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3 years ago

Feldspars producing clay is an example of ___

Chemistry

1 answer:

BaLLatris [955]3 years ago

3 0

Answer: A

Explanation:

Hydrolysis reactions break down not only feldspars but many other silicate minerals as well, amphiboles, pyroxenes, micas, and olivines.

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Bryan and Alyssa are playing tug-of-war against Daniel and Maria. Bryan and Alyssa are exerting a combined force of 10 N. Daniel

mr_godi [17]

Answer:

Explanation:

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2 years ago

A particle that makes up the basic unit of an element is called an __________.

AleksAgata [21]

I think it’s atoms because of google

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3 years ago

Write and balance the equation for the combination of ammonia gas with solid copper (II) oxide to produce copper metal, nitrogen

Katena32 [7]

Explanation :

The balanced chemical reaction will be,

$3CuO(s)+2NH_3(g)\rightarrow 3Cu(s)+N_2(g)+3H_2O(l)$

By the stiochiometry, 3 moles of solid copper(II)oxide react with 2 moles of ammonia gas to give 3 moles of copper metal, 1 mole of nitrogen gas and 3 moles of liquid water.

The states of matter of each elements and compound is,

Copper(II)oxide is in solid state

Ammonia is in gaseous state

Copper metal is in solid state

Nitrogen is in gaseous state

Water is in liquid state

7 0

2 years ago

Read 2 more answers

Complete the mechanism for the reaction of 2-butanol in sulfuric acid at 140 °C by adding any missing atoms, bonds, charges, non

Svetlanka [38]

Answer:

2-Butene

Explanation:

The first step is the ionization of the acid to produce the hydronium ion. Then the OH will attack this ion to produce a charged species that can be stabilized when H2O is produced.

Then an elimination takes place to produce the more substituted alkene 2-butene and the hydronium ion is gain produced.

4 0

2 years ago

The density of water is 1.00 g/ml at 4°c. how many water molecules are present in 2.56 ml of water at this temperature?

o-na [289]

Answer:

8.55 × 10²² Molecules

Solution:

Step 1: Calculate the Mass of Water as;

Density = Mass ÷ Volume

Solving for Mass,

Mass = Density × Volume

Putting values,

Mass = 1 g.mL⁻¹ × 2.56 mL

Mass = 2.56 g

Step 2: Calculate Moles of Water as,

Moles = Mass ÷ M.Mass

Putting values,

Moles = 2.56 g ÷ 18 g.mol⁻¹

Moles = 0.142 mol

Step 3: Calculate Number of Molecules of Water as,

# of Molecules = Moles × 6.022 × 10²³

Putting value of mole,

# of Molecules = 0.142 × 6.022 × 10²³

# of Molecules = 8.55 × 10²² Molecules

5 0

3 years ago