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3 years ago

Each of the following models represents particles present before and after a

Chemistry

1 answer:

lana [24]3 years ago

5 0

Answer:

Explanation:

According to the law of conservation of mass, matter can neither be created nor destroyed. The implication of this is that the total mass of reactants should be equal to the total mass of products.

There should be equal masses of reactants and products on both sides of the reaction equation. This most important condition is only satisfied by option D.

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A strong acid is one that

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Answer:

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3 years ago

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Unit 1- Unit Assessment (Matter & Density)

konstantin123 [22]

Answer:

<h3>The answer is 11 g/mL</h3>

Explanation:

The density of a substance can be found by using the formula

$density = \frac{mass}{volume} \\$

From the question

mass = 3025 g

volume = 275 mL

We have

$density = \frac{3025}{275} \\$

We have the final answer as

Hope this helps you

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3 years ago

Why do non-metal aroms form covalent bonds e.g. H2O

Oksana_A [137]

Answer:

Covalent bonds usually occur between nonmetals. For example, in water (H2O) each hydrogen (H) and oxygen (O) share a pair of electrons to make a molecule of two hydrogen atoms single bonded to a single oxygen atom. ... Covalent compounds tend to be soft, and have relatively low melting and boiling points.

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3 years ago

Which aqueous solution will have the highest boiling point temperature? A. 0.100 molal NiBr2(aq) B. 0.250 molal CH3OH(aq) C. 0.1

zaharov [31]

Answer: 0.150 m $Na_2SO_4(aq)$ will have highest boiling point.

Explanation:

Formula used for Elevation in boiling point :

$\Delta T_b=i\times k_b\times m$

where

$\Delta T_b=T_b-T^o_b$ = elevation in boiling point

[tex[k_b[/tex] = boiling point constant

m = molality

i = Van't Hoff factor

A) 0.100 m $NiBr_2$

i = 3 as $NiBr_2\rightarrrow Ni^{2+}+2Br^-$

concentration will be $3\times 0.100=0.300$

B) 0.250 m $CH_3OH$

i = 1 as $CH_3OH$ is a non electrolyte

concentration will be $1\times 0.250=0.250$

C) 0.100 molal $MgSO_4(aq)$

i = 2 as $MgSO_4\rightarrrow Mg^{2+}+SO_4^{2-}$

concentration will be $2\times 0.100=0.200$

D. 0.150 molal $Na_2SO_4(aq)$

i = 3 as $Na_2SO_4\rightarrrow 2Na^{+}+SO_4^{2-}$

concentration will be $3\times 0.150=0.450$

E. 0.150 molal $NH_4NO_3(aq)$

i = 2 as $NH_4NO_3\rightarrrow NH_4^{+}+NO_3^{-}$

concentration will be $2\times 0.150=0.300$

The solution having the highest concentration of ions will have the highest boiling point and thus 0.150 m $Na_2SO_4(aq)$ will have highest boiling point.

8 0

3 years ago

Please show all of your work! :)

allsm [11]

Answer:

Explanation:

The problem says that carbon dioxide was collected at 740.4 mmHg, but this is a pressure that includes the pressure of the water. We want to only use the pressure of the carbon dioxide, so subtract the pressure of the water (21.0 mmHg) from 740.4 mmHg:

740.4 - 21.0 = 719.4 mmHg

Now, we can use the ideal gas law to find the number of moles of carbon dioxide we have: PV = nRT.

- the pressure P is 719.4 mmHg

- the volume V is 38.82 mL, but we need Litres, so divide 38.82 by 1000: 38.82 / 1000 = 0.03882 L

- the moles n is what we want to find

- the gas constant R is 62.36 L mmHg / (mol K)

- the temperature T is 23.0°C, but we need this in Kelvins, so add 273 to 23.0: 23.0 + 273 = 296 K

Plug all these in:

PV = nRT

(719.4 mmHg) * (0.03882 L) = n * (62.36) * (296 K)

n ≈ 0.00151 mol $CO_2$

Note that this is moles of carbon dioxide, but since we want CaCO3, we need to convert moles using the reaction. It's just a 1 to 1 ratio, so we still have 0.00151 moles of CaCO3. Now, convert moles to grams. The molar mass of CaCO3 is 40.08 + 12.01 + 3 * 16 = 100.09 g/mol.

$0.00151 molCaCO_3*\frac{100.09g}{1mol} =0.151gCaCO_3$

To find the mass percent, divide 0.151 by the total mass of the tablet, which is 0.3211 g:

0.151 g / 0.3211 g = 0.471 = 47.1%

The answer is D.

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3 years ago

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