Chm test 3

how many molecules of sulfur trioxide are in 78.0g?

5.9 X 10^23

For a chemical reaction to occur, at least one new substance must be formed as a product. Which of the following are chemical reactions? 1. 2 Na(s) + Cl2(g) Right Arrow 2 NaCl(s) 2. CO2(s) Right Arrow CO2(g) 3. BaCO3(s) Right Arrow BaO(s) + CO2(g) 4. NaI(aq) + AgNO3(aq) Right Arrow Ag NO3(aq) + NaI(aq) 5. C3 H6 O(l) + CO2(s) Right Arrow CO2(g) + C3 H6 O(l) A) 1 and 3 B) 1, 2, and 3 C) 1, 3, and 5 D) 4 and 5 E) 2, 4, and 5

A) 1 and 3

What is the mass, in grams, of one molecule of OF2? A) 8.97 ×10−23 grams B) 54.0 grams C) 3.25×10²⁵ grams D) 1.12×10²⁴ grams E) 3.08 ×10⁻²⁶ grams

A) 8.97 ×10⁻²³ grams

For the following reaction, identify the covalent bonds being broken and the bonds being formed. Mg(s) + 2 HCl(g) Right Arrow MgCl2(s) + H2(g) A) H—Cl bonds are broken and H— H bonds are formed. B) Mg— Mg bonds are broken and Mg—Cl bonds are formed. C) Mg—Mg bonds are broken and H—H bonds are formed. D) H—H bonds are broken and H—Cl bonds are formed. E) H—Cl bonds are broken and Mg—Mg bonds are formed.

A) H—Cl bonds are broken and H— H bonds are formed.

H₂SO₄(aq) + KOH(aq) → H₂O(l) + K₂SO₄(aq)

Acid-base H₂SO₄(aq) + 2KOH(aq) → 2H₂O(l) + K₂SO₄(aq)

How many moles of iron are there in 84.9 grams of Fe? A) 9.16x1023 moles. B) 6.57x10−1 moles C) 1.52 moles D) 5.11x1025 moles E) 4.74x103 moles

C) 1.52 moles

The reason we balance chemical equations is A) actually, chemical reactions do not have to be balanced. B) to obey the law of conservation of energy. C) to obey the law of balancing electrons. D) to obey the law of conservation of matter.

D) to obey the law of conservation of matter.

Select the compound that is soluble in water. A) PbCl2 B) Mg(OH) 2 C) Ag3PO4 D) BaSO4 E) FeI2

E) FeI2

What is a salt?

Metal ion from a base and an anion of the acid.

Which one is insoluble in water NH₄Cl NaCl PbCl₂ CaCl₂ FeCl₃

PbCl₂

Strontium periodate has the formula Sr(IO4)2. Calculate the mass percent of oxygen in this compound. A) 3.67% oxygen B) 3.40% oxygen C) 5.73% oxygen D) 23.0% oxygen E) 27.2% oxygen

Sr(IO₄)₂=88+2(127)+8(16)=470; 8(16)/470= E) 27.2% oxygen

HNO₃ + Al(OH)₃ →

acid- base reaction 3HNO₃ + Al(OH)₃ → Al(NO₃)₃ + 3H₂O

CH₃COOH + KOH →

acid- base reaction CH₃CO₂H + KOH → KCH₃CO₂ + H₂O

Li(s) + N₂(g) → Li₃N(s)

combination reaction 6Li(s) + N₂(g) → 2Li₃N(s)

