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4 years ago

Write a balanced chemical equation for the reaction that occurs when calcium metal undergoes a combination reaction with O2(g).

1 answer:

7 0

In order to balance this, you have to count each element where the elements in the reactants side and the product side should have equal number of molecules. The balanced reaction is as follows:

2 Ca + O2 ---> 2CaO

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A certain element has only two naturally occurring isotopes: one with 18 neutrons and the other with 20 neutrons. The element fo

AURORKA [14]

Explanation:

I hope this one is useful, I will complete later

5 0

3 years ago

How many atoms of zinc are in 6.05 moles of zinc

stiv31 [10]

As we know that one mole contains 6.022 × 10²³ particles. And the number of particles are related to moles as,

# of Particles = Moles × 6.022 × 10²³ particles

In case of Zinc atoms,

# of Atoms = Moles × 6.022 × 10²³ Atoms/mol

Putting value of moles.

# of Atoms = 6.05 mol × 6.022 × 10²³ Atoms/mol

# of Atoms = 3.64 × 10²⁴ Atoms

4 0

3 years ago

You have a friend who wants to move to Hawaii because, "Hawaii has better weather". Based on your knowledge from the text, is th

Harrizon [31]

Answer:

"Hawaii has better weather" is an opinion.

Therefore, you would need to support it with facts in order to deem it accurate or not.

If the text suggests that Hawaii has nice weather, then the statement would be accurate.

If the text hints that Hawaii does not have ideal weather, the statement would be inaccurate.

5 0

4 years ago

How many grams of O2 are needed to react with 8.15 g of C2H2?

xxTIMURxx [149]

Answer:

25.08 grams of O₂ are needed to react with 8.15 g of C₂H₂.

Explanation:

The balanced reaction is:

2 C₂H₂ + 5 O₂ → 4 CO₂ + 2 H₂O

By reaction stoichiometry, the following amounts of moles of each compound participate in the reaction:

C₂H₂: 2 moles
O₂: 5 moles
CO₂: 4 moles
H₂O: 2 moles

The molar mass of each compound is:

C₂H₂: 26 g/mole
O₂: 32 g/mole
CO₂: 44 g/mole
H₂O: 18 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

C₂H₂: 2 moles* 26 g/mole= 52 g
O₂: 5 moles* 32 g/mole= 160 g
CO₂: 4 moles* 44 g/mole= 176 g
H₂O: 2 moles* 18 g/mole= 36 g

Then you can apply the following rule of three: if by stoichiometry 52 grams of C₂H₂ react with 160 grams of O₂, 8.15 grams of C₂H₂ react with how much mass of O₂?

$mass of O_{2} =\frac{8.15 grams of C_{2} H_{2}*160 grams of O_{2} }{52 grams of C_{2} H_{2}}$

mass of O₂= 25.08 grams

25.08 grams of O₂ are needed to react with 8.15 g of C₂H₂.

8 0

3 years ago

For the following reaction, KP = 0.455 at 945°C: At equilibrium, is 1.78 atm. What is the equilibrium partial pressure of CH4 in

Alborosie

Answer:

See explanation below

Explanation:

The question is incomplete. However, here's the missing part of the question:

"For the following reaction, Kp = 0.455 at 945 °C:

C(s) + 2H2(g) <--> CH4(g).

At equilibrium the partial pressure of H2 is 1.78 atm. What is the equilibrium partial pressure of CH4(g)?"

With these question, and knowing the value of equilibrium of this reaction we can calculate the partial pressure of CH4.

The expression of Kp for this reaction is:

Kp = PpCH4 / (PpH2)²

We know the value of Kp and pressure of hydrogen, so, let's solve for CH4:

PpCH4 = Kp * PpH2²

*: You should note that we don't use Carbon here, because it's solid, and solids and liquids do not contribute in the expression of equilibrium, mainly because their concentration is constant and near to 1.

Now solving for PpCH4:

PpCH4 = 0.455 * (1.78)²

PpCH4 = 1.44 atm

6 0

3 years ago