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3 years ago

A sample of magnesium oxide has a mass of 94.4 g. How many molecules

Chemistry

1 answer:

ella [17]3 years ago

7 0

Answer: 1.414x10^24 molecules in 94.4g MgO

Explanation: molar mass MgO 40.204

molecules in 40.204 g MgO = avogadro number

molecules in 94.4 g MgO = (94.4/40.204)*avogadro number

(94.4/40.204)*6.02214076*10^23 = 14.14x10^23

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Given the equation representing a system at equilibrium N2(g)

RoseWind [281]

Answer:

Decreasing the temperature of the system will shift the reaction rightward.

Explanation:

The complete question is:

Given the equation representing a system at equilibrium:

N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + energy

what changes occur when the temperature of this system is decreased?

<h2>Solution</h2>

Modifying the temperature of a system in equilibrium changes the equilibrium constant and the equilibrium position (concentrations) of the system.

When the temperature is decreased, following LeChatelier's principle that the system will react in a way that seeks to counteract the disturbance, the reaction will shift toward the reaction that produces more heat energy to compensate the temperature decrease.

Thus, decreasing the temperature of the system will favor the forward reaction, more N₂(g) and H₂(g) will be consumed and more NH₃(g) and energy will be produced. Hence, the equilibrium will shift rightward.

8 0

3 years ago

How many moles of p are in 2.4 moles of p2o10?

Vedmedyk [2.9K]

In order to solve this type of problem, we take a look at the subscript of each element involved in the compound. These values signifies the number of particles present of that element in that compound. The calculation is as follows:

2.4 moles P2O10 ( 2 moles P / 1 moles P2O10 ) = 4.8 moles P

8 0

3 years ago

Give 3 examples of solutions, suspensions and colloids..

Vlad [161]

Some examples of solutions":" are salt water, rubbing alcohol, and sugar dissolved in water.

examples of suspensions are muddy water milk of magnesia Slaked lime for whitewashing.

examples of colloids are whipped cream, mayonnaise, milk,

5 0

3 years ago

Read 2 more answers

SO42- + 2Cr(OH)3 + 4OH- â†’ + 2CrO42- + 3SO32- + 5H2O

gizmo_the_mogwai [7]

Answer:

Reduced species and oxidizing agent: sulfur in the form of sulfate.

Oxidized species and reducing agent: chromium in the form of chromous hydroxide.

Explanation:

Hello!

In this case, for the reaction:

$SO_4^{2-} + 2Cr(OH)_3 + 4OH^- \rightarrow 2CrO_4^{2-} + 3SO_3^{2-} + 5H_2O$

We can see that the oxidation states of sulfur and chromium change from +6 to +4 and +3 to +6 respectively; in such a way, since the oxidized species is the same reducing agent because it undergoes an increase in the oxidation state, we infer that chromium is it as it goes from +3 to +6.

Moreover, since the reduced species is the same oxidizing agent because it undergoes a decrease in the oxidation state, we infer that sulfur is it as it goes from +6 to +4.

Best regards!

6 0

3 years ago

A 125 ml sample of gas is at STP how many moles of gas are in the sample

IRINA_888 [86]

Answer:

5.58*10⁻³ moles of gas are in the sample.

Explanation:

The STP conditions refer to the standard temperature and pressure. Pressure values at 1 atmosphere and temperature at 0 ° C are used and are reference values for gases. And in these conditions 1 mole of any gas occupies an approximate volume of 22.4 liters.

Being 1000 mL equivalent to 1 L, then 125 mL is equal to 0.125 L. Then you can apply the following rule of three: if by STP conditions 22.4 L are occupied by 1 mole, 0.125 L are occupied by how many moles?

$amount of moles=\frac{0.125 L*1 mole}{22.4 L}$

aomunt of moles= 5.58*10⁻³ moles

5.58*10⁻³ moles of gas are in the sample.

4 0

3 years ago

Read 2 more answers