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lubasha [3.4K]
3 years ago
11

HELP ASAP ITS TIMED!!!

Chemistry
2 answers:
Tpy6a [65]3 years ago
5 0

Answer:

C would be the right answer

IgorLugansk [536]3 years ago
3 0

Answer:

B

Explanation:

I have a similar question and it was correct try B

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hram777 [196]
I think it’s false : D
4 0
3 years ago
Based on the chemical equation, use the drop-down menu to choose the coefficients that will balance the chemical equation:
Elan Coil [88]

Answer:

3

2

Explanation:

3O2 => 2O3

the equation is balancing

6 0
3 years ago
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A force of 99 N causes a box to accelerate at a rate of 11 m/s2. What is the mass of the box? (Ignore frictional effects.)
wlad13 [49]
F =  ma

<span>m = F/a = 99/11 = 9 kg</span>
3 0
3 years ago
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If 16.0 grams of aluminum oxide were actually produced, what is the percent yield of the reaction below given that you start wit
Svetllana [295]

Answer: The percent of yield is 50.03%.

Explanation:

First, we need to balance the equation:

4Al + 3O_{2} ⇒ 2Al_{2}O_{3}

We need to remember that the chemical equations are written in moles, so we have to convert the amounts in grams to moles, using the molecular weight of every compound: Al2O3 (101.96 g/mol), Al (29.98 g/mol) and O2 (31.99 g/mol).

In consequence, the amounts in moles of every compound will be:

16 gAl_{2}O_{3} * \frac{1 mol}{101.96 g} =0.157 mol Al_{2}O_{3}

10 g Al * \frac{1mol}{29.98 g}= 0.333 mol Al

19 g O_{2}*\frac{1 mol}{31.99 g} =0.594 mol O_{2}

Now, we have to find out which is the limit reagent or in other words, which of the reagents will be consumed first, taking into account the stoichiometric ratio of the balanced equation:

0.333 mol Al * \frac{2 mol Al_{2}O_{3}}{4 mol Al} =0.1665 mol Al_{2}O_{3}

0.594 mol O_{2} * \frac{2 mol Al_{2}O_{3}}{3 mol O_{2}} =0.396 mol Al_{2}O_{3}

As you can see, the maximum amount (theoretically) of Al2O3 that can be produced is 0.1665 mol.

Finally, we have to use the yield formula to calculate the percent yield of the reaction:

Percent of yield = \frac{actual yield}{theoretical yield} * 100 = \frac{0.157 mol Al_{2}O_{3}}{0.1665 mol Al_{2}O_{3}} * 100 = 94.25

Therefore, the percent of yield is 50.03%.

4 0
3 years ago
A spherical sample has a mass of 2.813 g it has a diameter of 8.0 mm what is the sphere made of
Hoochie [10]

The sphere is probably made of silver.

<em>V</em> = ⁴/₃π<em>r</em>^3 = ⁴/₃π(0.40 cm)^3 = 0.268 cm^3

<em>D</em> = <em>m</em>/<em>V</em> = 2.813 g/0.268 cm^3 = 10.5 g/cm^3

The density of silver is 10.5 g/cm^3.

8 0
3 years ago
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