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2 years ago

Which conversion factor would you use to correctly calculate the number of moles in 25.0 g of the element titanium (ti) ?

1 answer:

4 0

To convert grams to moles, you need molar mass.

according to the periodic table, the molar mass of 47.88 g/mol. answer is C

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a student adds 3.5 moles of solute to enough water to make a 1500mL solution. what is the concentration?

aksik [14]

<h2>Hello!</h2>

The answer is:

$MolarConcentration=\frac{3.5moles}{volume(1.5L)}=2.33molar$

Since there is not information about the solute but only its mass, we need to assume that we are calculating the molar concentration of a solution or molarity. So, need to use the following formula:

$MolarConcentration=\frac{mass(solute)}{volume(solution)}$

Now, we know that the mass of the solute is equal 3.5 moles and the volume is equal to 1500 mL or 1.5L

Then, substituting into the equation, we have:

$MolarConcentration=\frac{3.5moles}{1.5L}=2.33molar$

Have a nice day!

7 0

2 years ago

Read 2 more answers

Bobby's mom sets a small pot of water on the stove and lights the burner. Ten minutes later, Bobby notices small bubbles and see

dolphi86 [110]

There are no answers, list them so I can answer.

7 0

2 years ago

Read 2 more answers

Butyl butyrate is an ester that is a naturally occurring oil used in the flavor industry for its fruity scent. If the steam dist

Snezhnost [94]

Answer:

The correct answer is 62.5 %.

Explanation:

Based on the given information, the partial pressure of butyl butyrate is 50 mmHg and the partial pressure of water is 710 mmHg.

Hence, the total pressure is 710+50 = 760 mmHg

According to Dalton's law of partial pressure,

Partial pressure = mole fraction * total pressure

Mole fraction of water is,

Partial pressure of water/Total pressure = 710/760 = 0.93

Similarly, the mole fraction of butyl butyrate is,

Partial pressure of butyl-butyrate/Total pressure = 50/760 = 0.07

Therefore, mole% of water is 0.93 * 100 = 93 %

For calculating mass%,

Mass of H2O = 0.93 * 18 = 16.8 grams (The molecular mass of water is 18 grams per mole)

The molecular mass of butyl-butyrate is 144 gram per mole

The mass of butyl-butyrate = 144 * 0.07 = 10.08 grams

The mass percent of water will be,

Mass % of water/Total mass % * 100 = 16.8 / 10.08 + 16.8 * 100 = 62.5%.

8 0

2 years ago

For a single component system, why do the allotropes stable at high temperatures have higher enthalpies than allotropes stable a

solniwko [45]

Answer:

The difference in the magnetic orientation influences the thermal stability of the allotropes of iron.

Explanation:

It is known that the allotropes of iron exist in three phases: α - phase, β- phase, and γ-phase. However, two prominent structures are the α - phase and γ-phase. Now, let us look at the two phrases:

α - phase

This structure is a body-centered cube. It means that the unit cell structure resembles a cube. The lattice points are in the face of the cube. This subsequently affects the magnetic structure of the iron allotrope.

γ-phase

This allotrope has a lattice structure. It simply means that the structure has lattice points on the face of the cube. The structure generally affects the magnetic properties of the transitional metal; hence the stability of the γ-phase compared to α-phase.

8 0

2 years ago

In the equilibrium system described by: PO43-(aq) + H2O(1) = HPO42-(aq) + OH-(aq) Brønsted-Lowry theory would designate: A) PO43

Kamila [148]

Answer:

The correct option is: B) H₂0 and OH⁻ as a conjugate pair

Explanation:

According to Brønsted-Lowry theory, the<u> </u><u>acids</u><u> are the chemical substances that form a conjugate base by donating a proton</u> and <u>bases</u><u> are the chemical substances that form conjugate acid by accepting a proton.</u>

In the given chemical reaction: PO₄³⁻(aq) + H₂O(l) ⇄ HPO₄²⁻(aq) + OH⁻(aq)

<u>According to Brønsted-Lowry theory, PO₄³⁻ and OH⁻ are bases. Whereas, H₂O and HPO₄²⁻ are acids.</u>

<u>Also, PO₄³⁻ and HPO₄²⁻ are the conjugate acid-base pair; and H₂O and OH⁻ are the conjugate acid-base pair.</u>

6 0

2 years ago