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3 years ago

What is an empirical formula

2 answers:

8 0

A formula giving the proportions of the elements present in a compound but not the actual numbers or arrangement of atoms.

zlopas [31]3 years ago

6 0

An empirical shows the simplest ratio among atoms in a compound .

<h2>More information</h2>

an empirical formula is the simplest formula for a compound .For example, H2O2 can be reduced to a simpler formula.
Determining a Molecular Formula from an Empirical Formula The empirical formula for a compound is P 2 O 5 . Its experimental molar mass is 284 g/mol.
For example, the empirical formula of benzene (C5H5) is Qj, - because the mole ratio of carbon am'hydrogen is 1:1.

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How many moles of silver oxide (l) are needed to produce 4 moles of silver?

ozzi

The number of moles of silver oxide (I) needed to produce 4 moles of silver is 2 moles

<h3>Stoichiometry </h3>

From the question, we are to determine the number of moles of silver oxide (I) needed to produce 4 moles of silver

First, we will write the balaced chemical equation for the decomposition of silver oxide (I)

2Ag₂O(s) → 4Ag(s) + O₂(g)

This means, 2 moles of silver oxide (I) [Ag₂O] decomposes to give 4 moles of silver and 1 mole of oxygen gas.

From the balanced chemical equation, it is easy to deduce the number of moles of silver oxide (I) that would give 4 moles of silver.

Hence, the number of moles of silver oxide (I) needed to produce 4 moles of silver is 2 moles

Learn more on Stoichiometry here: brainly.com/question/18834543

7 0

3 years ago

. Calculate the final Celsius temperature of sulfur dioxide gas if 50.0 mL of the gas at 20 C and 0.450 atm is heated until the

Anna [14]

Answer:

The final temperature of sulfur dioxide gas is 215.43 C

Explanation:

Gay Lussac's Law establishes the relationship between the temperature and the pressure of a gas when the volume is constant. This law says that if the temperature increases the pressure increases, while if the temperature decreases the pressure decreases. In other words, the pressure and temperature are directly proportional quantities.

Mathematically, the Gay-Lussac law states that, when a gas undergoes a transformation at constant volume, the quotient of the pressure exerted by the temperature of the gas remains constant:

$\frac{P}{T}=k$

Assuming you have a gas that is at a pressure P1 and at a temperature T1 at the beginning of the experiment, by varying the temperature to a new value T2, then the pressure will change to P2, and it will be true:

$\frac{P1}{T1} =\frac{P2}{T2}$

The reference temperature is the absolute temperature (in degrees Kelvin)

In this case:

P1= 0.450 atm
T1= 20 C= 293.15 K (being 0 C= 273.15 K)
P2=0.750 atm
T2= ?

Replacing:

$\frac{0.450atm}{293.15 K} =\frac{0.750 atm}{T2}$

Solving:

$T2 =\frac{0.750 atm}{\frac{0.450atm}{293.15 K} }$

$T2=\frac{0.750 atm}{0.450 atm} *293.15K$

T2=488.58 K

Being 273.15 K= 0 C, then 488.58 K= 215.43 C

The final temperature of sulfur dioxide gas is 215.43 C

6 0

3 years ago

which would you think would be a stronger interaction and why: an interaction between a sodium ion and the prtial negative charg

Karo-lina-s [1.5K]

Answer:

The interaction between sodium ion and the partial negative charge on the oxygen is stronger.

Explanation:

The predominant interaction that exists between sodium ion and the partial negative charge on the oxygen is ion-dipole interaction.

The predominant interaction that exists between two ethanol molecules is hydrogen bonding interaction.

The order of strength of the intermolecular interactions in decreasing order:

Ionic bond > ion-dipole interaction > hydrogen bonding > dipole-dipole interaction > ion-induced dipole interaction > induced dipole- dipole interaction > london force

So, ion-dipole interaction is stronger than hydrogen bonding.

Hence, the interaction between sodium ion and the partial negative charge on the oxygen is stronger.

4 0

3 years ago

Which scenario is an example of primary succession?

pishuonlain [190]

Answer:

the answer to your question is A

8 0

3 years ago

For the following systems at equilibrium C: CaCO3(s) ⇌ CaO(s)+CO2(g) ΔH=+178 kJ/mol D: PCl3(g)+Cl2(g) ⇌ PCl5(g) ΔH=−88 kJ/mol cl

Rama09 [41]

Explanation:

C: $CaCO_3(s)\rightleftharpoons CaO(s)+CO_2(g)$ ΔH=+178 kJ/mol

For an endothermic reaction, heat is getting absorbed during a chemical reaction and is written on the reactant side.

$A+\text{heat}\rightleftharpoons B$

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle. This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

Treat heat as a reactant and on increasing a reactant at equilibrium, shifts the reaction in the forward direction.

Increase temperature → increase in heat → forward direction

Decrease temperature → decease in heat → backward direction

System C - Increase temperature : Reaction will move forward

System C - Decrease temperature : Reaction will move backward

D: $PCl_3(g)+Cl_2(g)\rightleftharpoons PCl_5(g)$ ΔH=−88 kJ/mol

The total enthalpy of the reaction comes out to be negative .

The temperature of the surrounding will increase.

For an exothermic reaction, heat is released during a chemical reaction and is written on the product side.

$A\rightleftharpoons B+\text{ heat}$

Treat heat as a product and on increasing a product at equilibrium, shifts the reaction in the backward direction.

Increase temperature → increase in heat → backward direction

Decrease temperature → decease in heat → forward direction

System D - Increase temperature : Reaction will move backward

System D - Decrease temperature : Reaction will move forward

7 0

3 years ago