K₂SO₃ + S₈ → K₂S₂O₃

combination reaction 8K₂SO₃ + S₈ → 8K₂S₂O₃

CO + H₂ → CH₃OH

combination reaction CO + 2H₂ → CH₃OH

Na₂O + H₂O → NaOH

combination reaction Na₂O + H₂O → 2NaOH

N₂ + H₂ → NH₃

combination reaction N₂ + 3H₂ → 2NH₃

Cu + O₂ → CuO

combustion 2Cu + O₂ → 2CuO

CH₄ + O₂ → CO₂ + H₂O

combustion CH₄ + 2O₂ → CO₂ + 2H₂O

C₂H₂ + O₂ → H₂O + CO₂

combustion reaction 2C₂H₂ + 5O₂ → 2H₂O + 4CO₂

C₅H₁₀O₂(l) + O₂(g) → CO₂(g) + H₂O(g)

combustion reaction 2C₅H₁₀O₂(l) + 13O₂(g) → 10CO₂(g) + 10H₂O(g)

SO₂(g) + O₂(g) → SO₃(g)

combustion reaction 2SO₂(g) + O₂(g) → 2SO₃(g)

Fe(s) + O₂(g) → Fe₂O₃(s)

combustion reaction 4Fe(s) + 3O₂(g) → 2Fe₂O₃(s)

Ca(OH)₂ + NH₄Cl → NH₄OH + CaCl₂

double replacement Ca(OH)₂ + 2NH₄Cl → 2NH₄OH + CaCl₂

CH₄ + H₂S → CS₂ + H₂

double replacement CH₄ + 2H₂S → CS₂ + 4H₂

What ppt do you get when an aq. solution of potassium carbonate is added to an aq. solution of silver nitrate?

silver carbonate

Al + H₂SO₄ → H₂ + Al₂(SO₄)₃

single replacement 2Al + 3H₂SO₄ → 3H₂ + Al₂(SO₄)₃

CO(g) + NO(g) → CO₂(g) + N₂(g)

single replacement 2CO(g) + 2NO(g) → 2CO₂(g) + N₂(g)

name the 7 major categories of chemical reactions.

single replacement reactions A + BX → AX + B double replacement reactions AX + BY → AY + BX Decomposition reactions A → X + Y Combination reactions A + B → AB combustion reactions nonmetal compound + oxygen → X + Y metal +oxygen → metal oxide precipitation reaction AX + BY → AY + BX(s) Acid-base reaction HA + BOH → AB + H₂O

Which of the following is soluble in H₂O? AgCl Ba₃(PO₄)₂ (NH₄)₂S PbCl₂

(NH₄)₂S

how many moles of chlorine gas (Cl₂) are in 42.0g?

0.592 mol

The reaction of 1.45 moles of Cl2 with excess F2 produced 66.9 grams of ClF3. What percentage yield of ClF3 was obtained? The balanced equation is as follows: Cl2 + 3 F2 arrow 2 ClF3 A) 4.00 % CIF3 B) 24.9 % ClF3 C) 49.9 % CIF3 D) 65.0 % CIF3 E) 32.5 % CIF3

2ClF₃ = 2(35.45+3(19)) = 184.9 * 1.45 = 268.105; 66.9/268.105 = B) 24.9 % ClF₃

What is the mass in grams of 6.20 moles of sodium?

142.5g

3.09 X 10²⁴ atoms of sulfur is equal to how many grams of sulfur?

164.6

Identify the spectator ions in the following reaction Li2CO3 + Ba(NO3) 2 Right Arrow 2 LiNO3 + BaCO3 A) Li+ and Ba2+ B) Li+ and NO3- C) Ba2+ and NO3- D) Li+ and CO32- E) Ba2+ and CO32-

B) Li+ and NO3-

HCL + NaOH →

acid- base reaction HCL + NaOH → NaCl + H₂O

H₂SO₄ + Ca(OH)₂ →

acid- base reaction H₂SO₄ + Ca(OH)₂ → CaSO₄ + 2H₂O

Fe(NO₃)₃(aq) + Na₂S(aq) → Fe₂S₃(s) + NaNO₃(aq)

precipitation reaction 2Fe(NO₃)₃(aq) + 3Na₂S(aq) → Fe₂S₃(s) + 6NaNO₃(aq)

