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wolverine [178]
2 years ago
11

4.5 × 1025 atoms of nickel equal how many moles? A. 27 mol B. 2.7 × 1048 mol C. 0.75 mol D. 75 mol

Chemistry
2 answers:
crimeas [40]2 years ago
7 0

Answer:

75 mol

Explanation:

The number of atoms in a mole of substance is 6.023X10²³ [Avagadro's number]

if the given sample of nickel contains 4.5X10²⁵ atoms it means the moles are

moles = \frac{numberofatoms}{Avagadro'snumber}

moles = \frac{4.5X10^{25}}{6.023X^{23}}=74.71mol

If we round of the given answer the number of moles = 75 moles

Molodets [167]2 years ago
4 0
It's 75
PS use ^ to mean to the power of
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Answer:

Dilute

Explanation:

A concentrated solutions is a one which has relatively large amount of dissolved solute in the solution whereas a dilute solution is a one which has relatively lower concentration of dissolved solute.

In the given solution there is only 3.3% of solute. So, we can say that the given solution is a dilute solution. However, these terms are relative.

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How many grams in 6.20 x 10^25 atoms of bromine (Br) ? image attached , will give brainliest
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Answer:

8239.2g

Explanation:

Given parameters:

Number of atoms in Br  = 6.2 x 10²⁵atoms

Unknown:

Mass of Br = ?

Solution:

From mole concepts, we know that:

       1 mole of a substance contains 6.02 x 10²³ atoms/mol

 Molar mass of Br  = 80g/mol

6.2 x 10²⁵atoms  x \frac{1}{6.02 x 10^{23} } \frac{mol}{atoms} x  80 x \frac{g}{moles}  

          = 8239.2g

8 0
3 years ago
What is the mass of a piece of iron if its density is 1.98 g/mL and its volume is 2.45 mL?
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Answer:

4.858 g

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Start with the formula

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volume = 2.45 mL

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rearrange the formula to solve for mass

(density) x (volume) = mass

Add in the substitutes and solve for mass

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3 0
3 years ago
How do you find the # of sigma and pi bonds using a Lewis dot structure
Lubov Fominskaja [6]

Every single bond is a sigma bond.

A double bond contains 1 sigma bond and 1 pi bond.

A triple bond contains 1 sigma bond and 2 pi bonds.


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3 years ago
Phosgene, COCl2, gained notoriety as a chemical weapon in World War I. Phosgene is produced by the reaction of carbon monoxide w
jek_recluse [69]

The question is incomplete, here is the complete question:

Phosgene, COCl_2, gained notoriety as a chemical weapon in World War I. Phosgene is produced by the reaction of carbon monoxide with chlorine:  

CO(g)+Cl_2(g)\rightleftharpoons COCl_2(g)

The value of K_c for this reaction is 5.79 at 570 K. What are the equilibrium partial pressures of the three gases if a reaction vessel initially contains a mixture of the reactants in which p_{CO}=p_{Cl_2}=0.265atm and p_{COCl_2}=0.000atm ?

<u>Answer:</u> The equilibrium partial pressure of CO, Cl_2\text{ and }COCl_2 is 0.257 atm, 0.257 atm and 0.008 atm respectively.

<u>Explanation:</u>

The relation of K_c\text{ and }K_p is given by:

K_p=K_c(RT)^{\Delta n_g}

K_p = Equilibrium constant in terms of partial pressure

K_c = Equilibrium constant in terms of concentration = 5.79

\Delta n_g = Difference between gaseous moles on product side and reactant side = n_{g,p}-n_{g,r}=1-2=-1

R = Gas constant = 0.0821\text{ L. atm }mol^{-1}K^{-1}

T = Temperature = 570 K

Putting values in above equation, we get:

K_p=5.79\times (0.0821\times 570)^{-1}\\\\K_p=0.124

We are given:

Initial partial pressure of CO = 0.265 atm

Initial partial pressure of chlorine gas = 0.265 atm

Initial partial pressure of phosgene = 0.00 atm

The given chemical equation follows:

                      CO(g)+Cl_2(g)\rightleftharpoons COCl_2(g)

<u>Initial:</u>            0.265      0.265

<u>At eqllm:</u>        0.265-x    0.265-x        x

The expression of K_p for above equation follows:

K_p=\frac{p_{COCl_2}}{p_{CO}\times p_{Cl_2}}

Putting values in above equation, we get:

0.124=\frac{x}{(0.265-x)\times (0.265-x)}\\\\x=0.0082,8.59

Neglecting the value of x = 8.59 because equilibrium partial pressure cannot be greater than initial pressure

So, the equilibrium partial pressure of CO = (0.265-x)=(0.265-0.008)=0.257atm

The equilibrium partial pressure of Cl_2=(0.265-x)=(0.265-0.008)=0.257atm

The equilibrium partial pressure of COCl_2=x=0.008atm

Hence, the equilibrium partial pressure of CO, Cl_2\text{ and }COCl_2 is 0.257 atm, 0.257 atm and 0.008 atm respectively.

6 0
3 years ago
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