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3 years ago

An igneous rock that contains mostly proxene and olivene has ___.

Chemistry

1 answer:

tangare [24]3 years ago

6 0

It has an ultramafic composition
Hope this helps ;)

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Is magnetism, reactivity, and fluorescence used to identify minerals

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Yes it is used , hope this helps

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3 years ago

True or Flase: dissolving salt in distilled water creates a homogeneous mixture.

chubhunter [2.5K]

Answer:

true

Explanation:

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3 years ago

Read 2 more answers

Ammonia reacts with sulfuric acid to produce the important fertilizer, ammonium hydrogen sulfate.

Liula [17]

Answer:

404.8g of (NH4)HSO4 is produced.

Explanation:

Step 1:

Data obtained from the question. This include the following:

Temperature (T) = 10°C = 10°C + 273 = 283K

Pressure (P) = 110KPa = 110/101.325 = 1.09atm

Volume (V) = 75L

Step 2:

Determination of the number of mole of ammonia, NH3.

The number of mole (n) of ammonia, NH3 can be obtained by using the ideal gas equation. This is illustrated below:

Note:

Gas constant (R) = 0.0821atm.L/Kmol

Number of mole (n) =?

PV = nRT

1.09 x 75 = n x 0.0821 x 283

Divide both side by 0.0821 x 283

n = (1.09 x 75) /(0.0821 x 283)

n = 3.52 moles

Step 3:

Determination of the number of mole ammonium hydrogen sulfate produced from the reaction.

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

NH3 + H2SO4 —> (NH4)HSO4

From the balanced equation above,

1 mole of NH3 produced 1 mole of (NH4)HSO4

Therefore, 3.52 moles of NH3 will also produce 3.52 moles of (NH4)HSO4.

Therefore, 3.52 moles of ammonium hydrogen sulfate, (NH4)HSO4 is produced.

Step 4:

Conversion of 3.52 moles of ammonium hydrogen sulfate, (NH4)HSO4 to grams. This is illustrated below:

Molar Mass of (NH4)HSO4 = 14 + (4x1) + 1 + 32 + (16x4) = 115g/mol

Number of mole of (NH4)HSO4 = 3.52 moles

Mass of (NH4)HSO4 =..?

Mass = mole x molar Mass

Mass of (NH4)HSO4 = 3.52 x 115 = 404.8g

Therefore, 404.8g of (NH4)HSO4 is produced.

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3 years ago

Binomial nomenclature example and sentence using that word<br><br> please help im going to cry

Alexandra [31]

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3 years ago

complete and balance the molecular equation for the reaction of aqueous copper(II) chloride, CuCl2,CuCl2, and aqueous potassium

oee [108]

Answer : The net ionic equation will be,

$3Cu^{2+}(aq)+2PO_4^{3-}(aq)\rightarrow Cu_3(PO_4)_2(s)$

Explanation :

First we have to balance the chemical reaction.

The given balanced ionic equation will be,

$3CuCl_2(aq)+2K_3PO_4(aq)\rightarrow Cu_3(PO_4)_2(s)+6KCl(aq)$

In the net ionic equations, we are not include the spectator ions in the equations.

Spectator ions : The ions present on reactant and product side which do not participate in a reactions. The same ions present on both the sides.

The ionic equation in separated aqueous solution will be,

$3Cu^{2+}(aq)+6Cl^-(aq)+6K^+(aq)+2PO_4^{3-}(aq)\rightarrow Cu_3(PO_4)_2(s)+6K^+(aq)+6Cl^-(aq)$

In this equation, $K^+\text{ and }Cl^-$ are the spectator ions.

By removing the spectator ions from the balanced ionic equation, we get the net ionic equation.

The net ionic equation will be,

$3Cu^{2+}(aq)+2PO_4^{3-}(aq)\rightarrow Cu_3(PO_4)_2(s)$

4 0

3 years ago