Question 1

Match the following. -NaCl(aq)+ AgNO₃(aq)→ AgCl(s)+ NaNO₃(aq)

Accepted Answer

This equation represents a precipitation reaction, where the solid AgCl is formed from the reaction of Ag+ and Cl- ions in the aqueous solution.

Question 2

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+ O₂(g)→ 2MgO(s) How many moles of O₂ are consumed when 0.770 mol of magnesium burns in excess oxygen?

Accepted Answer

According to the balanced chemical equation, 2 moles of Mg react with 1 mole of O2. Therefore, 0.770 moles of Mg will react with 0.770/2 = 0.385 moles of O2.

Question 3

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+ O₂(g)→ 2MgO(s) When 4.00 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

Accepted Answer

The molar mass of Mg is 24.31 g/mol, and MgO is 40.31 g/mol. For 4.00 g of Mg, moles = 4.00 g / 24.31 g/mol = 0.1645 mol. The reaction produces an equal number of moles of MgO, so mass of MgO = 0.1645 mol * 40.31 g/mol = 6.63 g.

Question 4

List the spectator ions in the following reaction. Ba⁺²(aq)+ 2 OH^-(aq)+ 2 Na ⁺(aq)+ CO₃^-2(aq)→ 2 Na ⁺(aq)+ 2 OH^-(aq)+ BaCO₃₍_s₎

Accepted Answer

The answer of List the spectator ions in the following...

Question 5

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN₃(s)→ 2Na(s)+ 3N₂(g) How many grams of sodium azide are required to produce 33.0 g of nitrogen?

Accepted Answer

To find the grams of sodium azide required, first calculate the moles of nitrogen produced: 33.0 g N₂ / 28.02 g/mol = 1.178 moles N₂. From the balanced equation, 2 moles of NaN₃ produce 3 moles of N₂, so 1.178 moles N₂ require (2/3) * 1.178 = 0.785 moles NaN₃. The molar mass of NaN₃ is 65.01 g/mol, so 0.785 moles * 65.01 g/mol = 51.1 g NaN₃.

Question 6

Determine the oxidation state of Mn in KMnO₄.

Accepted Answer

The answer of Determine the oxidation state of Mn in...

Question 7

Match the following. -HCl(aq)+ (NH₄)₂S(aq)→ H₂S(g)+ 2NH₄Cl(aq)

Accepted Answer

The reaction produces a gas (HS) which evolves out of the solution, indicating that it is a gas evolution reaction.

Question 8

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN₃(s)→ 2Na(s)+ 3N₂(g) How many moles of N₂ are produced by the decomposition of 2.88 mol of sodium azide?

Accepted Answer

According to the balanced equation, 2 moles of sodium azide produce 3 moles of N₂. Therefore, we can use a proportion to find the number of moles produced by 2.88 mol of sodium azide: 2 mol NaN3 / 3 mol N₂ = 2.88 mol NaN3 / x Solving for x gives: x = (3 mol N₂ × 2.88 mol NaN3) / 2 mol NaN3 = 4.32 mol N₂ Therefore, 2.88 mol of sodium azide produces 4.32 mol of N₂, and the answer is (C).

Question 9

Define a net ionic equation.

Accepted Answer

The answer of Define a net ionic equation....

Question 10

Lithium and nitrogen react to produce lithium nitride: 6Li(s)+ N₂(g)→ 2Li₃N(s) How many moles of lithium nitride are produced when 0.450 mol of lithium react in the presence of excess nitrogen?

Accepted Answer

According to the balanced chemical equation, 6 moles of lithium react to produce 2 moles of lithium nitride. Therefore, 0.450 mol of lithium will react to produce 0.150 mol of lithium nitride.

Question 11

How would the concentration change if a 1.0 L flask of 1.0 M NaCl were left uncapped on a laboratory bench for several days.Why?

Accepted Answer

The answer of How would the concentration change if a...

Question 12

How can you tell if a reaction is an oxidation-reduction reaction?

Accepted Answer

The answer of How can you tell if a reaction...

