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3 years ago

Several ways in which water is an unusual List several ways in substance.

1 answer:

4 0

Boiling Point and Freezing Point., Surface Tension, Heat of Vaporization, and Vapor Pressure, Viscosity and Cohesion, solid State, Liquid State, Gas State.

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Which of the following compounds would be expected to have the strongest ionic bonds?

Luba_88 [7]

Answer:

Compound that has the smallest ions with the greatest charge.

Explanation:

4 0

3 years ago

Read 2 more answers

Ammonia (NH3) is one of the most common chemicals produced in the united states. it is used to make fertilizer and other product

Greeley [361]

Answer:

a) N2 is the limiting reactant

b) 1215.9 grams NH3

c) 2283.6 grams H2

Explanation:

Step 1: Data given

Mass of N2 = 1000 grams

Molar mass N2 = 28 g/mol

Mass of H2 = 2500 grams

Molar mass H2 = 2.02 g/mol

Step 2: The balanced equation

N2(g) +3H2(g) → 2NH3(g)

Step 3: Calculate moles N2

Moles N2 = mass N2 / molar mass N2

Moles N2 = 1000 grams / 28.0 g/mol

Moles N2 = 35.7 moles

Step 4: Calculate moles H2

Moles H2 = 2500 grams / 2.02 g/mol

Moles H2 = 1237.6 moles

Step 5: Calculate limiting reactant

For 1 mol N2 we need 3 moles H2 to produce 2 moles NH3

N2 is the limiting reactant. There will be consumed 35.7 moles.

H2 is in excess. There will react 3*35.7 = 107.1 moles

There will remain 1237.6 - 107.1= 1130.5 moles H2

This is 1130.5 * 2.2 = 2283.6 grams H2

Step 6: Calculate moles NH3

For 1 mol N2 we need 3 moles H2 to produce 2 moles NH3

For 35.7 moles N2 we'll have 2*35.7 = 71.4 moles NH3

Step 7: Calculate mass NH3

Mass NH3 = moles NH3 * molar mass NH3

Mass NH3 = 71.4 moles * 17.03 g/mol

Mass NH3 = 1215.9 grams NH3

7 0

3 years ago

1. Describe how an acidic solution forms when HCl is mixed in water and how a basic solution forms when NaOH is mixed in water.

NeX [460]

Answer:

Dissociation

Explanation:

When HCl and NaOH are mixed with water, the HCl and NaOH molecules interacts with the water, forming what is known as ions. Ions are atoms with electric charge.

When HCl, it forms H+ and Cl-. The mixture is acid because what define a mixture as acid is the amount of H+ ions.

When NaOH mixes with water, it forms Na+ and OH- ions. The amount of OH- ions in a mixture defines it as basic.

6 0

3 years ago

Name the type of bond in organic chemistry that corresponds to a glycoside bond

Semenov [28]

Answer:

covalent bond

Explanation:

The bond which is most common in the organic molecules is the covalent bond which involves sharing of the electrons between the two atoms.

Glycosidic bond, also known as glycosidic linkage is type of the covalent bond which joins carbohydrate molecule to other group that may not or may be a carbohydrate.

Glycosidic bond is the bond which is formed between hemiacetal or hemiketal group of the saccharide and hydroxyl group of compounds like alcohol.

5 0

3 years ago

Write the balanced chemical equation for the complete, stoichiometric combustion of ethylene in (a) nitrous oxide and (b) air. C

Liono4ka [1.6K]

Answer: Mass of nitrous oxide used is 264 grams and mass of oxygen gas used is 96 grams.

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ....(1)

For a: Combustion of ethylene in nitrous oxide

The chemical equation for the combustion of ethylene in nitrous oxide follows the equation:

$C_2H_4+N_2O\rightarrow 2CO_2+2H_2O+6N_2$

By stoichiometry of the reaction;

6 moles of nitrous oxide are required for the complete combustion of ethylene molecule.

Calculating the mass of nitrous oxide using equation 1:

Molar mass of nitrous oxide = 44 g/mol

Moles of nitrous oxide = 6 moles

Putting values in equation 1, we get:

$6mol=\frac{\text{Mass of nitrous oxide}}{44g/mol}\\\\\text{Mass of nitrous oxide}=264g$

Thus, 264 grams of nitrous oxide are required for the complete combustion of ethylene.

For b: Combustion of ethylene in air

The chemical equation for the combustion of ethylene in air follows the equation:

$C_2H_4+3O_2\rightarrow 2CO_2+2H_2O$

By stoichiometry of the reaction;

3 moles of oxygen are required for the complete combustion of ethylene molecule.

Calculating the mass of oxygen using equation 1:

Molar mass of oxygen = 32 g/mol

Moles of oxygen = 3 moles

Putting values in equation 1, we get:

$3mol=\frac{\text{Mass of oxygen}}{32g/mol}\\\\\text{Mass of oxygen}=96g$

Thus, 96 grams of oxygen are required for the complete combustion of ethylene.

7 0

3 years ago