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3 years ago

Mole fraction of the solute in a 1.00. What is the molal aqueous eqaution?

1 answer:

6 0

Mole fraction is expressed as the number of moles of solute over the total number of moles of solute and the number of moles of solvent. When expressed in molal, this is equal to number of moles of solute per liter solvent. If the mole fraction is 1.00, this means, all that is in the solution is solute. Hence the molal equivalent is 1.00 too

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How many atoms are in 9.35 moles of lithium?

Fudgin [204]

Answer:

3.45 moles Li contains 2.08 × 10 (to the power of)24 atoms .

Explanation:

The relationship between atoms and moles is:

1 mole atoms =

6.022 × 10 (to the power of)23

atoms

In order to determine how many atoms occupy a given number of moles, multiply the given moles by

6.022 × 10 (to the power of)23

atoms/mole

In the case of 3.45 moles lithium (Li):

3.45 mol Li × 6.022 × 10 (to the power of)23 atoms Li/ 1 mol Li =

2.08 × 10 (to the power of)24

atoms Li rounded to three

6 0

3 years ago

pH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: pH=−log[H+] Due to the autoioniz

Sophie [7]

Answer:

pH = 2,4

Explanation:

pH is defined as a measure of acidity or alkalinity of a solution based on H⁺ concentration

The HCl dissociates in water thus:

HCl → H⁺ + Cl⁻

That means that moles of HCl are the same than H⁺.

0,35gHCl $\frac{1mol}{36,46g}$ = 9,6x10⁻³ moles HCl ≡ moles H⁺

H⁺ molarity is: $\frac{9,6x10^{-3}moles}{2,5L}$ = 3,84x10⁻³M

As pH = -log [H⁺]

I hope it helps!

7 0

3 years ago

How many cm3 are contained in 3.83 x 107 mm3?

gulaghasi [49]

Answer:

3.38 x 10⁴cm³

Explanation:

Given that:

Volume of the substance = 3.83 x 10⁷mm³

The problem entails use to convert from mm³ to cm³;

1000mm³ = 1cm³

So;

3.83 x 10⁷mm³ will produce $\frac{ 3.83 x 10^{7} }{1000}$ = 3.38 x 10⁴cm³

5 0

3 years ago

What is the volume of 0.80 grams of o2 gas at stp? (5 points) group of answer choices 0.59 liters 0.56 liters 0.50 liters 0.47 l

Vladimir [108]

Answer:

0.56L

Explanation:

This question requires the Ideal Gas Law: $PV=nRT$ where P is the pressure of the gas, V is the volume of the gas, n is the number of moles of the gas, R is the Ideal Gas constant, and T is the Temperature of the gas.

Since all of the answer choices are given in units of Liters, it will be convenient to use a value for R that contains "Liters" in its units: $R=0.0821\frac{L\cdot atm}{mol\cdot K}$

Since the conditions are stated to be STP, we must remember that STP is Standard Temperature Pressure, which means $T=273.15K$ and $P=1atm$

Lastly, we must calculate the number of moles of $O_2(g)$ there are. Given 0.80g of $O_2(g)$ , we will need to convert with the molar mass of $O_2(g)$ . Noting that there are 2 oxygen atoms, we find the atomic mass of O from the periodic table (16g/mol) and multiply by 2: $32g\text{ }O_2=1mol\text{ }O_2$