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2 years ago

What is the mass in grams of the following measurements? 1.00 mol Al _ 6.02 x 10 23atoms Al _

Chemistry

1 answer:

omeli [17]2 years ago

6 0

Answer:

Mass of 1 mole of Aluminium = Mass of 6.02 x 10 23atoms of Aluminium = 26.98 grams.

Explanation:

1 mole of any element or molecule has 6.02 x 10 23atoms or subparts.

Hence 1 mole of aluminum will also have 6.02 x 10 23atoms. Hence, it is clear that mass of 1 mole of Aluminium will be equal to 6.02 x 10 23atoms of Aluminium.

Thus,

Mass of 1 mole of Aluminium = Mass of 6.02 x 10 23atoms of Aluminium = 26.98 grams.

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How many moles are there in 3.612 x 1024 formula units of Na2SO4?

vitfil [10]

Answer:

<h3>Theanswer is 6 moles</h3>

Explanation:

To find the number of moles in a substance given it's number of entities we use the formula

$n = \frac{N}{L} \\$

where n is the number of moles

N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

From the question we have

$n = \frac{3.612 \times {10}^{24} }{6.02 \times {10}^{23} } \\$

We have the final answer as

<h3>6 moles</h3>

Hope this helps you

5 0

2 years ago

I NEED HELPPPP

Vinil7 [7]

Answer:

3 Handsprings

Explanation:

18 divided by 6 is 3

3 0

2 years ago

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way:

LiRa [457]

Explanation:

(a) As the given chemical reaction equation is as follows.

$OCl^{-} + I^{-} \rightarrow OI^{-1} + Cl^{-1}$

So, when we double the amount of hypochlorite or iodine then the rate of the reaction will also get double. And, this reaction is "first order" with respect to hypochlorite and iodine.

Hence, equation for rate law of reaction will be as follows.

Rate = $K \times [OCl^{-}] \times [l^{-}]$

(b) Since, the rate equation is as follows.

Rate = $K [OCl^{-}][l^{-}]$

Let us assume that ( $[OCl^{-}] = [l^{-}]$ )

Putting the given values into the above equation as follows.

$1.36 \times 10^{-4} = K \times (1.5 \times 10^{-3})^2$

$1.36 \times 10^{-4} = K \times (2.25 \times 10^{-6})$

K = $\frac{1.36 \times 10^{-4}}{2.25 \times 10^{-6}}$

= $60.4 M^{-1}sec^{-1}$

Hence, the value of rate constant for the given reaction is $60.4 M^{-1}sec^{-1}$ .

(c) Now, we will calculate the rate as follows.

Rate = $K [OCl^{-}][l^{-}]$

= $60.4 \times (1.8 \times 10^{3}) \times (6.0 \times 10^{4})$

= $6.52 \times 10^{5}$

Therefore, rate when $[OCl^{-}] = 1.8 \times 10^{3}$ M and $[I^{-}]= 6.0 \times 10^{4}$ M is $6.52 \times 10^{5}$ .

8 0

2 years ago

Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) 2H2(g) CH3OH(g) . A reaction vessel contains the th

mihalych1998 [28]

Answer:

The answer is C. The partial pressure of hydrogen will be unchanged.

Explanation:

$CO_{(g)} + 2H_{2(g)}$ ⇒ $CH_{3}OH$

Argon with electronic configuration $1s^{2}$ $2s^{2}$ $2p^{6}$ $3s^{2}$ $3p^{6}$ (that is atomic number 18) is an inert gas making it unreactive and it's addition to the reaction has no effect on the partial pressure of either the reactant or production or the state of the system.

The partial pressure of hydrogen will remain unchanged on the addition of Argon.

6 0

2 years ago

A chemist wants to produce 12.00 grams of barium sulfate by reacting a .6000 M BaCl2 solution with excess H2SO as show in the re

worty [1.4K]

Find the moles of BaSO4 first. Then since we know it's a one to one ratio from barium chloride to barium sulfate we can just solve for liters.
<span>First you need to find the moles BaSO4 , and the you will require to find barium sulfate in liters.

</span>12.00gBaSO4 / 233.31 grams per mole

=.05141moles

Molarity=moles/liters

Hence,

Liters=.05141moles/.6Molarity
=.85 liters

7 0

2 years ago

Read 2 more answers

What is the mass in grams of the following measurements? 1.00 mol Al ___________ 6.02 x 10 23atoms Al ___________

What is the mass in grams of the following measurements? 1.00 mol Al _ 6.02 x 10 23atoms Al _