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27 days ago

gypsum is insoluble in water. you are asked to purify a sample of gypsum that is contaminated with a soluble salt.

Chemistry

1 answer:

KiRa [2.7K]27 days ago

7 0

Response:

a. To purify a gypsum sample, you will need the following equipment: Bunsen burner, beaker, filter funnel, stirring rod, and filter paper.

b. Gypsum, a sulfate mineral consisting of calcium sulfate dihydrate, can be purified by following these steps:

1. Add water to the gypsum in a beaker.

2. Stir the mixture thoroughly with the stirring rod.

3. Use the filter paper and filter funnel to remove excess solids from the mixture.

4. Heat the filtered mixture on the Bunsen burner to evaporate the remaining water.

5. After cooling, filter again through the filter paper to obtain pure gypsum.

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An average copper penny minted in the 1960s contained about 3.000 g of copper. how much chalcopyrite had be mined to produce 100

lorasvet [2542]

To find the answer, start by calculating the total mass of the copper utilized:

Copper used = 100 pennies x 3.0g Cu per penny = 300.0 g Cu

Next, identify the path and molar ratios from Cu produced back to CuFeS2 needed using the established balanced reactions:

1 Cu2S from 2 CuS; 2Cu from 1 Cu2S; 2CuS from 2CuFeS2
Thus, 2Cu comes from 2CuFeS2, indicating a 1:1 molar ratio.

Then convert grams of Cu to moles and grams of CuFeS2:
= 300.0 g Cu * 1 mol Cu/63.546g Cu * 2 mol CuFeS2/2 moles Cu

= 4.72 moles CuFeS2

The required amount of chalcopyrite mined = 4.72 moles CuFeS2 * 183.54 g CuFeS2/1 mole CuFeS2 = 866.49 g CuFeS2

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22 days ago

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his is the chemical formula for chromium(III) nitrate: . Calculate the mass percent of oxygen in chromium(III) nitrate. Round yo

eduard [2520]

Answer:

$\%\ Composition\ of\ iron=69.92\ \%$

Explanation:

The percent composition indicates the mass percentage of a specific element within the compound.

The chemical formula for chromium(III) nitrate is $Cr(NO_3)_3$ .

The molar mass for chromium(III) nitrate is calculated at 238.011 g/mol.

Each mole of chromium(III) nitrate includes 9 moles of oxygen.

The molar mass of oxygen is 16 g/mol.

Hence, Mass = Molar mass * Moles = 16 * 9 g = 144 g.

$\%\ Composition\ of\ iron=\frac{Mass_{iron}}{Total\ mass}\times 100$

$\%\ Composition\ of\ iron=\frac{144}{238.011}\times 100$

$\%\ Composition\ of\ iron=69.92\ \%$

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1 month ago

Calculate the grams of so2 gas present at stp in a 5.9 l container. (r = 0.0821 l·atm/k·mol)

KiRa [2726]

At standard conditions of 1 atm and 273 K, the specific volume for any ideal gas is set at 22.4 L/mol. Therefore, the moles of SO₂ can be calculated as 5.9 L multiplied by 1 mol/22.4 L, equating to 0.263 mol. The molar mass of SO₂ is 64.066 g/mol, leading to a mass of 0.263 mol multiplied by 64.066 g/mol, resulting in 16.87 g of SO₂.

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15 days ago

Based on the bond energies for the reaction below, what is the enthalpy of the reaction?HC≡CH (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O

alisha [2718]

Answer:

1219.5 kJ/mol

Explanation:

The calculation for this value requires using the following equation:

ΔHºrxn = Σn * (BE of reactants) - Σn * (BE of products)

ΔHºrxn = [1 * (BE C = C) + 2 * (BE C-H) + 5/2 * (BE O = O)] - [4 * (BE C = O) + 2 * (BE O-H)].

The bond energy (BE) values are:

BE C = C: 839 kJ/mol

BE C-H: 413 kJ/mol

BE O = O: 495 kJ/mol

BE C = O: 799 kJ/mol

BE O-H: 463 kJ/mol

By substituting these values into the equation, you will get:

ΔHºrxn = [1 * 839 + 2 * (413) + 5/2 * (495)] - [4 * (799) + 2 * (463)] = 1219.5 kJ/mol

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1 month ago

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eduard [2520]

Molarity is calculated using moles divided by the volume in liters. Convert 200 mL to 0.2 L, then divide 2 moles by 0.2 L.

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