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sweet-ann [11.9K]
3 years ago
10

When a scientific theory has been tested and proved by the scientific community, it

Chemistry
2 answers:
nlexa [21]3 years ago
8 0
The answer is true it does become a law
beks73 [17]3 years ago
3 0

Answer:

True

Explanation:

When a theory is proven over and over it will become a law

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A mixture of gaseous CO and H2, called synthesis gas, is used commercially to prepare methanol (CH3OH), a compound considered an
mr_godi [17]

Answer : The value of equilibrium constant (K) is, 424.3

Explanation :  Given,

Concentration of H_2 at equilibrium = 0.067 mol

Concentration of CO at equilibrium = 0.021 mol

Concentration of CH_3OH at equilibrium = 0.040 mol

The given chemical reaction is:

CO+2H_2\rightarrow CH_3OH

The expression for equilibrium constant is:

K_c=\frac{[CH_3OH]}{[CO][H_2]^2}

Now put all the given values in this expression, we get:

K_c=\frac{(0.040)}{(0.021)\times (0.067)^2}

K_c=424.3

Thus, the value of equilibrium constant (K) is, 424.3

4 0
3 years ago
Determine the [H3O+] in a 0.265 M HClO solution. The Ka of HClO is 2.9 × 10-8.
dexar [7]

8.8 × 10-5 M is the  [H3O+] concentration in 0.265 M HClO solution.

Explanation:

HClO is a weak acid and does not completely dissociate in water as ions.

the equation of dissociation can be written and ice table to be formed.

 HClO +H2O ⇒ ClO- + H3O+

I  0.265                0        0

C  -x                    +x     +x

E  0.265-x          +x      +x

Now applying the equation of Ka, where Ka is given as 2.9 × 10-8.

Ka = \frac{[ClO-][H3O+]}{[HClO]}

2.9 × 10^-8 = \frac{[x] [x]}{[0.265-x]}

x^{2} = 7.698 x10^{-9}

x = 8.8 × 10-5 M

The hydronium ion concentration is 8.8 × 10-5 M  in 0.265 M solution of HClO.

8 0
3 years ago
Exercise 2:
vagabundo [1.1K]

Answer:

1. KCLO3------>KCL + 3/2O2(g)

2. 122.5g/mol

3. 0.2mol

4. 18.5g

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3 years ago
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DedPeter [7]
Sissy imposter among us haha
6 0
3 years ago
Nickname for nebula "star _ u _ _ _ _ _
Vilka [71]
Star clusters is the only thing i can think of that would apply.
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3 years ago
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