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MatroZZZ [7]
3 years ago
6

What is the number of moles of beryllium in 36 g of Be?

Chemistry
2 answers:
GarryVolchara [31]3 years ago
3 0
4 moles i believe cos mole = mass/ molar mass
mole =36/9
=4

g100num [7]3 years ago
3 0
First, as a unit of quantity = 6.02 x 1023 objects .

<span>Calculate the moles of Be by dividing 36/9.0 = 4.0 moles</span>
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An environmental scientist developed a new analytical method for the determination of cadmium (cd^2+) in mussels. To validate th
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Answer:

The method is accurate  in the calculation of the Cu^+2

Explanation:

As a first step we have to calculate the <u>average concentration </u>of Cu^+2 find it by the method.

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lower limit: 0.75

If we compare the limits of the value obtanied by the method (Figure 1 Red line) with the reference material (Figure 1 blue line) we can see that the values obtained by the method are within the values suggested by the reference material. So, it's method is accurate.

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Read 2 more answers
Propane (C3H8) can be burned to produce heat for homes. The products of the reaction are CO2 and H2O. For complete combustion to
Natalija [7]

Answer:

1- 3 Moles of CO2  

2- 132 g of CO2  

3- 105,6 g of CO2

4- Limiting Reagent O2

<u>Products form based on limiting reagent (384g O2) :</u>

CO2: 316,8 g

H2O: 172,8 g

<u>Products form based on C3H8 (132,33 g):</u>

CO2: 396,99 g

H2O: 216,54 g  

Explanation:

<u>Atomic Masses:</u>

C: 12

H: 1

O: 16

<u>Molecular weights:</u>

C3H8: 44 g

O2: 32 g

H2O: 18 g

CO2: 44 g

C3H8 + 5 O2⇒ 3 CO2 + 4 H2O

C3H8 (44g)+ O2 (160 g) ⇒ CO2 (132 g) + H2O (72 g)

In 5 moles of O2 are produced 3 moles of CO2, equivalent to 132 g

For 160g of O2 are produced 132 g of CO2, so 128 g of O2

160 g  O2 ⇒ 132 g CO2

128 g  O2⇒ × = 105,6 g CO2

(128×132÷160= 105,6)

The limiting reagent is the substance that is totally consumed when the chemical reaction is complete. The amount of product formed is limited by this reagent, because the reaction cannot continue without it.

If I have 132,33 g of C3H8 and 384 g O2 we can calculate:

For          44 g of CH3H8  ⇒160 g of O2

With   132,33 g of CH3H8 ⇒ ×= 481,2 g of O2

(132,33×160÷44=481,2)

As this amount exceeds the quantity of O2 that we have, we can assume that the 384 g O2 will be totally consumed.

<u>Calculations of the products formed in base of quantity of O2 (limiting reagent):</u>

160 g  O2 ⇒ 132 g CO2

384 g  O2⇒ × = 316,8 g CO2

(384×132÷160= 316,8)

160 g  O2 ⇒ 72 g H2O

384 g  O2⇒ × = 172,8 g H2O

(384×72÷160= 172,8)

<u>Calculations of the products formed in base of quantity of C3H8 (excess reagent):</u>

     44 g  C3H8 ⇒ 132 g CO2

132,33 g  C3H8 ⇒ × = 396,99 g CO2

(132,33×132÷44=396,99)

     44 g C3H8 ⇒ 72 g H2O

132,33 g  C3H8⇒ × = 216,54 g H2O

(132,33×72÷44= 216,54)

<u />

3 0
3 years ago
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