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4 years ago

Why can't u mix a chemical with and element

Chemistry

1 answer:

Ilia_Sergeevich [38]4 years ago

7 0

Chemical reaction is elements react with each other so you can mix them

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ACTIVITY: SOLUTION CONCENTRATION VS. CONDUCTIVITY

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the amount of Ba(OH)2 compared to H2SO4?

The Ba(OH)2 dissociates as Ba+2 + 2 OH-. H2SO4 dissociates as 2 H+ + SO4-2.

Why does it not conduct at this low point?

Why does it conduct more before and after this minimum point

Can someone please help with this I am not that great at chemistry. Thankyou fo any help that I ge

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3 years ago

Anything that is measured as 8 on the pH scale is known as a _________.

tatuchka [14]

There could be something more specific, but I do know that 8 indicates a very weak base

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3 years ago

4.2 grams of magnesium metal reacts with excess gold III chloride to form 5.9 grams of gold and also magnesium chloride. What is

Margaret [11]

Answer:

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Explanation:

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3 years ago

Trichloroethylene, a widely used degreasing solvent for machine parts, is produced in a two-step reaction sequence. Ethylene is

solmaris [256]

Answer:

ΔH°C2H2Cl4(l) = -333,36 kJ/mol

ΔH°r₂ = -35,14 kJ/mol

Explanation:

The ΔH°r of the first reaction is:

ΔH°r = -385,76 kJ/mol = (ΔH°C2H2Cl4(l) + ΔH°H2(g)) - (ΔH°C2H4(g) + 2ΔHCl2 (g))

ΔH°H2(g) = 0 kJ/mol

ΔH°C2H4(g) = 52,4 kJ/mol

Δ°HCl2 (g) = 0 kJ/mol

Replacing:

ΔH°C2H2Cl4(l) = -385,76 kJ/mol + 52,4 kJ/mol = <em>-333,36 kJ/mol</em>

The standard heat of the second reaction is:

ΔH°r₂ = ΔH°C2HCl3(l) + ΔH°HCl(g) - ΔH°C2H2Cl4(l)

Where:

ΔH°C2HCl3(l) = -276,2 kJ/mol; ΔH°HCl(g) = -92,3 kJ/mol; ΔH°C2H2Cl4(l) = -333,36 kJ/mol

Replacing:

ΔH°r₂ = -276,2 kJ/mol -92,3 kJ/mol + 333,36 kJ/mol

I hope it helps!

4 0

3 years ago

An equilibrium mixture contains 0.750 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the

sasho [114]

1.302 moles of carbon dioxide would have to be added

<h3>Further explanation</h3>

The equilibrium constant is the value of the product in the equilibrium state of the substance in the right (product) divided by the substance in the left (reactant) with the exponents of each reaction coefficient

The equilibrium constant is based on the concentration (Kc) in a reaction

pA + qB -----> mC + nD

$\large {\boxed {\bold {Kc ~ = ~ \frac {[C] ^ m [D] ^ n} {[A] ^ p [B] ^ q}}}}$

While the equilibrium constant is based on partial pressure

$\large {\boxed {\bold {Kp ~ = ~ \frac {[pC] ^ m [pD] ^ n} {[pA] ^ p [pB] ^ q}}}}$

The value of Kp and Kc can be linked to the formula '

$\large {\boxed {\bold {Kp ~ = ~ Kc. (R.T) ^ {\Delta n}}}}$

R = gas constant = 0.0821 L.atm / mol.K

=n = number of product coefficients-number of reactant coefficients

An equilibrium mixture: 0.750 moles of CO2 and H2, and 0.200 moles of CO and H2O

We determine Kc (constant concentration)

$\displaystyle Kc=\frac{0.75.0.75}{0.2.0.2}\\\\Kc=14.1$

the amount of carbon monoxide to 0.300 mol

Reaction :

CO +H₂O ⇔ CO₂ + H₂

initially 0.2 0.2 0.75+x 0.75

reaction 0.1 0.1 0.1 0.1

product 0.3 0.3 0.65+x 0.65

$\displaystyle Kc=\frac{(0.650+x)(0.65)}{0.3.0.3}\\\\14.1(0.09)=0.4225+0.65x\\\\1.269-0.4225=0.65x\\\\0.8465=0.65x\\\\x=1.302$

<h3>Learn more</h3>

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Keywords: constant equilibrium, Kc, concentration, product, reactant, reaction coefficient

3 0

4 years ago

Read 2 more answers