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4 years ago

Why are some rocks more easily weathered than other rocks

1 answer:

3 0

Because of their atom's composition. some are naturally packed closer together and stronger and more durable, while others tend to be more loose and breakable and/or weaker/less durable. also with how their atoms are composed is how the atoms interact with each other/ how they share or give or take electrons.

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Solid iron(III) oxide reacts with hydrogen gas to form solid iron and liquid water.

Marrrta [24]

Hello, this question is incomplete. The complete question would be:

"Write the balanced chemical equation for the following reaction.

Solid iron(III) oxide reacts with hydrogen gas to form solid iron and liquid water"

Answer:

Fe2O3 + 3 H2 = 2 Fe + 3 H2O

Explanation:

In a chemical reaction, the structure of atoms as chemical elements is unchanged. Atoms in one element do not become atoms in another element. There is also no loss or creation of new atoms. The number of atoms of the reagents must be equal to the number of atoms of the products. When this happens, we say that the chemical equation is balanced.

For this reason, we can state that the balanced chemical reaction where solid iron (III) oxide reacts with hydrogen gas to form solid iron and liquid water would be:

5 0

3 years ago

Given the balanced equation 2C4H10 + 13O2 → 8CO2 + 10H2O, how many moles of CO2 are produced when 14.9g of O2 are used?

Anna [14]

Answer: The number of moles of $CO_2$ produced are, 0.287 moles.

Explanation : Given,

Mass of $O_2$ = 14.9 g

Molar mass of $O_2$ = 32 g/mol

First we have to calculate the moles of $O_2$

$\text{Moles of }O_2=\frac{\text{Given mass }O_2}{\text{Molar mass }O_2}$

$\text{Moles of }O_2=\frac{14.9g}{32g/mol}=0.466mol$

Now we have to calculate the moles of $CO_2$

The balanced chemical equation is:

$2C_4H_{10}+13O_2\rightarrow 10H_2O+8CO_2$

From the reaction, we conclude that

As, 13 mole of $O_2$ react to give 8 moles of $CO_2$

So, 0.466 mole of $O_2$ react to give $\frac{8}{13}\times 0.466=0.287$ mole of $CO_2$

Therefore, the number of moles of $CO_2$ produced are, 0.287 moles.

3 0

3 years ago

I have a sample of galena. It appears there may be some gold in it. It is a piece of raw ore so I took it to a metallurgist and

Lubov Fominskaja [6]

Yes it is possible

Explanation:

Galena and gold can become encrusted together. They can form together in the same geologic setting.

Gold usually occurs freely in nature uncombined with other atoms.
Galena is the largest ore of lead.
Both minerals can become twinned under appropriate geologic conditions.
They are usually seen in pegmatitic intrusions in a rock body as product of late stage melt crystallization.

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Renewable resources brainly.com/question/4344417

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7 0

3 years ago

153 mL of 2.5 M HF is reacted with an excess of Ca(OH)2. How many grams of CaF2 will be produced?

Delvig [45]

Answer:

15 g

Explanation:

Data given:

amount of HF = 153 mL 2.5 M HF

amount of Ca(OH)₂ = Excess

grams of CaF₂ = ?

Reaction Given:

2HF + Ca(OH)₂ ------→ 2H₂O + CaF₂

Solution:

First we have to find number of moles of HF in 153 mL of 2.5 M HF

For this we will use following formula

Molarity = moles of solute / liter of solution

Rearrange above equation

moles of solute = Molarity x liter of solution . . . . . (1)

Put values in above equation (1)

moles of solute = 2.5 x 1 L

moles of solute = 2.5

So,

we come to know that there are 2.5 moles of solute (HF) in 1 L of solution

Now how many moles of solute will be present in 153 ml of solution

Convert 153 mL to Liter

1000 mL = 1 L

153 mL = 153/1000 = 0.153 L

Apply Unity Formula

2.5 moles HF ≅ 1 L solution

X moles of HF ≅ 0.153 L solution

moles of HF = 2.5 moles x 0.153 mL solution / 1 L solution

moles of HF = 0.383 moles

So, 153 mL contains 0.383 moles of HF

Now Look at the reaction:

2HF + Ca(OH)₂ ------→ 2H₂O + CaF₂

2 mol 1 mol

From the reaction we come to know that 2 moles of HF gives 1 mole of CaF₂ then how many moles of CaF₂ will be produced from o.383 moles of HF

Apply Unity Formula

2 moles HF ≅ 1 mole of CaF₂

0.383 moles of HF ≅ X moles of CaF₂

moles of CaF₂ = 0.383 moles x 1 mole / 2 mol

moles of CaF₂ = 0.192 moles

So, 0.192 moles of CaF₂ will be produced by 0.383 moles of HF

Now we will find mass of 0.192 moles of CaF₂

Formula will be used

mass in grams = no. of moles x molar mass . . . . . . . (2)

molar mass of CaF₂ = 40 + 2(19)

molar mass of CaF₂ = 40 + 38 = 78 g/mol

Put values in eq. 2

mass in grams = 0.192 x 78 g/mol

mass in grams = 14.976 g

rounding the value

mass in grams = 15 g

So,153 mL of 2.5 M HF is reacted with an excess of Ca(OH)₂ will produce 15 g of CaF₂.

6 0

4 years ago

A metal oxide reacts chemically with water to form a base in the reaction shown below. If the temperature of the metal oxide and

Alla [95]

increase the rate of chemical change.

Explanation:

The reaction of the metal oxide with water to form a base in the presence of a spike in temperature will lead to an increase in the rate of chemical change.

Temperature change has considerable effect on reaction rates.

Temperature is directly proportional to the average kinetic energy of reacting particles.
Reaction rates varies directly with a spike in temperature.
It has been known that for every 10°C rise in temperature, above the room temperature, reaction rates become double or tripled.
Temperature increases the kinetic energy of each of the reacting particles.
Many of the reacting particles also acquires an energy greater than or equal to the activation energy of the reaction.
The frequency of ordinary collisions and effective collisions per unit time increases.

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Activation energy brainly.com/question/3930233

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6 0

3 years ago