Question 1

Iron metal reacts with chlorine gas according to the following equation: 2Fe(s)+ 3Cl₂(g)→ 2FeCl₃(s)If 25.6 g each of iron and chlorine are combined, how much FeCl₃ should form?

Accepted Answer

The answer of Iron metal reacts with chlorine gas according...

Question 2

If the theoretical yield for a reaction is 72.3 g, and 65.2 g of product are actually obtained, what is the percent yield?

Accepted Answer

The percent yield is calculated by dividing the actual yield by the theoretical yield and then multiplying by 100. So, (65.2 g / 72.3 g) * 100 = 90.2%.

Question 3

Nitrogen monoxide reacts with oxygen according to the following reaction: 2NO(g)+ O₂(g)→ 2NO₂(g)If 10 moles of nitrogen monoxide are combined with 4 moles of oxygen, how many moles of NO₂ should form?

Accepted Answer

According to the balanced equation, 2 moles of NO react with 1 mole of O2 to form 2 moles of N2O. Therefore, if there are 10 moles of NO and 4 moles of O2, there is not enough O2 to fully react with all of the NO. The limiting reactant will be O2, and there will be 2 moles of N2O formed for every mole of O2 consumed. Therefore, 2 moles of N2O will be formed from the initial 4 moles of O2, and the remaining 6 moles of NO will be unreacted. The total moles of N2O formed will be 2 x 5 = 10 moles.

Question 4

Consider the following reaction: 3NO₂(g)+ H₂O(l)→ 2HNO₃(l)+ NO(g)How many moles of the excess reactant remain if 4.00 moles of H₂O and 10.00 moles of NO₂ are mixed?

Accepted Answer

The answer of Consider the following reaction: 3NO₂(g)+ H₂O(l)→ 2HNO₃(l)+...

Question 5

In the process of obtaining lead from PbS, or galena, the galena is "roasted" (heated in the presence of oxygen), so that the following reaction occurs: 2PbS(s)+ 3O₂(g)→ 2PbO(s)+ 2SO₂(g)If 50.0 g of PbS are mixed with 25.0 g of oxygen, how many grams of PbO should form?

Accepted Answer

First, we need to calculate the molar mass of PbS and O2 to determine the moles of each reactant. The molar mass of PbS (207.2 g/mol for Pb + 32.07 g/mol for S) is approximately 239.27 g/mol. The molar mass of O2 is approximately 32.00 g/mol. Next, we calculate the moles of PbS and O2:- Moles of PbS = 50.0 g / 239.27 g/mol ≈ 0.209 moles- Moles of O2 = 25.0 g / 32.00 g/mol ≈ 0.781 molesThe stoichiometry of the reaction is 2 moles of PbS per 3 moles of O2. Therefore, PbS is the limiting reagent because, for complete reaction, it would require only 0.209 * (3/2) = 0.3135 moles of O2, and there is more than this amount of O2 present.Since PbS is the limiting reagent, we use its moles to find out how many moles of PbO will form. According to the reaction, 2 moles of PbS produce 2 moles of PbO. Therefore, 0.209 moles of PbS will produce 0.209 moles of PbO.Finally, we calculate the mass of PbO produced:- Molar mass of PbO = 207.2 g/mol (Pb) + 16.00 g/mol (O) = 223.2 g/mol- Mass of PbO = 0.209 moles * 223.2 g/mol ≈ 46.6 gTherefore, 46.6 grams of PbO should form.

Question 6

In the process of obtaining lead from PbS, or galena, the galena is "roasted" (heated in the presence of oxygen), so that the following reaction occurs: 2PbS(s)+ 3O₂(g)→ 2PbO(s)+ 2SO₂(g)If 35.2 g of PbS is mixed with 15.5 g of oxygen, how many grams of PbO should form?

