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Akimi4 [234]
2 years ago
15

1. Complete the balanced dissociation equation for the compound below. If the compound does not dissociate, write NR after the r

eaction arrow.
(NH4)2S(s) -> ______


2. Write the balanced NET ionic equation for the reaction when Al(NO₃)₃ and Na₃PO₄ are mixed in aqueous solution. If no reaction occurs, write only NR.
Chemistry
1 answer:
puteri [66]2 years ago
7 0

Answer:

1. (NH₄)₂S(s) -----> NH₄+(aq) + S²-(aq)

2. Al³+ (aq) + PO₄³+ (aq) ----> AlPO₄ (s)

Explanation:

The dissociation of ammonium sulphide, (NH₄)₂S when dissolved in water is given in the equation below:

(NH₄)₂S(s) -----> NH₄+(aq) + S²-(aq)

However very little S²- ions are present in solution due to the very basic nature of the S²- ion (Kb = 1 x 105).

The ammonium ion being a better proton donor than water, donates a proton to sulphide ion to form hydrosulphide ion which exists in equilibrium with aqueous ammonia.

S²- (aq) + NH₄+ (aq) ⇌ SH- (aq) + NH₃ (aq)

Aqueous solutions of ammonium sulfide are smelly due to the release of hydrogen sulfide and ammonia, hence, their use in making stink bombs.

2. The reaction between aluminium nitrate and sodium phosphatein aqueous solution is a double decomposition reaction whish results in the precipitation of insoluble aluminium phosphate. The equation of the reaction is given below :

Al(NO₃)₃ (aq) + Na₃PO₄ (aq) ----> AlPO₄ (s) + 3 NaNO₃ (aq)

The net ionic equation is given below:

Al³+ (aq) + PO₄³+ (aq) ----> AlPO₄ (s)

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Marina CMI [18]

Answer:

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Type the correct answer in the box. Express your answer to three significant figures. This balanced equation shows the reaction
Ratling [72]

Answer:

514.5 g.

Explanation:

  • The balanced equation of the reaction is: 2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O.
  • It is clear that every 2.0 moles of NaOH react with 1.0 mole of H₂SO₄ to produce 1.0 mole of Na₂SO₄ and 2.0 moles of 2H₂O.
  • Since NaOH is in excess, so H₂SO₄  is the limiting reactant.
  • We need to calculate the no. of moles of 355.0 g of H₂SO₄:

n of H₂SO₄ = mass/molar mass = (355.0 g)/(98.0 g/mol) = 3.622 mol.

Using cross multiplication:

∵ 1.0 mol H₂SO₄ produces → 1.0 mol of Na₂SO₄.

∴ 3.622 mol H₂SO₄ produces → 3.662 mol of Na₂SO₄.

  • Now, we can get the theoretical mass of Na₂SO₄:

∴ mass of Na₂SO₄ =  no. of moles x molar mass = (3.662 mol)(142.04 g/mol) = 514.5 g.

8 0
3 years ago
B) How many kilograms of carbon dioxide are formed when 24.42 g of iron is<br> produced?
charle [14.2K]

Answer:

0.0289 kg of CO2 will be formed

Explanation:

Step 1: Data given

Mass of iron produced = 24.42 grams

Atomic mass iron = 55.845 g/mol

Molar mass CO2 = 44.01 g/mol

Step 2: The balanced equation

Fe2O3 + 3CO → 2Fe + 3CO2

Step 3: Calculate moles iron

Moles iron = mass iron / molar mass iron

Moles iron = 24.42 grams / 55.845 g/mol

Moles iron = 0.437 moles

Step 4: Calculate moles CO2

For 1 mol Fe2O3 we need 3 moles CO to produce 2 moles Fe and 3 moles CO2

For 0.437 moles Fe we'll have 3/2 * 0.437 = 0.6555 moles CO2

Step 5: Calculate mass CO2

Mass CO2 = moles CO2 * molar mass CO2

Mass CO2 = 0.6555 moles * 44.01 g/mol

Mass CO2 = 28.85 grams = 0.0289 kg

0.0289 kg of CO2 will be formed

5 0
3 years ago
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