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nataly862011 [7]
2 years ago
12

A sample of 8.00 g of Mg(OH)2 is added to 24.2 mL of 0.205 M HNO3. How many moles of Mg(OH)2 our present after the reaction is c

omplete?
Chemistry
1 answer:
kogti [31]2 years ago
6 0

The amount of Mg(OH)2  present after the reaction is complete is 0.136 moles of Mg(OH)2.

The equation of the reaction is;

2HNO3(aq) + Mg(OH)2(aq) -------> Mg(NO3)2(aq) + 2H2O(l)

Number of moles of Mg(OH)2 = 8.00 g/58 g/mol = 0.138 moles

Number of moles of HNO3 = 0.205 M × 24.2 mL/1000 = 0.00496 moles

Given that;

2 moles of HNO3 reacts with 1 mole of Mg(OH)2

0.00496 moles of HNO3 reacts with 0.00496 moles ×  1 mole /2 moles = 0.00248 moles of Mg(OH)2

Hence, Mg(OH)2 is the reactant in excess.

The amount of Mg(OH)2 remaining = Amount present - Amount reacted

Hence; 0.138 moles - 0.00248 moles = 0.136 moles of Mg(OH)2

Learn more: brainly.com/question/9743981

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Which of the following have deliquescent Nature ? ​
Alla [95]

Answer:

Most deliquescent substances are salts. Examples include sodium hydroxide , potassium, hydroxide, ammonium chloride, gold

4 0
3 years ago
How many moles of a gas would occupy 22.4 Liters at 273 K and 1 atm?
Molodets [167]

Answer:

1 mole of a gas would occupy 22.4 Liters at 273 K and 1 atm

Explanation:

An ideal gas is a set of atoms or molecules that move freely without interactions. The pressure exerted by the gas is due to the collisions of the molecules with the walls of the container. The ideal gas behavior is at low pressures, that is, at the limit of zero density. At high pressures the molecules interact and intermolecular forces cause the gas to deviate from ideality.

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:

P * V = n * R * T

In this case:

  • P= 1 atm
  • V= 22.4 L
  • n= ?
  • R= 0.082 \frac{atm*L}{mol*K}
  • T=273 K

Reemplacing:

1 atm* 22.4 L= n* 0.082 \frac{atm*L}{mol*K} *273 K

Solving:

n=\frac{1 atm* 22.4 L}{0.082 \frac{atm*L}{mol*K} *273 K}

n= 1 mol

Another way to get the same result is by taking the STP conditions into account.

The STP conditions refer to the standard temperature and pressure. Pressure values at 1 atmosphere and temperature at 0 ° C (or 273 K) 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.

<u><em>1 mole of a gas would occupy 22.4 Liters at 273 K and 1 atm</em></u>

4 0
2 years ago
Consider the following balanced equation:
Serga [27]
<span>Zn⁰ + 2H⁺ ------> Zn²⁺ + H2⁰

H⁺ ion has oxidation number +1.
Zn²⁺ ion has oxidation number +2.
Atom of Zn has electric charge 0, and each hydrogen atom in the molecule H2 have oxidation number 0. So, </span> Zn and each hydrogen atom in H2 have oxidation numbers equals "0".<span>

</span><span>Answer is
D. Zn and each hydrogen atom in H2</span><span>

</span>
4 0
3 years ago
Hurricanes derive their energy from: Group of answer choices the latent heat of condensation. the latent heat of fusion. the lat
klemol [59]

Hurricanes derive their energy from the Latent heat of condensation.

Hence, Option (1) is correct answer.

<h3>What is Latent Heat ? </h3>

The heat that is released or absorbed during a phase change of a substance is known as Latent heat.

<h3>What is Hurricanes ?</h3>

Hurricanes is basically a type of storm called a tropical cyclone. These are intense low pressure areas. Hurricanes derive their energy from the latent heat of CONDENSATION.

Thus from the above conclusion we can say that Hurricanes derive their energy from the Latent heat of condensation.

Hence, Option (1) is correct answer.

Learn more about the Latent heat here: brainly.com/question/5401454

#SPJ4  

7 0
2 years ago
Please help! due soon!
nekit [7.7K]

Answer:

I think it's

there are the same number of molecules on each side of the equation, then a change of pressure makes no difference to the position of equilibrium

7 0
3 years ago
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