All categories

3 years ago

Which substance cannot be broken down by a chemical change?

Chemistry

2 answers:

san4es73 [151]3 years ago

5 0

Answer:

Zirconium

Explanation:

This is because if you look it up in the periodic table you cannot break it apart by a chemical.

Marta_Voda [28]3 years ago

3 0

<span>Zirconium cannot be broken down by a chemical change, because it is an element. The others are all molecules. Hope ive helped :)</span>

You might be interested in

If the methane contained in 2.50 L of a saturated solution at 25 ∘C was extracted and placed under STP conditions, what volume w

Sunny_sXe [5.5K]

116.6 x $10^{ -3$ } is the volume of methane contained in 2.50 L of a saturated solution at 25 ∘C that was extracted and placed under STP conditions.

<h3>What is an ideal gas equation?</h3>

The ideal gas law (PV = nRT) relates to the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

The solubility of methane in water at 25 degrees Celcius is 1.3 x $10^{ -3}$ M. It implies 1.3 x $10^{ -3}$ moles of methane are dissolved in one litre of water.

The number of moles of methane in 4 L of water can be calculated as follows:

Moles of methane = $\frac{1.3 . 10^{ -3} }{1L}$ x $\frac{4L}{1L}$

Moles of methane = 5.2 x $10^{ -3}$

STP refers to standard temperature and pressure. Under STP conditions, the temperature of the substance is 0 degrees celcius and its pressure is 1 atm.

An ideal gas is an imaginary gas comprising of a large number of randomly moving particles and the motion between such articles is considered to be perfectly elastic. The ideal gas equation describes the relationship between pressure, volume, temperature and number of moles of a gas.

The expression for ideal gas equation is as follows:

PV=nRT, where n is the moles and R is the gas constant. Then divide the given mass by the number of moles to get molar mass.

Given data:

P= 1 atm

V= ?

R= $0.082057338 \;L \;atm \;K^{-1}mol^{-1}$

T=273K

n=?

Putting value in the given equation:

$\frac{PV}{RT}=n$

5.2 x $10^{ -3} = \frac{1 \;atm\; X \;V}{0.082057338 \;L \;atm \;K^{-1}mol^{-1} X 273}$

V= 116.6 x $10^{ -3}$

Hence, 116.6 x $10^{ -3$ } is the volume of methane contained in 2.50 L of a saturated solution at 25 ∘C was extracted and placed under STP conditions.

Learn more about the ideal gas here:

brainly.com/question/27691721

#SPJ1

4 0

3 years ago

Which two locations are MOST probable for locating the cloud of electrons?

rjkz [21]

On the edges or the outer magnetic fields

4 0

4 years ago

Read 2 more answers

Imagine two solutions with the same concentration and the same boiling point, but one has benzene as the solvent and the other h

11Alexandr11 [23.1K]

Complete question:

Imagine two solutions with the same concentration and the same boiling point, but one has benzene as the solvent and the other has carbon tetrachloride as the solvent. Determine that molal concentration, m (or b), and boiling point, Tb.

benzene boiling point=80.1 Kb=2.53

carbon tetrachloride boiling point=76.8 Kb=5.03

Answer:

m = 1.32 mol/kg

Boiling point: 83.4°C

Explanation:

When a nonvolatile solute is added to a pure solvent, the boiling point of the solvent increases, a phenomenon called ebullioscopy. This happens because of the interactions between the solute and the solvent. The temperature variation (new boiling point - normal boiling point) can be calculated by:

ΔT = m*Kb*i

Where m is the molal concentration (moles o solute/mass of solvent in kg), Kb is the ebullioscopy constant of the solvent, and i is the van't Hoff factor, which indicates how much of the solute dissociates. Let's assume that i is equal in both solvents and equal to 1 (the solvent dissociates completely)

Calling the new boiling point as Tb, for benzene:

Tb - 80.1 = m*2.53*1

Tb = 2.53m + 80.1

For carbon tetrachloride:

Tb - 76.8 = m*5.03*1

Tb = 5.03m + 76.8

Because Tb and m are equal for both:

5.03m + 76.8 = 2.53m + 80.1

2.5m = 3.3

m = 1.32 mol/kg

So, substituting m in any of the equations (choosing the first):

Tb = 2.53 * 1.32 + 80.1

Tb = 83.4°C

3 0

4 years ago

Read 2 more answers

True and False: Atoms combine in different ways to make up all the substances you encounter every day

marissa [1.9K]

True! Everything in the whole wide world is made up of matter, and the 3 types of matter are all made from atoms!!!

Even you made up of atoms :)

3 0

3 years ago

Read 2 more answers

A mixture of 0.2000 mol of CO2, 0.1000 mol of H2 and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium

Slav-nsk [51]

Answer:

a) p(CO2) = 4.103 atm

p(H2) = 2.0515 atm

p(H2O) = 3.2824 atm

b) pCO2 = 3.8754 atm

pH2 = 1.8239 atm

pCO = 0.2276 atm

pH2O = 3.51 atm

c) Kp= 0.113

Explanation:

Step 1: Data given

Moles of CO2 = 0.2000 mol

Moles of H2 = 0.1000 mol

Moles of H2O = 0.1600 mol

Volume = 2.000 L

Temperature = 500 k

Step 2: The balanced equation

CO2 (g) + H2 (g) → CO (g) + H2O (g)

Step 3: Calculate the initial partial pressures of CO2, H2, and H2O.

pV = nRT

P = (nRT)/V

p(CO2) = (0.2000 mol * 0.08206 * 500)/2.000L

⇒ p(CO2) = 4.103 atm

p(H2) = (0.1000 mol * 0.08206 * 500)/2.000L

⇒ p(H2) = 2.0515 atm

p(H2O) = (0.1600 mol * 0.08206 * 500)/2.000L

⇒ p(H2O) = 3.2824 atm

b. At equilibrium PH2O= 3.51 atm. Calculate the equilibrium partial pressures of CO2, H2, and CO.

Step 1: Calculate the change in pH2O

The change in pH2O = 3.51 - 3.2824 = 0.2276

Step 2: the initial pressures

pCO2 = 4.103 atm

pH2 = 2.0515 atm

pCO = 0 atm

pH2O = 3.2824

Step 3: The partial pressure at the equilibrium

Since there reacts 0.2276 atm for H2O, and the mol ratio is 1:1:1:1

For each gas, there will react 0.2276 atm

pCO2 = 4.103 - 0.2276 = 3.8754 atm

pH2 = 2.0515 - 0.2276 = 1.8239 atm

pCO = 0 + 0.2276 = 0.2276 atm

pH2O = 3.51 atm

c. Calculate Kp for this reaction

Kp = (pCO * pH2O)/ (pCO2 * pH2)

Kp = (0.2276 * 3.51) /( 3.8754 *1.8239)

Kp = 0.113

5 0

3 years ago