What is the theoretical yield for the following reaction if you start with 10.0g of hydrogen and an excess of nitrogen? 3H₂ + N₂ → 2NH₃

(10/6) = (x/(2(17))) (10/6)(34)=56.7g

Consider the following unbalanced reaction: H2 + Br2 arrow HBr If the theoretical yield is 78.2 grams HBr and the percent yield is 45.0%, what is the actual yield? A) 174 grams HBr B) Not enough information is given to solve this problem. C) 0.575 grams HBr D) 1.74 grams HBr E) 35.2 grams HBr

(x/78.2g)=0.45; x = 78.2g*0.45 = E) 35.2 grams HBr

Determine the simplest formula of the compound with the following mass percents of the elements present: 17.9% Fe, 51.3% bromine and 30.8% oxygen. A) Fe(BrO3)3 B) Fe(BrO)2 C) Fe(BrO2)3 D) Fe(BrO2)2 E) Fe(BrO3)2

17.9gFe*(1moleFe/55.8gFe)=0.321moleFe 51.3gBr*(1moleFe/79.9gBr)=0.642moleBr 30.8gO*(1moleO/16.0gO)=1.93moleO E) Fe(BrO₃)₂

Balance/Complete also write net ionic rxn (NH₄)₃PO₄(aq) + CaCl₂(aq) →

2(NH₄)₃PO₄(aq) + 3CaCl₂(aq) → 6(NH₄)Cl + Ca₃(PO₄)₂ 3Ca+2 + 2PO4-3 = Ca3(PO4)2

If the theoretical yield of the reaction below is 149.2g of KOH and the actual is 30.2g of KOH what is the % yield

20.2%

Balance: Pb(NO₃)₂(g) → PbO(s) + NO(g) + O₂(g)

2Pb(NO₃)₂(g) → 2PbO(s) + 4NO(g) + 3O₂(g)

what is the molar mass of aluminum sulfate?

342.15

What is the limiting reactant for the reaction below if 5.00g of sodium and 30.0g of bromine gas react to form sodium bromide? 2Na + Br₂ → 2NaBr

5/23 = 0.217 30/160 = 0.190 for every 0.190 moles of Br₂ you need 2(0.190) = 0.375 moles of Na

What is the mass in grams of 1.00 mole of a compound with the formula C₄H₈O₂?

88g

Balance the following chemical equation by inspection, and then add the coefficients of all reactants and products to select an answer. (Do not forget to add coefficients of 1). Example: If the balanced equation is 2 Na(s) + Cl2(g) Right Arrow 2 NaCl(s), the sum of the coefficients is 5, obtained by adding 2 + 1 + 2=5. Even though there is no number in front of Cl2, it represents one molecule of chlorine, so the number 1 is used. Al(s) + HCl(aq) Right Arrow AlCl3(aq) + H2(g) A) 13 B) 7 C) 5 D) 11 E) 9

A) 13

A submarine sandwich requires one loaf of bread, 3 slices of turkey, ½ cup of shredded lettuce, 4 tomato slices, 3 slices of cheese and various spices and oil and vinegar. If you have 12 slices of turkey and enough of all the other components, how many tomato slices do you need? A) 16 tomato slices B) 12 tomato slices C) 4 tomato slices D) 6 tomato slices E) 8 tomato slices

A) 16 tomato slices

Calculate the number of grams in 0.617 moles of Ba(IO2)2. A) 281 grams Ba(IO2)2 B) 738 grams Ba(IO2)2 C) 3.71x1023 grams Ba(IO2)2 D) 455 grams Ba(IO2)2. E) 183 grams Ba(IO2)2

A) 281 grams Ba(IO2)2

All of the following compounds are soluble in water EXCEPT: A) Al(OH) 3 B) CuSO4 C) Fe(NO3) 3 D) Ca(OH) 2 E) (NH4) 2S

A) Al(OH) 3

what is the mass of a sample of A) Ca, that has Avogadro's number of atoms B) Fe, That has Avogadro's number of atoms

A) Ca = 40.08g B) Fe = 55.85g

an acid is any substance that A) produces H⁺ (aq) ions when added to water B) produces hydroxide OH⁻ (aq) ions when added to water C) contains hydrogen, H, atoms in its formula. D) forms a precipitate when added to a soluble compound.