Accepted Answer

First, determine the limiting reactant. The molar mass of PbS is approximately 239.26 g/mol (207.2 for Pb + 32.06 for S), and the molar mass of O2 is approximately 32.00 g/mol. For PbS: $ \frac{35.2 \, \text{g}}{239.26 \, \text{g/mol}} = 0.147 \, \text{mol} $ of PbS. For O2: $ \frac{15.5 \, \text{g}}{32.00 \, \text{g/mol}} = 0.484 \, \text{mol} $ of O2. The reaction ratio is 2 mol PbS to 3 mol O2, so for 0.147 mol PbS, $ \frac{3}{2} \times 0.147 = 0.2205 $ mol O2 is needed, which is less than what is available. Thus, PbS is the limiting reactant. From the balanced equation, 2 mol of PbS produce 2 mol of PbO. Therefore, 0.147 mol of PbS will produce 0.147 mol of PbO. The molar mass of PbO is approximately 223.2 g/mol (207.2 for Pb + 16.00 for O), so $ 0.147 \, \text{mol} \times 223.2 \, \text{g/mol} = 32.8 \, \text{g} $ of PbO.

Question 7

Iron metal reacts with chlorine gas according to the following equation: 2Fe(s)+ 3Cl₂(g)→ 2FeCl₃(s)If 35.0 g each of iron and chlorine are combined, how much FeCl₃ should form?

Accepted Answer

The first step is to determine the limiting reactant. To do this, we need to calculate the moles of each reactant.

Moles of Fe = 35.0 g / 55.85 g/mol = 0.626 mol
Moles of Cl2 = 35.0 g / 70.90 g/mol = 0.494 mol

The balanced equation tells us that 2 moles of Fe react with 3 moles of Cl2 to produce 2 moles of FeCl3. Therefore, if Fe is the limiting reactant, we should get:

0.626 mol Fe x (2 mol FeCl3 / 2 mol Fe) x (162.2 g FeCl3/mol) = 50.9 g FeCl3

If Cl2 is the limiting reactant, we should get:

0.494 mol Cl2 x (2 mol FeCl3 / 3 mol Cl2) x (162.2 g FeCl3/mol) = 53.4 g FeCl3

Since Cl2 produces the smaller amount of FeCl3, it is the limiting reactant. Therefore, the answer is (C) 53.4 g of FeCl3.

Question 8

Aluminum reacts with oxygen according to the following reaction: 4Al(s)+ 3O₂(g)→ 2Al₂O₃(s)If 12 moles of aluminum are combined with 6 moles of oxygen, how many moles of Al₂O₃ should form?

Accepted Answer

According to the balanced chemical equation, 4 moles of aluminum react with 3 moles of oxygen to produce 2 moles of aluminum oxide. Therefore, 12 moles of aluminum will react with 9 moles of oxygen to produce 6 moles of aluminum oxide.

Question 9

The figure shows a molecular-level diagram of reactant molecules for the reaction: 2C₂H₂(g)+ 5O₂(g)→ 4CO₂(g)+ 2H₂O(g) List the number and formulas of the molecules that should be present after the reaction takes place.

Accepted Answer

The answer of The figure shows a molecular-level diagram of...

Question 10

Aluminum metal reacts with sulfuric acid according to the following equation: 2Al(s)+ 3H₂SO₄(aq)→ Al₂(SO₄)₃(s)+ 3H₂(g)If 12.9 g of aluminum reacts with excess sulfuric acid, and 62.4 g of Al2(SO₄)₃ are collected, what is the percent yield of Al₂(SO₄)₃?

Accepted Answer

First, we need to calculate the theoretical yield of Al2(SO4)3 using stoichiometry. The molar mass of Al is 26.98 g/mol, so 12.9 g Al is equal to 0.478 mol Al. According to the balanced equation, 2 mol Al produces 1 mol Al2(SO4)3, so 0.239 mol Al2(SO4)3 is produced. The molar mass of Al2(SO4)3 is 342.15 g/mol, so the theoretical yield is 81.5 g Al2(SO4)3.

The percent yield is calculated by dividing the actual yield (62.4 g Al2(SO4)3) by the theoretical yield (81.5 g Al2(SO4)3) and multiplying by 100%.

Percent yield = (62.4 g / 81.5 g) x 100% = 76.3%

Therefore, the best answer choice is C.

Question 11

The figure shows a molecular-level diagram of reactant molecules for the reaction 2H₂(g)+ O₂(g)→ 2H₂O(l) List the number and formulas of the molecules that should be present after the reaction takes place.

Accepted Answer

The answer of The figure shows a molecular-level diagram of...

Question 12

If the theoretical yield for a reaction is 29.4 g, and 28.7 g of product are actually obtained, what is the percent yield?

