Cosmic rays are

Can someone please describe these characteristics from the periodic table? Were looking at the elements F, Cl, S, and NE

Vlad [161]

Once you have identified the limiting reactant, you calculate how much of the other reactant it must have reacted with and subtract from the original amount.

7 0

2 years ago

Select the correct answer.

Step2247 [10]

Answer:

Vanadium(V) oxide is the inorganic compound with the formula V2O5. Commonly known as vanadium pentoxide,

Explanation:

then it is answer D

5 0

2 years ago

The equilibrium constant for the formation of ammonia from nitrogen and hydrogen is 1.6 × 102. what is the form of the equilibri

Nimfa-mama [501]

Answer: The expression for equilibrium constant is $\frac{[NH_3]^2}{[H_2]^3[N_2]}$

Explanation: Equilibrium constant is the expression which relates the concentration of products and reactants preset at equilibrium at constant temperature. It is represented as $k_c$

For a general reaction:

$aA+bB\rightleftharpoons cC+dD$

The equilibrium constant is written as:

$k_c=\frac{[C]^c[D]^d}{[A]^a[B]^b}$

Chemical reaction for the formation of ammonia is:

$N_2+3H_3\rightleftharpoons 2NH_3$

$k_c=1.6\times 10^2$

Expression for $k_c$ is:

$k_c=\frac{[NH_3]^2}{[H_2]^3[N_2]}$

$1.6\times 10^2=\frac{[NH_3]^2}{[H_2]^3[N_2]}$

8 0

2 years ago

A mixture of gases with a pressure of 800.0 mm hg contains 60% nitrogen and 40% oxygen by volume. What is the partial pressure o

larisa86 [58]

Answer:

The partial pressure of oxygen in the mixture is 320.0 mm Hg

Explanation:

1) Take a base of 100 liters of mixture:

N: 60% × 100 liter = 60 liter

O: 40 % × 100 liter = 40 liter.

2) Volume fraction:

At constant pressure and temperature, the volume of a gas is proportional to the number of molecules.

Then, the mole ratio is equal to the volume ratio. Callin n₁ and n₂, the number of moles of nitrogen and oxygen, respectively, and V₁, V₂ the volume of the respective gases you can set the proportion:

V₁ / V₂ = n₁ / n₂

That means that the mole ratio is equal to the volume ratio, and the mole fraction is equal to the volume fraction.

Then, since the law of partial pressures of gases states that the partial pressure of each gas is equal to the mole fraction of the gas multiplied by the total pressure, you can draw the conclusion that the partial pressure of each gas is equal to the volume fraction of the gas in the mixture multiplied by the total pressure.

Then calculate the volume fractions:

Volume fraction of a gas = volume of the gas / volume of the mixture

N: 60 liter / 100 liter = 0.6 liter

V: 40 liter / 100 liter = 0.4 liter

3) Partial pressures:

These are the final calculations and results:

Partial pressure = volume fraction × total pressure

Partial pressure of N = 0.6 × 800.0 mm Hg = 480.0 mm Hg

Partial pressure of O = 0.4 × 800.0 mm Hg = 320.0 mm Hg

8 0

2 years ago

Compared to CH4,NH3 has:

vitfil [10]

a) NH₃ molecules have stronger intermolecular attractions than CH₄ molecules.

Explanation:

Ammonia molecules have stronger intermolecular attractions compared to methane.

Ammonia molecules have london dispersion forces and hydrogen bonds between their molecules.

Methane molecules have only london dispersion forces in their structure.

hydrogen bonds are very strong attractive forces between molecules in which the hydrogen of a molecule is attracted by a more electronegative atom of another usually oxygen, nitrogen and fluorine.
London dispersion forces are weak forces of attraction between heteronuclear atoms.

Learn more:

Hydrogen bonds brainly.com/question/10602513

#learnwithBrainly

3 0

2 years ago