Question 13

Match the following. -H₂SO₄(aq)+ 2 LiOH(aq)→ 2 H₂O(l)+ Li₂SO₄(aq)

Accepted Answer

This reaction is an acid-base reaction where sulfuric acid (H₂SO₄) reacts with lithium hydroxide (LiOH) to form water and lithium sulfate.

Question 14

Lithium and nitrogen react to produce lithium nitride by the following reaction. 6Li(s)+ N₂(g)→ 2Li₃N(s) How many moles of N₂ are needed to react with 0.500 mol of lithium?

Accepted Answer

The answer of Lithium and nitrogen react to produce lithium...

Question 15

What causes a precipitation reaction to occur between two soluble compounds?

Accepted Answer

The answer of What causes a precipitation reaction to occur...

Question 16

Describe the difference between complete ionic and net ionic equations.

Accepted Answer

The answer of Describe the difference between complete ionic and...

Question 17

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s)+ N₂(g)→ 2Li₃N(s) How many moles of lithium are needed to produce 0.60 mol of Li₃N when the reaction is carried out in the presence of excess nitrogen?

Accepted Answer

According to the balanced chemical equation, 6 moles of lithium reacts with 1 mole of nitrogen to produce 2 moles of lithium nitride. Therefore, to produce 0.60 mol of lithium nitride, we need (6/2) x 0.60 = 1.8 mol of lithium. Hence, the answer is B.

Question 18

Explain the difference between a strong and weak electrolyte.Give an example of each.

Accepted Answer

The answer of Explain the difference between a strong and...

Question 19

Match the following. -Mg(s)+ Cu(NO₃)₂(aq)→ Mg(NO₃)₂(aq)+ Cu(s)

Accepted Answer

This is an example of an oxidation-reduction reaction, as magnesium is oxidized and copper is reduced.

Question 20

Define a strong electrolyte.

Accepted Answer

The answer of Define a strong electrolyte....

Quiz 4: Chemical Quantities and Aqueous Reactions

Match the following. -NaCl(aq) + AgNO₃(aq) → AgCl(s) + NaNO₃(aq)

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O₂(g) → 2MgO(s) How many moles of O₂ are consumed when 0.770 mol of magnesium burns in excess oxygen?

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O₂(g) → 2MgO(s) When 4.00 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

List the spectator ions in the following reaction. Ba⁺²(aq)+ 2 OH^-(aq)+ 2 Na ⁺(aq)+ CO₃^-2(aq)→ 2 Na ⁺(aq)+ 2 OH^-(aq)+ BaCO₃₍_s₎

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN₃(s) → 2Na(s) + 3N₂(g) How many grams of sodium azide are required to produce 33.0 g of nitrogen?

Determine the oxidation state of Mn in KMnO₄.

Match the following. -HCl(aq) + (NH₄) ₂S(aq) → H₂S(g) + 2NH₄Cl(aq)

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN₃(s) → 2Na(s) + 3N₂(g) How many moles of N₂ are produced by the decomposition of 2.88 mol of sodium azide?

Define a net ionic equation.

Lithium and nitrogen react to produce lithium nitride: 6Li(s) + N₂(g) → 2Li₃N(s) How many moles of lithium nitride are produced when 0.450 mol of lithium react in the presence of excess nitrogen?

How would the concentration change if a 1.0 L flask of 1.0 M NaCl were left uncapped on a laboratory bench for several days.Why?

How can you tell if a reaction is an oxidation-reduction reaction?

Match the following. -H₂SO₄(aq) + 2 LiOH(aq) → 2 H₂O(l) + Li₂SO₄(aq)

Lithium and nitrogen react to produce lithium nitride by the following reaction. 6Li(s) + N₂(g) → 2Li₃N(s) How many moles of N₂ are needed to react with 0.500 mol of lithium?

What causes a precipitation reaction to occur between two soluble compounds?

Describe the difference between complete ionic and net ionic equations.

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N₂(g) → 2Li₃N(s) How many moles of lithium are needed to produce 0.60 mol of Li₃N when the reaction is carried out in the presence of excess nitrogen?

Explain the difference between a strong and weak electrolyte.Give an example of each.