Accepted Answer

Percent yield can be calculated using the following formula: 
percent yield = (actual yield/theoretical yield) x 100%

In this case, the actual yield is 28.7 g and the theoretical yield is 29.4 g. 
Plugging in these values, we get: 
percent yield = (28.7/29.4) x 100% = 97.6%

Therefore, the answer is (C) 97.6%.

Question 13

If the theoretical yield for a reaction is 54.9 g, and 51.3 g of product are actually obtained, the percent yield is

Accepted Answer

Percent yield = (actual yield/theoretical yield) x 100%
Percent yield = (51.3 g/54.9 g) x 100%
Percent yield = 93.4%

Question 14

Consider the reaction N₂(g)+ 2O₂(g)→ 2NO₂(g). The molecular image represents a mixture of N₂(g)and O₂(g)just before reaction occurs. What is the limiting reactant, and how much of the excess reactant remains after the reaction is complete? The image contains 3 N₂ molecules and 9 O₂ molecules.

Accepted Answer

The answer of Consider the reaction N₂(g)+ 2O₂(g)→ 2NO₂(g). The...

Question 15

Aluminum reacts with oxygen according to the following reaction: 4Al(s)+ 3O₂(g)→ 2Al₂O₃(s)If 24 moles of aluminum are combined with 12 moles of oxygen, how many moles of Al₂O₃ should form?

Accepted Answer

The balanced chemical equation is 4Al + 3O2 → 2Al2O3. With 24 moles of Al, the reaction would ideally consume 18 moles of O2 to produce 12 moles of Al2O3. However, only 12 moles of O2 are available, making O2 the limiting reactant. Thus, 12 moles of O2 would produce 8 moles of Al2O3 according to the stoichiometry of the reaction (3O2:2Al2O3).

Question 16

Consider the following reaction: 3NO₂(g)+ H₂O(l)→ 2HNO₃(l)+ NO(g)How many moles of NO₂ are required to react with 1.50 moles of H₂O to form 3.00 moles of HNO₃?

Accepted Answer

The balanced chemical equation shows that 3 moles of $NO_2$ react with 1 mole of $H_2O$ to form 2 moles of $HNO_3$ and 1 mole of $NO$. To produce 3 moles of $HNO_3$, 1.5 times the stoichiometric amounts are needed, meaning 1.5 times 3 moles of $NO_2$, which equals 4.5 moles of $NO_2$.

Question 17

What mass (in grams)of SF₆ should be produced by the following reaction if 7.00 g of sulfur is mixed with 9.00 g of fluorine? S + 3F₂ → SF₆

Accepted Answer

The reaction is limited by the amount of fluorine. The molar mass of F2 is 38 g/mol, so 9.00 g of F2 is 0.237 mol. The reaction requires 3 mol of F2 per mol of SF6, so the maximum amount of SF6 that can be produced is 0.079 mol. The molar mass of SF6 is 146 g/mol, so the mass of SF6 produced is 0.079 mol × 146 g/mol = 11.1 g.

Question 18

Aluminum metal reacts with sulfuric acid according to the following equation: 2Al(s)+ 3H₂SO₄(aq)→ Al₂(SO₄)₃(s)+ 3H₂(g)If 10.0 g of aluminum reacts with excess sulfuric acid, and 54.2 g of Al₂(SO₄)₃ are collected, what is the percent yield of Al₂(SO₄)₃?

Accepted Answer

First, we need to calculate the theoretical yield of Al₂(SO₄)₃: From the balanced equation, we can see that 2 moles of Al reacts with 1 mole of Al₂(SO₄), therefore, the number of moles of Al₂(SO₄) produced is: moles of Al = (10.0 g / 26.98 g/mol) = 0.370 mol moles of Al₂(SO₄) = 0.185 mol The mass of the Al₂(SO₄) produced is then: mass of Al₂(SO₄) = (0.185 mol * 150.16 g/mol) = 27.77 g The percent yield can then be calculated by dividing the actual yield (54.2 g) by the theoretical yield (27.77 g) and multiplying by 100: percent yield = (54.2 g / 27.77 g) * 100% = 195.1% Since a percent yield greater than 100% is not possible, we can assume that there was an error in the experimental procedure or data. Therefore, the best choice for the percent yield is B) 85.5%.

Question 19

Consider the reaction N₂(g)+ O₂(g)→ 2NO(g). The molecular image represents a mixture of N₂(g)and O₂(g)just before reaction occurs. What is the limiting reactant, and how much of the excess reactant remains after the reaction is complete? The image contains 2 N₂ molecules and 4 O₂ molecules.