A) produces H⁺ (aq) ions when added to water

A good hint for balancing chemical equations is A) save the elemental substances for last. B) balance the elemental substance first. C) divide all the balancing coefficients by a number that makes them all whole. D) take random guesses until you are right

A) save the elemental substances for last.

NH₄OH + H₂SO₄ → (NH₄)₂SO₄ + H₂O

Acid base 2NH₄OH + H₂SO₄ → (NH₄)₂SO₄ + 2H₂O

The theoretical yield is how much product can be produced from specific amounts of reactants. Very often the theoretical yield is a much higher value than the actual yield obtained in a reaction. The factors that may reduce the actual yield are... 1. competing side reactions may consume part of the reactants. 2. one of the reactants is in excess. 3. difficulties in collecting the products. 4. difficulties in purifying the products. A) 1 and 2 B) 1, 3, and 4 C) 1, 2, and 3 D) 3 and 4 E) 2, 3, and 4

B) 1, 3, and 4

A piece of copper pipe has 9.78 ×1025 copper atoms. How much does the piece of pipe weigh in grams? A) 6.21 × 10²⁷ grams Cu B) 1.03 × 10⁴ grams Cu C) 6.49 × 10⁻²⁵ grams Cu D) 2.55 grams Cu E) 162 grams Cu

B) 1.03 × 10⁴ grams Cu

Balance the following chemical equation by inspection, and then add the coefficients of all reactants and products to select an answer. (Do not forget to add coefficients of 1). C3H6O(l) + O2(g) Right Arrow CO2(g) + H2O(l) A) 17 B) 11 C) 14 D) 23 E) 20

B) 11

How many moles of hydrogen atoms are there in 50.0 grams of ammonia, NH3? A) 2.94 moles hydrogen atoms B) 8.82 moles hydrogen atoms C) 1.59 × 10⁻²⁵ moles hydrogen atoms D) 1.47 × 10⁻²³ moles hydrogen E) 3.40 × 10⁻¹ moles hydrogen

B) 8.82 moles hydrogen atoms

A precipitation reaction is A) a single-replacement reaction B) a double- replacement reaction C) a combination reaction D) B and C

B) a double- replacement reaction

the energy required to yield a chemical change in a gas-phase reaction A) comes from high-energy electrons. B) comes from collisions between molecules. C) is supplied by the products. D) has nothing to do with the reactant molecules.

B) comes from collisions between molecules.

To find if there is a limiting reactant requires A) removing the balancing coefficients from the chemical equation B) dividing the moles of each reactant present by its balancing coefficient from the balanced chemical equation C) multiplying the moles of each reactant present by its balancing coefficient from the balanced chemical equation D) adding up the moles of products and reactants

B) dividing the moles of each reactant present by its balancing coefficient from the balanced chemical equation

It is possible to go from a molecular formula to percent by mass composition for each element because A) the formula subscripts can be interpreted as grams of each element present B) the formula subscripts can be interpreted as moles of each element present C) the empirical formula is a multiple of the actual formula D) it is not possible to go from formula to percent composition; it is only possible to go the other way

B) the formula subscripts can be interpreted as moles of each element present

Stoichiometry is the study of A) the energetics of a reaction. B) the quantitative aspects of a reaction C) how reactants turn into products D) stoicheons (Greek for elements) involved in a chemical reaction

B) the quantitative aspects of a reaction

Which one of the following is true about chemical reactions? A) They accomplish only physical changes. B) they are represented with a chemical equation C) Products are converted into reactants. D) the arrow means "heat and stir."

