Find the volume of an object that has a mass of 20g and density of 184 glcm

Aluminum and copper are examples of what

agasfer [191]

They are examples of elements.

3 0

3 years ago

If you mix equal concentrations of reactants and products, will the reaction proceed to the right or the left? HF(aq)+NO3−(aq)⇌H

kaheart [24]

Answer:

hypompast

Explanation:

4 0

3 years ago

titration 25.0 ml of 3.4 x 10^ -3 M of Ba(OH) Neutralize 16.6 mL of HCL solution. What is the molarity of HCL solution?

marusya05 [52]

What we are give: Concentration of base (CB) = 3.4 × $10^{-3}$
Then convert all volume in ml to L.
Volume of base (VB) 25.0ml = 0.025L
Volume of acid (VA) 16.6ml = 0.0166L
Now that we have everything we use the formula CAVA=CBVB.
Make 'CA' the subject then solve.
CA= $\frac{CBVB}{VA}$

8 0

3 years ago

Determine whether the following hydroxide ion concentrations ([OH−]) correspond to acidic, basic, or neutral solutions by estima

Rzqust [24]

Answer:

See explanation below

Explanation:

To do this, we will use the following expression to calculate the [H⁺]:

[H⁺] = Kw / [OH⁻]

[H⁺] is the same as [H₃O⁺]. So we have the [OH⁻] so, let's replace every value into the above expression to calculate the hydronium concentration and say if it's acidic, basic or neutral. This can be known because if the [H⁺] > 1x10⁻⁷ M the solution is acidic. If it's [H⁺] < 1x10⁻⁷ M the solution is basic, and if it's [H⁺] = 1x10⁻⁷ M the solution is neutral.

a) [H⁺] = 1x10⁻¹⁴ / 6x10⁻¹² = 1.67x10⁻³ M. Acidic.

b) [H⁺] = 1x10⁻¹⁴ / 9x10⁻⁹ = 1.11x10⁻⁶ M. Acidic.

c) [H⁺] = 1x10⁻¹⁴ / 8x10⁻¹⁰ = 1.25x10⁻⁵ M. Acidic.

d) [H⁺] = 1x10⁻¹⁴ / 7x10⁻¹³ = 0.0143 M. Acidic.

e) [H⁺] = 1x10⁻¹⁴ / 2x10⁻² = 5x10⁻¹³ M. Basic.

f) [H⁺] = 1x10⁻¹⁴ / 9x10⁻⁴ = 1.11x10⁻¹¹ M. Basic.

g) [H⁺] = 1x10⁻¹⁴ / 5x10⁻⁵ = 2x10⁻¹⁰ M. Basic.

h) [H⁺] = 1x10⁻¹⁴ / 1x10⁻⁷ = 1x10⁻⁷ M. Neutral.

Part B.

In this part, we'll use the following expression and replace the given values:

[OH⁻] = Kw / [H⁺]

Replacing the values:

[OH⁻] = 1x10⁻¹⁴ / 5.2x10⁻⁵

[OH⁻] = 1.92x10⁻¹⁰ M

PArt C:

In this case, we will use expression of part A, and replace the given values:

[H⁺] = 1x10⁻¹⁴ / 2.7x10⁻²

[H⁺] = 3.7x10⁻¹³ M

8 0

3 years ago

For the reactions system 2H2(g) + S2(g) 2H2S(g), a 1.00 liter vessel is found to contain 0.50 moles of H2, 0.020 moles of S2, an

Mnenie [13.5K]

Answer: 1) $2H_2(g)+S_2(g)\rightleftharpoons 2H_2S(g)$

Equilibrium constant is defined as the ratio of the product of concentration of products to the product of concentration of reactants each term raised to their stochiometric coefficients.

$K_{eq}=\frac{[H_2S]^2}{H_2]^2\times [S_2]}$

where [] = concentration in Molarity= $\frac{moles}{\text {Volume in L}}$

Thus $[H_2S]=\frac{68.5}{1.0}=68.5M$

$[H_2]=\frac{0.50}{1.0}=0.50M$

$[S_2]=\frac{0.020}{1.0}=0.020M$

$K_{eq}=\frac{[68.5]^2}{0.50]^2\times [0.020]}=938450$

As the value of K is greater than 1, the reaction is product favored.

2) $N_2O_4(g)\rightleftharpoons 2NO_2(g)$

$K_{eq}=\frac{[NO_2]^2}{[N_2O_4]}$

$K_{eq}=\frac{[0.500]^2}{[0.0250]}=10$

3) $N_2+3H_2\rightleftharpoons 2NH_3$

$K_{eq}=\frac{[NH_3]^2}{[N_2]\times [H_2]^3}$

4) Reactions which do not continue to completion are called equilibrium reactions as the rate of forward reaction is equal to the rate of backward direction.

3 0

3 years ago

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