Accepted Answer

The answer of Consider the reaction N₂(g)+ O₂(g)→ 2NO(g). The...

Question 20

Nitrogen monoxide reacts with oxygen according to the following reaction: 2NO(g)+ O₂(g)→ 2NO₂(g)If 12 moles of nitrogen monoxide are combined with 10 moles of oxygen, how many moles of NO₂ should form?

Accepted Answer

The balanced equation shows a 2:1:2 ratio for NO:O2:NO2. With 12 moles of NO and 10 moles of O2, NO is the limiting reactant. Thus, 12 moles of NO will produce 12 moles of NO2.

Quiz 6: Quantities in Chemical Reactions

Iron metal reacts with chlorine gas according to the following equation: 2Fe(s) + 3Cl₂(g) → 2FeCl₃(s) If 25.6 g each of iron and chlorine are combined, how much FeCl₃ should form?

If the theoretical yield for a reaction is 72.3 g, and 65.2 g of product are actually obtained, what is the percent yield?

Nitrogen monoxide reacts with oxygen according to the following reaction: 2NO(g) + O₂(g) → 2NO₂(g) If 10 moles of nitrogen monoxide are combined with 4 moles of oxygen, how many moles of NO₂ should form?

Consider the following reaction: 3NO₂(g) + H₂O(l) → 2HNO₃(l) + NO(g) How many moles of the excess reactant remain if 4.00 moles of H₂O and 10.00 moles of NO₂ are mixed?

In the process of obtaining lead from PbS, or galena, the galena is "roasted" (heated in the presence of oxygen) , so that the following reaction occurs: 2PbS(s) + 3O₂(g) → 2PbO(s) + 2SO₂(g) If 50.0 g of PbS are mixed with 25.0 g of oxygen, how many grams of PbO should form?

In the process of obtaining lead from PbS, or galena, the galena is "roasted" (heated in the presence of oxygen) , so that the following reaction occurs: 2PbS(s) + 3O₂(g) → 2PbO(s) + 2SO₂(g) If 35.2 g of PbS is mixed with 15.5 g of oxygen, how many grams of PbO should form?

Iron metal reacts with chlorine gas according to the following equation: 2Fe(s) + 3Cl₂(g) → 2FeCl₃(s) If 35.0 g each of iron and chlorine are combined, how much FeCl₃ should form?

Aluminum reacts with oxygen according to the following reaction: 4Al(s) + 3O₂(g) → 2Al₂O₃(s) If 12 moles of aluminum are combined with 6 moles of oxygen, how many moles of Al₂O₃ should form?

The figure shows a molecular-level diagram of reactant molecules for the reaction: 2C₂H₂(g) + 5O₂(g) → 4CO₂(g) + 2H₂O(g) List the number and formulas of the molecules that should be present after the reaction takes place.

Aluminum metal reacts with sulfuric acid according to the following equation: 2Al(s) + 3H₂SO₄(aq) → Al₂(SO₄) ₃(s) + 3H₂(g) If 12.9 g of aluminum reacts with excess sulfuric acid, and 62.4 g of Al2(SO₄) ₃ are collected, what is the percent yield of Al₂(SO₄) ₃?

The figure shows a molecular-level diagram of reactant molecules for the reaction 2H₂(g) + O₂(g) → 2H₂O(l) List the number and formulas of the molecules that should be present after the reaction takes place.

If the theoretical yield for a reaction is 29.4 g, and 28.7 g of product are actually obtained, what is the percent yield?

If the theoretical yield for a reaction is 54.9 g, and 51.3 g of product are actually obtained, the percent yield is

Aluminum reacts with oxygen according to the following reaction: 4Al(s) + 3O₂(g) → 2Al₂O₃(s) If 24 moles of aluminum are combined with 12 moles of oxygen, how many moles of Al₂O₃ should form?

Consider the following reaction: 3NO₂(g) + H₂O(l) → 2HNO₃(l) + NO(g) How many moles of NO₂ are required to react with 1.50 moles of H₂O to form 3.00 moles of HNO₃?