B) they are represented with a chemical equation

which of the following gives a ppt when an aq. solution of Na₂SO₄ is added to an aq. solution of each below? BaCl₂ FeCl₃ MgCl₂ KCl LiBr

BaCl₂

How many atoms of titanium are there in 100. grams of Ti? A) 4.79 × 10³ atoms Ti B) 6.02 × 10²⁵ atoms Ti C) 1.26 × 10²⁴ atoms Ti D) 2.09 atoms Ti E) 4.79 × 10⁻¹ atoms Ti

C) 1.26 × 10²⁴ atoms Ti

From the following, identify the acid-base reaction 1. Mg + SnBr2 Right Arrow MgBr2 + Sn 2. 2 LiCl + Ba(OH) 2 Right Arrow 2 LiOH + BaCl2 3. NH4OH + HNO3 Right Arrow NH4NO3 + H2O 4. MnSO4 + 2 NaC2H3O2 Right Arrow Mn(C2H3O2)2 + Na2SO4 5. 2 Al + 3 Br2 Right Arrow 2 AlBr3 A) 2 B) 5 C) 3 D) 4 E) 1

C) 3

From the following, identify the precipitation reactions 1. Sr + SnBr2 Right Arrow SrBr2 + Sn 2. 2 LiNO3 + Ba(OH) 2 Right Arrow 2 LiOH + Ba(NO3) 2 3. 2 NH4I + Pb(NO3) 2 Right Arrow 2 NH4NO3 + PbI2 4. K2SO4 + Ca(C2H3O2) 2 Right Arrow 2 KC2H3O2 + CaSO4 A) 1 and 2 B) 1 and 3 C) 3 and 4 D) 2 and 3 E) 2 and 4

C) 3 and 4

Classify the following reaction: Mg(s) + 2 HBr(aq) Right Arrow MgBr2(aq) + H2(g) A) Combustion reaction B) Combination reaction C) Single-replacement reaction D) Decomposition reaction E) Double-replacement reaction

C) Single-replacement reaction

A precipitation reaction will occur when A) the reactants and products are incompatible. B) all of the reactants are soluble. C) at least one of the possible products is insoluble D) all of the reactants are insoluble.

C) at least one of the possible products is insoluble

Which one of the following is true about chemical bonds? A) it takes energy to break a bond only for polar compounds. B) energy is released when breaking weak bonds. C) it always takes energy to break chemical bonds. D) they can survive molecular collisions of any amount of energy.

C) it always takes energy to break chemical bonds.

One mole of an element weighs A) its atomic mass divided by 6.022 X 10²³ /mol B) its atomic mass times 6.022 X 10²³ /mol C) its atomic mass listed on the periodic table in grams. D) one-twelfth its atomic mass listed on the periodic table in grams

C) its atomic mass listed on the periodic table in grams.

To write a net ionic equation, you must A) write every species in solution B) include the spectator ions. C) omit the spectator ions. D) write the precipitate with (aq) after it.

C) omit the spectator ions.

complete & balance: H₂SO₄ + Ca(OH)₂ →

CaSO₄ + 2H₂O

C₂H₄ + O₂ → CO₂ + H₂O

Combution reaction C₂H₄ + 3O₂ → 2CO₂ + 2H₂O

For the following reaction, calculate the number of moles of Cu that can be produced from 30.1 grams of Cu2SO4 with excess Na. 2 Na + Cu2SO4 arrow Na2SO4 + 2 Cu A) 17.1 moles Cu B) 0.270 moles Cu C) 0.948 moles Cu D) 60.2 moles Cu E) 0.135 moles Cu

Cu₂SO₄ = 2(63.5)+32.06+4(16) = 223.06g/mol; (30.1g/223.06g/mol)*(2*63.5) = 17.3/63.5 = B) 0.270 moles Cu

A compound that contains carbon, hydrogen and oxygen is found to have an empirical formula of C3H4O. If the molar mass of this compound is 224 g/mol, what is its molecular formula? A) C9H12O3 B) C3H4O C) C6H8O2 D) C12H16O4 E) C15H20O5

C₃H₄O = 3(12)+4+16 = 56; 224/56 = 4; C(4*3)H(4*4)O(4) = D) C₁₂H₁₆O₄

A compound has the empirical formula C₂H₄O Its molar mass is about 88g/mol what is the molecular formula.

