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Dimas [21]
2 years ago
8

4. Substances that existed before mixing-still exist-after substances-are-mixed----

Chemistry
1 answer:
pantera1 [17]2 years ago
5 0
False; Because when 2 substances are mixed another substance is created.
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Calculate the number of grams in magnesium present in 25 g of magnesium phosphate
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Suppose that in an ionic compound, "m" represents a metal that could form more than one type of ion. in the formula mf2 , the ch
geniusboy [140]
F (Fluorine) is in column (group/family) VIIA, or the "halogens". When you see the halogens (Fluorine, Chlorine, Bromine, and Iodine) in combination with a metal, each halogen atom present will carry a -1 charge. We can see that the atom has no charge, so the metal must cancel out the negative charges brought by the two fluorine atoms.
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3 0
3 years ago
Can you help me out plz and thank u​
Nonamiya [84]

Answer:

stirring

Explanation:

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5 0
3 years ago
The molecular weight of a gas is ________ g/mol if 3.5 g of the gas occupies 2.1 l at stp
bija089 [108]
<span>Pre-1982 definition of STP: 37 g/mol Post-1982 definition of STP: 38 g/mol This problem is somewhat ambiguous because the definition of STP changed in 1982. Prior to 1982, the definition was 273.15 K at a pressure of 1 atmosphere (101325 Pascals). Since 1982, the definition is 273.15 K at a pressure of exactly 100000 Pascals). Because of those 2 different definitions, the volume of 1 mole of gas is either 22.414 Liters (pre 1982 definition), or 22.71098 liters (post 1982 definition). And finally, there's entirely too many text books out there that still use the 35 year obsolete definition. So let's solve this problem using both definitions and you need to pick the correct answer for the text book you're using. First, determine how many moles of gas you have. Just simply divide the volume you have by the molar volume. Pre-1982: 2.1 / 22.414 = 0.093691443 moles Post-1982: 2.1 / 22.71098 = 0.092466287 moles Now determine the molar mass. Simply divide the mass by the moles. So Pre-1982: 3.5 g / 0.093691443 moles = 37.35666667 g/mol Post-1982: 3.5 g / 0.092466287 moles = 37.85163333 g/mol Finally, round to 2 significant figures. So Pre-1982: 37 g/mol Post-1982: 38 g/mol</span>
5 0
3 years ago
Hydrogen and iodine react to form hydrogen iodide, like this: H_2 (g) + I_2 (g) rightarrow 2 HI(g) Also, a chemist finds that at
telo118 [61]

This is an incomplete question, here is a complete question.

Hydrogen and iodine react to form hydrogen iodide, like this:

H_2(g)+I_2(g)\rightarrow 2HI(g)

Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen, iodine, and hydrogen iodide has the following composition:

Compound            Pressure at equilibrium

H_2                                   61.8 atm

I_2                                    46.5 atm

HI                                  52.3 atm

Calculate the value of the equilibrium constant K_p for this reaction. Round your answer to 2 significant digits.

Answer : The value of equilibrium constant K_p for this reaction is, 0.952

Explanation :

The given chemical reaction :

H_2(g)+I_2(g)\rightarrow 2HI(g)

The expression of K_p for above reaction follows:

K_p=\frac{(P_{HI})^2}{P_{H_2}\times P_{I_2}}

We are given:

P_{H_2}=61.8atm

P_{I_2}=46.5atm

P_{HI}=52.3atm

Putting values in above equation, we get:

K_p=\frac{(52.3)^2}{61.8\times 46.5}\\\\K_p=0.952

Therefore, the value of equilibrium constant K_p for this reaction is, 0.952

7 0
3 years ago
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