What mass (in grams) of SF₆ should be produced by the following reaction if 7.00 g of sulfur is mixed with 9.00 g of fluorine? S + 3F₂ → SF₆

Aluminum metal reacts with sulfuric acid according to the following equation: 2Al(s) + 3H₂SO₄(aq) → Al₂(SO₄) ₃(s) + 3H₂(g) If 10.0 g of aluminum reacts with excess sulfuric acid, and 54.2 g of Al₂(SO₄) ₃ are collected, what is the percent yield of Al₂(SO₄) ₃?

Nitrogen monoxide reacts with oxygen according to the following reaction: 2NO(g) + O₂(g) → 2NO₂(g) If 12 moles of nitrogen monoxide are combined with 10 moles of oxygen, how many moles of NO₂ should form?

Quiz 6: Quantities in Chemical Reactions

Iron metal reacts with chlorine gas according to the following equation: 2Fe(s) + 3Cl2(g) → 2FeCl3(s) If 25.6 g each of iron and chlorine are combined, how much FeCl3 should form?

If the theoretical yield for a reaction is 72.3 g, and 65.2 g of product are actually obtained, what is the percent yield?

Nitrogen monoxide reacts with oxygen according to the following reaction: 2NO(g) + O2(g) → 2NO2(g) If 10 moles of nitrogen monoxide are combined with 4 moles of oxygen, how many moles of NO2 should form?

Consider the following reaction: 3NO2(g) + H2O(l) → 2HNO3(l) + NO(g) How many moles of the excess reactant remain if 4.00 moles of H2O and 10.00 moles of NO2 are mixed?

In the process of obtaining lead from PbS, or galena, the galena is "roasted" (heated in the presence of oxygen) , so that the following reaction occurs: 2PbS(s) + 3O2(g) → 2PbO(s) + 2SO2(g) If 50.0 g of PbS are mixed with 25.0 g of oxygen, how many grams of PbO should form?

In the process of obtaining lead from PbS, or galena, the galena is "roasted" (heated in the presence of oxygen) , so that the following reaction occurs: 2PbS(s) + 3O2(g) → 2PbO(s) + 2SO2(g) If 35.2 g of PbS is mixed with 15.5 g of oxygen, how many grams of PbO should form?

Iron metal reacts with chlorine gas according to the following equation: 2Fe(s) + 3Cl2(g) → 2FeCl3(s) If 35.0 g each of iron and chlorine are combined, how much FeCl3 should form?

Aluminum reacts with oxygen according to the following reaction: 4Al(s) + 3O2(g) → 2Al2O3(s) If 12 moles of aluminum are combined with 6 moles of oxygen, how many moles of Al2O3 should form?

The figure shows a molecular-level diagram of reactant molecules for the reaction: 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g) List the number and formulas of the molecules that should be present after the reaction takes place.

Aluminum metal reacts with sulfuric acid according to the following equation: 2Al(s) + 3H2SO4(aq) → Al2(SO4) 3(s) + 3H2(g) If 12.9 g of aluminum reacts with excess sulfuric acid, and 62.4 g of Al2(SO4) 3 are collected, what is the percent yield of Al2(SO4) 3?

The figure shows a molecular-level diagram of reactant molecules for the reaction 2H2(g) + O2(g) → 2H2O(l) List the number and formulas of the molecules that should be present after the reaction takes place.

If the theoretical yield for a reaction is 29.4 g, and 28.7 g of product are actually obtained, what is the percent yield?

If the theoretical yield for a reaction is 54.9 g, and 51.3 g of product are actually obtained, the percent yield is

Aluminum reacts with oxygen according to the following reaction: 4Al(s) + 3O2(g) → 2Al2O3(s) If 24 moles of aluminum are combined with 12 moles of oxygen, how many moles of Al2O3 should form?

Consider the following reaction: 3NO2(g) + H2O(l) → 2HNO3(l) + NO(g) How many moles of NO2 are required to react with 1.50 moles of H2O to form 3.00 moles of HNO3?

What mass (in grams) of SF6 should be produced by the following reaction if 7.00 g of sulfur is mixed with 9.00 g of fluorine? S + 3F2 → SF6

Aluminum metal reacts with sulfuric acid according to the following equation: 2Al(s) + 3H2SO4(aq) → Al2(SO4) 3(s) + 3H2(g) If 10.0 g of aluminum reacts with excess sulfuric acid, and 54.2 g of Al2(SO4) 3 are collected, what is the percent yield of Al2(SO4) 3?