C₄H₈O₂

Predict the products for the following precipitation reaction. NH4Cl(aq) + Pb(NO3) 2(aq) Right Arrow A) NO3Cl + Pb(NH4) 2 B) NH4Cl + NO2 + PbO C) NH3 + HCl + Pb(NO3) 2 D) 2NH4NO3 + PbCl2 E) NH4Cl + Pb(NO3)2

D) 2NH4NO3 + PbCl2

A limiting reactant A) is always present in a reaction B) makes it impossible to write a balanced chemical equation C) ends up becoming an excess reactant D) Limits the yield of a reaction

D) Limits the yield of a reaction

For the reaction CH₄ + O₂ → CO₂ + H₂O A) a2 is needed in front of H₂O B) a 2 is needed in front of O₂ C) a 2 in needed in front of CH₄ and CO₂ D) a 2 is needed in front of O₂ and H₂O

D) a 2 is needed in front of O₂ and H₂O

A balanced chemical equation can always be read A) in terms of individual molecules B) in terms of moles of molecules C) in terms (as a source) of conversion factors D) all of the above are correct

D) all of the above are correct

In grams, one mole of a molecule weighs A) the sum of its constituent element atomic masses, each multiplied by its subscript in the formula. B) its molar mass in grams C) 6.022 X 10²³ times the mass of one single molecule in grams D) all of the above are correct

D) all of the above are correct

The mole is A) the number of ¹²₆C atoms in exactly 12g of ¹²₆C B) 6.022 X 10²³ of anything C) also called Avogadro's number D) all of the above are correct statments

D) all of the above are correct statments

A combination reaction is a reaction in which A) the chemical properties of the reactants are combined. B) decomposition occurs. C) atoms are exchanged between reactants D) different reactant molecules are combined to yield products.

D) different reactant molecules are combined to yield products.

Conversion factors are A) never written in fractional form (something over something else) B) used to eliminate all units from a calculation C) used to improve accuracy and precision of a calculated result D) used to translate or convert from one unit to another unit.

D) used to translate or convert from one unit to another unit.

NaCl → Na + Cl₂

Decomposition 2NaCl → 2Na + Cl₂

Balance the following chemical equation by inspection. What is the coefficient for Na2O? CaO + Na3P Right Arrow Ca3P2 + Na2O A) 2 B) 5 C) 1 D) 4 E) 3

E) 3

Identify the double-replacement reaction from the choices below. A) Sr + FeBr2 Right Arrow SrBr2 + Fe B) H2CO3 Right Arrow CO2 + H2O C) C3H8(l) + 5 O2(q) Right Arrow 3 CO2(q) + 4 H2O(l) D) 2 Ga + 3 Br2 Right Arrow 2 GaBr3 E) 3 K2O + Ba3N2 Right Arrow 2 K3N + 3 BaO

E) 3 K2O + Ba3N2 Right Arrow 2 K3N + 3 BaO

Aqueous solutions of aluminum nitrate and potassium phosphate combine to produce a precipitate. This precipitate is A) AlK3 B) Al(NO3) 3 C) K3PO4 D) KNO3 E) AlPO4

E) AlPO4

What is the net ionic equation for the following acid-base neutralization reaction? H2SO4(aq) + 2 NaOH(aq) Right Arrow Na2SO4(aq) + 2 H2O(l) A) H2SO4(aq) Right Arrow 2 H+ + SO42− B) 2NaOH(aq)Right Arrow 2 Na+ + 2 OH− C) 2 H+ + SO42− + 2 Na+ + 2 OH− Right Arrow 2 Na+ + SO42− + 2 H2O(l) D) 2 Na+ + SO42− Right Arrow Na2SO4(aq) E) H+(aq) + OH−(aq) Right Arrow H2O(l)

E) H+(aq) + OH−(aq) Right Arrow H2O(l)

What is the net ionic reaction for the reaction of hydrochloric acid and sodium hydroxide?