Match the following. -Mg(s) + Cu(NO₃) ₂(aq) → Mg(NO₃) ₂(aq) + Cu(s)

Define a strong electrolyte.

Quiz 4: Chemical Quantities and Aqueous Reactions

Match the following. -NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq)

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O2(g) → 2MgO(s) How many moles of O2 are consumed when 0.770 mol of magnesium burns in excess oxygen?

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O2(g) → 2MgO(s) When 4.00 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

List the spectator ions in the following reaction. Ba+2(aq)+ 2 OH-(aq)+ 2 Na +(aq)+ CO3-2(aq)→ 2 Na +(aq)+ 2 OH-(aq)+ BaCO3(s)

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3(s) → 2Na(s) + 3N2(g) How many grams of sodium azide are required to produce 33.0 g of nitrogen?

Determine the oxidation state of Mn in KMnO4.

Match the following. -HCl(aq) + (NH4) 2S(aq) → H2S(g) + 2NH4Cl(aq)

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3(s) → 2Na(s) + 3N2(g) How many moles of N2 are produced by the decomposition of 2.88 mol of sodium azide?

Define a net ionic equation.

Lithium and nitrogen react to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) How many moles of lithium nitride are produced when 0.450 mol of lithium react in the presence of excess nitrogen?

How would the concentration change if a 1.0 L flask of 1.0 M NaCl were left uncapped on a laboratory bench for several days.Why?

How can you tell if a reaction is an oxidation-reduction reaction?

Match the following. -H2SO4(aq) + 2 LiOH(aq) → 2 H2O(l) + Li2SO4(aq)

Lithium and nitrogen react to produce lithium nitride by the following reaction. 6Li(s) + N2(g) → 2Li3N(s) How many moles of N2 are needed to react with 0.500 mol of lithium?

What causes a precipitation reaction to occur between two soluble compounds?

Describe the difference between complete ionic and net ionic equations.

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) How many moles of lithium are needed to produce 0.60 mol of Li3N when the reaction is carried out in the presence of excess nitrogen?

Explain the difference between a strong and weak electrolyte.Give an example of each.

Match the following. -Mg(s) + Cu(NO3) 2(aq) → Mg(NO3) 2(aq) + Cu(s)

Define a strong electrolyte.

Match the following. -NaCl(aq) + AgNO₃(aq) → AgCl(s) + NaNO₃(aq)

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O₂(g) → 2MgO(s) How many moles of O₂ are consumed when 0.770 mol of magnesium burns in excess oxygen?

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O₂(g) → 2MgO(s) When 4.00 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

List the spectator ions in the following reaction. Ba⁺²(aq)+ 2 OH^-(aq)+ 2 Na ⁺(aq)+ CO₃^-2(aq)→ 2 Na ⁺(aq)+ 2 OH^-(aq)+ BaCO₃₍_s₎

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN₃(s) → 2Na(s) + 3N₂(g) How many grams of sodium azide are required to produce 33.0 g of nitrogen?

Determine the oxidation state of Mn in KMnO₄.

Match the following. -HCl(aq) + (NH₄) ₂S(aq) → H₂S(g) + 2NH₄Cl(aq)

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN₃(s) → 2Na(s) + 3N₂(g) How many moles of N₂ are produced by the decomposition of 2.88 mol of sodium azide?

Lithium and nitrogen react to produce lithium nitride: 6Li(s) + N₂(g) → 2Li₃N(s) How many moles of lithium nitride are produced when 0.450 mol of lithium react in the presence of excess nitrogen?

Match the following. -H₂SO₄(aq) + 2 LiOH(aq) → 2 H₂O(l) + Li₂SO₄(aq)

Lithium and nitrogen react to produce lithium nitride by the following reaction. 6Li(s) + N₂(g) → 2Li₃N(s) How many moles of N₂ are needed to react with 0.500 mol of lithium?

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N₂(g) → 2Li₃N(s) How many moles of lithium are needed to produce 0.60 mol of Li₃N when the reaction is carried out in the presence of excess nitrogen?

Match the following. -Mg(s) + Cu(NO₃) ₂(aq) → Mg(NO₃) ₂(aq) + Cu(s)