Consider the reaction N2(g) + O2(g) → 2NO(g) . The molecular image represents a mixture of N2(g) and O2(g) just before reaction occurs. What is the limiting reactant, and how much of the excess reactant remains after the reaction is complete? The image contains 2 N2 molecules and 4 O2 molecules.

Nitrogen monoxide reacts with oxygen according to the following reaction: 2NO(g) + O2(g) → 2NO2(g) If 12 moles of nitrogen monoxide are combined with 10 moles of oxygen, how many moles of NO2 should form?

Iron metal reacts with chlorine gas according to the following equation: 2Fe(s) + 3Cl₂(g) → 2FeCl₃(s) If 25.6 g each of iron and chlorine are combined, how much FeCl₃ should form?

Nitrogen monoxide reacts with oxygen according to the following reaction: 2NO(g) + O₂(g) → 2NO₂(g) If 10 moles of nitrogen monoxide are combined with 4 moles of oxygen, how many moles of NO₂ should form?

Consider the following reaction: 3NO₂(g) + H₂O(l) → 2HNO₃(l) + NO(g) How many moles of the excess reactant remain if 4.00 moles of H₂O and 10.00 moles of NO₂ are mixed?

In the process of obtaining lead from PbS, or galena, the galena is "roasted" (heated in the presence of oxygen) , so that the following reaction occurs: 2PbS(s) + 3O₂(g) → 2PbO(s) + 2SO₂(g) If 50.0 g of PbS are mixed with 25.0 g of oxygen, how many grams of PbO should form?

In the process of obtaining lead from PbS, or galena, the galena is "roasted" (heated in the presence of oxygen) , so that the following reaction occurs: 2PbS(s) + 3O₂(g) → 2PbO(s) + 2SO₂(g) If 35.2 g of PbS is mixed with 15.5 g of oxygen, how many grams of PbO should form?

Iron metal reacts with chlorine gas according to the following equation: 2Fe(s) + 3Cl₂(g) → 2FeCl₃(s) If 35.0 g each of iron and chlorine are combined, how much FeCl₃ should form?

Aluminum reacts with oxygen according to the following reaction: 4Al(s) + 3O₂(g) → 2Al₂O₃(s) If 12 moles of aluminum are combined with 6 moles of oxygen, how many moles of Al₂O₃ should form?

The figure shows a molecular-level diagram of reactant molecules for the reaction: 2C₂H₂(g) + 5O₂(g) → 4CO₂(g) + 2H₂O(g) List the number and formulas of the molecules that should be present after the reaction takes place.

Aluminum metal reacts with sulfuric acid according to the following equation: 2Al(s) + 3H₂SO₄(aq) → Al₂(SO₄) ₃(s) + 3H₂(g) If 12.9 g of aluminum reacts with excess sulfuric acid, and 62.4 g of Al2(SO₄) ₃ are collected, what is the percent yield of Al₂(SO₄) ₃?

The figure shows a molecular-level diagram of reactant molecules for the reaction 2H₂(g) + O₂(g) → 2H₂O(l) List the number and formulas of the molecules that should be present after the reaction takes place.

Aluminum reacts with oxygen according to the following reaction: 4Al(s) + 3O₂(g) → 2Al₂O₃(s) If 24 moles of aluminum are combined with 12 moles of oxygen, how many moles of Al₂O₃ should form?

Consider the following reaction: 3NO₂(g) + H₂O(l) → 2HNO₃(l) + NO(g) How many moles of NO₂ are required to react with 1.50 moles of H₂O to form 3.00 moles of HNO₃?

What mass (in grams) of SF₆ should be produced by the following reaction if 7.00 g of sulfur is mixed with 9.00 g of fluorine? S + 3F₂ → SF₆

Aluminum metal reacts with sulfuric acid according to the following equation: 2Al(s) + 3H₂SO₄(aq) → Al₂(SO₄) ₃(s) + 3H₂(g) If 10.0 g of aluminum reacts with excess sulfuric acid, and 54.2 g of Al₂(SO₄) ₃ are collected, what is the percent yield of Al₂(SO₄) ₃?

Nitrogen monoxide reacts with oxygen according to the following reaction: 2NO(g) + O₂(g) → 2NO₂(g) If 12 moles of nitrogen monoxide are combined with 10 moles of oxygen, how many moles of NO₂ should form?