H⁺ + ⁻OH → H₂O

Write the balanced ionic reaction for any acid-base reaction.

H⁺ + ⁻OH → H₂O

Which one is soluble in water. K₂CO₃ CaCO₃ CuCO₃ SrCO₃

K₂CO₃

which is insoluble in water MgSO₄ Mg₃(PO₄)₂ MgI₂ Mg(NO₃)₂

Mg₃(PO₄)₂

For 1 mole of each of the following, how many moles of hydrogen atoms are there? NaOH C₆H₅OH (NH₄)₂HPO₄

NaOH = 1 mol C₆H₅OH = 6 mol (NH₄)₂HPO₄ = 9 mol

Consider the following balanced equation: PBr3 + 3 H2O arrowH3PO3 + 3 HBr How many grams of water are required to react completely with 20.0 g PBr3? A) 0.443 grams H2O B) 60.0 grams H2O C) 3.99 grams H2O D) 0.221 grams H2O E) 1.33 grams H2O

PBr₃ = 31+3(80) = 271g/mol; 3H₂0 = 3(2+16) = 54g/mol; 20g/271g/mol = 0.074mol; 54g/mol*0.074mol = C) 3.99 grams H₂O

Which of the following is insoluble in H₂O? Ca(NO₃)₂ PbSO₄ Na₂S K₃PO₄

PbSO₄

HCl + NH₄OH →

acid- base reaction HCl + NH₄OH → NH₄Cl + H₂O

HNO₃ + KOH →

acid- base reaction HNO₃ + KOH → KNO₃ + H₂O

H₂SO₄ + Mg(OH)₂ →

acid- base reaction H₂SO₄ + Mg(OH)₂ → MgSO₄ + 2H₂O

What is the rxn type between sodium hydroxide (aq) and acetic acid (aq)? acid/Base precipitation oxidation/reduction gas evolution decomposition

acid/Base

Tell whether each of the following is soluble or insoluble in water ammonium chloride iron(III) chloride barium chloride magnesium bromide mercury(I) chloride calcium sulfide

ammonium chloride = soluble iron(III) chloride = soluble barium chloride = soluble magnesium bromide = soluble mercury(I) chloride = insoluble calcium sulfide = soluble

KClO₃ → KCl + O₂

decomposition reaction 2KClO₃ → 2KCl + 3O₂

N₂O₅(g) → NO₂(g) + O₂(g)

decomposition reaction 2N₂O₅(g) → 4NO₂(g) + O₂(g)

AsCl₃ + H₂S → As₂S₃ + HCl

double replacement 2AsCl₃ + 3H₂S → As₂S₃ + 6HCl

What type of rxn is this and balance AgNO₃(aq) + NaCl(aq) →

precipitation reaction AgCl(s) + NaNO₃

Pb(NO₃)₂(aq) + K₂CrO₄(aq) → KNO₃(aq) + PbCrO₄(s)

precipitation reaction Pb(NO₃)₂(aq) + K₂CrO₄(aq) → 2KNO₃(aq) + PbCrO₄(s)

Fe₂O₃ + H₂ → Fe + H₂O

single replacement Fe₂O₃ + 3H₂ → 2Fe + 3H₂O

Fe₂O₃ + C → Fe + CO₂

single replacement 2Fe₂O₃ + 3C → 4Fe + 3CO₂

Zn + HCl → ZnCl₂ + H₂

single replacement Zn + 2HCl → ZnCl₂ + H₂

if I mix solutions of calcium chloride and potassium carbonate do I get a ppt.

yes = calcium carbonate