) Which reactant is limiting?
Given the following chemical reaction 4Al(s) + 3O2(g)=2Al2O3(s). If 10.0grams of Al and 19.0gram of O2...
Given the following chemical reaction 4Al(s) + 3O2(g)=2Al2O3(s). If 10.0grams of Al and 19.0gram of O2 are mixed together how many moles of each reactants you have. b) how many moles of the product you will form c) which of these two reactant is the limiting reactant d) what is the theoritical yield of this reaction (in gram) e) If 15.0grams of Al2O3 was obtained, what is the percent yield of this reaction.
Consider the balanced chemical reaction shown below. 4 PH3(g) + 8 O2(g) 6 H2O(l) + 1...
Consider the balanced chemical reaction shown below. 4 PH3(g) + 8 O2(g) 6 H2O(l) + 1 P4O10(s) In a certain experiment, 3.118 g of PH3(g) reacts with 6.294 g of O2(g). (a) Which is the limiting reactant? (Example: type PH3 for PH3(g)) is the limiting reactant. (b) How many grams of H2O(l) form? g of H2O(l) form. (c) How many grams of P4O10(s) form? g of P4O10(s) form. (d) How many grams of the excess reactant remains after the limiting...
Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia....
Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia. N2 (g) +3 H2 (g) -------------------> 2 NH3 (g) Assume 0.240 mol of N2 and 0.772 mol of H2 are present initially. 1) After complete reaction, how many moles of ammonia are produced? 2) How many moles of H2 remain? 3) How many moles of N2 remain? 4) What is the limiting reactant?
2 Zn (s) + O2 (g) → 2 ZnO (s) If 25 g of O2 reacts...
2 Zn (s) + O2 (g) → 2 ZnO (s) If 25 g of O2 reacts with excess Zn in the reaction above, how many grams of ZnO will be formed? Question 2 options: 1.6 g ZnO 32 g ZnO 64 g ZnO 127 g ZnO H3PO4 + 3 NaOH → Na3PO4 + 3 H2O If 3.3 moles of H3PO4 react with 6.2 moles of NaOH, how many moles of H2O are formed? What is the limiting reactant? Question 3...
Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce...
Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia. N2(g)+3H2(g)⟶2NH3(g) Assume 0.230 mol N2 and 0.758 mol H2 are present initially.PLEASE SHOW steps!! 1)After complete reaction, how many moles of ammonia NH3 are produced? 2)How many moles of H2 remain? 3)How many moles of N2 remain? 4)What is the limiting reactant? nitrogen or hydrogen
3.156x103 g of C3H6 is mixed with 3.601 x 103 g of NO and produces 2.501...
3.156x103 g of C3H6 is mixed with 3.601 x 103 g of NO and produces 2.501 x 103 g of C3H3N according to the following equation. 4C3H6(g) + 6NO(g) --> 4C3H3N(g) + 6H2O(g) + N2(g) Determine the limiting reactant. Use molar ratios to justify your answer. Determine the theoretical yield of C3H3N in grams Determine the % yield of C3H3N. Determine the number of moles of excess reactant that remain once the reaction goes to completion. ASAP
Consider the balanced chemical reaction shown below. 2 C3H6(g) + 9 O2(g) 6 CO2(g) + 6...
Consider the balanced chemical reaction shown below. 2 C3H6(g) + 9 O2(g) 6 CO2(g) + 6 H2O(l) In a certain experiment, 6.004 g of C3H6(g) reacts with 2.118 g of O2(g). (a) Which is the limiting reactant? _____ is the limiting reactant. (b) How many grams of CO2(g) form? _____g of CO2(g) form. (c) How many grams of H2O(l) form? _____g of H2O(l) form. (d) How many grams of the excess reactant remains after the limiting reactant is completely consumed?_____...