What can you extract from a refinery

Molecules that contain nothing but hydrogen and carbon are

romanna [79]

Hydrocarbons. They usually burn. In fact, I can't think of one that does not.

4 0

3 years ago

EXPLAIN How did energy change form in the calorimeter lab?

timama [110]

Answer:

Chemical energy is converted into thermal and mechanical energy while kinetic energy into potential energy.

Explanation:

As the breakdown of food started, the chemical energy present in the food substances converted into thermal energy and mechanical energy. Thermal or heat energy is used to maintain the body's temperature while mechanical energy is used in other activities such as movement of muscles. Kinetic energy is also converted into potential energy when the object moves from top of a place such as hill.

7 0

3 years ago

Read 2 more answers

Can someone help me balance this equation please?<br> Br2 + S2O32– + H2O → Br1– + SO42– + H+

tamaranim1 [39]

Explanation:

Br2 + S2O32- + 5H2O –> 2Br- + 2SO4 + 10H+ + 6e

7 0

2 years ago

A molecule has one carbon-carbon double bond and four monovalent atoms or groups. How many different cis-trans isomers exist for

Lena [83]

There can be two cases

Case 1:

When a molecule has one carbon-carbon double bond and four monovalent atoms or groups in which two atoms on same carbon are different, there will be 2 isomers, one cis and one trans.

Case 2:

When a molecule has one carbon-carbon double bond and four monovalent atoms or groups where both atoms attached to the same carbon are same, there will be no geometrical isomerism.

As based on priority, there will be only two orientations possible , in which same priority atoms are on the same side that is cis and if they are on the opposite side that is trans.

3 0

4 years ago

if 14.0 g of aluminium reacts with excess sulfuric acid to produce 75.26 g of aluminium sulfate, what is the percent yield?

vlada-n [284]

Taking into account definition of percent yield, the percent yield for the reaction is 84.88%.

<h3>Reaction stoichiometry</h3>

In first place, the balanced reaction is:

2 Al + 3 H₂SO₄ → Al₂(SO₄)₃ + 3 H₂

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

Al: 2 moles
H₂SO₄: 3 moles
Al₂(SO₄)₃. 1 mole
H₂: 3 moles

The molar mass of the compounds is:

Al: 27 g/mole
H₂SO₄: 98 g/mole
Al₂(SO₄)₃: 342 g/mole
H₂: 2 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

Al: 2 moles ×27 g/mole= 54 grams
H₂SO₄: 3 moles ×98 g/mole= 294 grams
Al₂(SO₄)₃: 1 mole ×342 g/mole= 342 grams
H₂: 3 moles ×2 g/mole= 6 grams

<h3>Mass of aluminium sulfate formed</h3>

The following rule of three can be applied: if by reaction stoichiometry 54 grams of aluminium form 342 grams of aluminium sulfate, 14 grams of aluminium form how much mass of aluminium sulfate?

$mass of aluminium sulfate=\frac{14 grams of aluminium x342 grams of aluminium sulfate}{54 grams of aluminium}$

<u><em>mass of aluminium sulfate= 88.67 grams</em></u>

Then, 88.67 grams of aluminium sulfate can be produced if 14.0 g of aluminium reacts with excess sulfuric acid.

<h3>Percent yield</h3>

The percent yield is the ratio of the actual return to the theoretical return expressed as a percentage.

The percent yield is calculated as the experimental yield divided by the theoretical yield multiplied by 100%:

$percent yield=\frac{actual yield}{theorical yield} x100$

where the theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product, that is, it is the maximum amount of product that could be formed from the given amounts of reagents.

<h3>Percent yield for the reaction in this case</h3>

In this case, you know: