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Studentka2010 [4]
3 years ago
15

What problems might happen if an unnecessary hurricane warning was issues

Chemistry
1 answer:
deff fn [24]3 years ago
4 0
People would rush to the store to buy supplies and there might not be enough for the "last minute noticed" people
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An aluminum can (Al) has a mass of 15.8 grams. How many atoms of aluminum are in the can?
Naddik [55]

Answer:

i think this is the answer you can try it tho...

Explanation:

Notice that the value 12.01 grams of natural carbon is the same as the atomic mass value (12.01 amu). It also tells us that 26.98 grams of aluminum contains exactly 6.022 x 1023 atoms of aluminum.

5 0
2 years ago
Which one is not acid? Na₂O or CO₂
vodka [1.7K]

Answer:

It is Na2O because it doesn't show any acidic properties.

4 0
2 years ago
Three Stoichiometry Questions
andrezito [222]

Answer:

Explanation:

7)

Given data:

Mass of aluminium = 2.5 g

Mass of oxygen = 2.5 g

Mass of aluminium oxide = 3.5 g

Percent yield = ?

Solution:

Chemical equation:

4Al + 3O₂   →   2Al₂O₃

Number of moles of Al:

Number of moles = mass/ molar mass

Number of moles = 2.5 g/ 27 g/mol

Number of moles = 0.09 mol

Number of moles of oxygen:

Number of moles = mass/ molar mass

Number of moles = 2.5 g/ 32 g/mol

Number of moles = 0.08 mol

Now we will compare the moles of aluminium oxide with aluminium and oxygen.

                          Al         ;       Al₂O₃

                           4         :        2

                        0.09      :       2/4×0.09 = 0.045

                          O₂       :        Al₂O₃

                          3         :          2

                         0.08    :        2/3 ×0.08 = 0.053

The number of moles of aluminium oxide produced by Al are less so it will limiting reactant.

Mass of aluminium oxide:

Mass = number of moles × molar mass

Mass = 0.045  × 101.96 g/mol

Mass = 4.6 g

Percent yield:

Percent yield = actual yield / theoretical yield ×100

Percent yield = 3.5 g / 4.6 ×100

Percent yield = 76.1%

8)

Given data:

Mass of copper produced = 3.47 g

Mass of aluminium = 1.87 g

Percent yield = ?

Solution:

Chemical equation:

2Al + 3CuSO₄   →   Al₂(SO₄)₃ + 3Cu

Number of moles of Al:

Number of moles = mass/ molar mass

Number of moles = 1.87 g/ 27 g/mol

Number of moles = 0.07 mol

Now we will compare the moles of copper with aluminium.

                          Al         ;       Cu

                           2         :        3

                        0.07      :       3/2×0.09 = 0.105

             

Mass of copper:

Mass = number of moles × molar mass

Mass = 0.105  × 63.55 g/mol

Mass = 6.67 g

Percent yield:

Percent yield = actual yield / theoretical yield ×100

Percent yield =  3.47 g / 6.67 × 100

Percent yield = 52%

                       

4 0
3 years ago
A 118.0 g sample of a compound contains 72.0 g of C , 18.0 g of H and 28.0 g of N. Which of the following is the empirical formu
andrew11 [14]

Explanation:

Empirical formula = C6H18N2

5 0
3 years ago
How many joules of energy are necessary to heat a sample of water with a mass of 46.0 grams from 0.0 to 100.0
Luba_88 [7]

Answer:

Q = 19255.6 j

Explanation:

Specific heat capacity:

It is the amount of heat required to raise the temperature of one gram of substance by one degree.

Formula:

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

Given data:

Mass of water = 46 g

change in temperature = ΔT = 100-0.0 = 100 °C

Heat absorbed by water = ?

Solution:

Specific heat capacity of water = 4.186 j/g. °C

Q = m.c. ΔT

Q = 46 g×4.186 j/g. °C×100 °C

Q = 19255.6 j

3 0
3 years ago
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