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kirill115 [55]
3 years ago
12

Please helpppppppp helpppppppppppppppppppppppppppp

Chemistry
1 answer:
trasher [3.6K]3 years ago
3 0
Protons are positive
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According to the reaction below, what mass of oxygen gas is required to produce 22 g of carbon dioxide?
alisha [4.7K]
The answer is B)4.0g
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Which elements did the Curies discover?
Scilla [17]

Answer:

B on edge

Explanation:

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2 years ago
How many grams of iki would it take to obtain a 100 ml solution of 0.300 m iki? how many grams of iki would it take to create a
GalinKa [24]

0.300 M IKI represents the concentration which is in molarity of a potassium iodide solution. This means that for every liter of solution there are 0.300 moles of potassium iodide. Knowing that molarity is a ratio of solute to solution.

By using a conversion factor:

100 ml x (1L / 1000 mL) x (0.300 mol Kl / 1 L) x (166.0g / 1 mol Kl) = 4.98 g

Therefore, in the first conversion by simply converting the unit of volume to liter, Molarity is in L where the volume is in liters. The next step is converted in moles from volume by using molarity as a conversion factor which is similar to how density can be used to convert between volume and mass. After converting to moles it is simply used as molar mass of Kl which is obtained from periodic table to convert from mole to grams.

In order to get the grams of IKI to create a 100 mL solution of 0.600 M IKI, use the same formula as above:

100 ml x (1L / 1000 mL) x (0.600 mol Kl / 1 L) x (166.0g / 1 mol Kl) = 9.96 g

3 0
3 years ago
Which substance has a chemical formula with the same ratio of metal ions to nonmetal ions as in potassium sulfide?
pav-90 [236]
Answer=1

Potassium Sulfide= K2S (two metals, one non metal)


Sodium Oxide=Na2O (two metals. one nonmetal)

Sodium Chloride=NaCl (one metal, one nonmetal)

Magnesium Oxide=MgO (one metal, one nonmetal)

Magnesium Chloride=MgCl2 (one metal, two nonmetals)
6 0
3 years ago
Read 2 more answers
William measures a test tube and finds that the mass of the test tube is 5g. He places the lone reactant in the test tube and fi
iogann1982 [59]

86 percent is the percent yield for this experiment if he expected to produce 5g of product.

Explanation:

Given that:

mass of test tube = 5 grams

mass of test tube + reactant is 12.5 grams

mass of reactant = ( mass of test tube + reactant ) - (mass of test tube)

mass of reactant = 12.5 -5

                             = 7.5 grams

when 7.5 grams of reactant is heated mass of test tube was found to be 9.3 grams.

so mass of product formed = 9.3 - 5

                                             = 4. 3 grams of product is formed (actual yield)

However, he expected the product to be 5 grams (theoretical yield)

Percent yield = \frac{actual yield}{theoretical yield} x 100

          putting the values in the formula:

percent yield = \frac{4.3}{5} x 100

                     = 86 %

86 percent is the percent yield.

5 0
3 years ago
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