if the gas pressure exerted by a gas at 45 degrees celsius in a volume of 1.944 ATM, how many moles of gas are present?

Draw a highly magnified view of a sealed, rigid container filled with a gas. Then draw what it would look like if you cooled the

dusya [7]

Answer:

In order to fully understand the issue of the ideal gas or perfect gas, we must pay attention to the following, an ideal or perfect gas does not really exist, it is a hypothetical gas whose sharing of the variables of pressure, volume and temperature can be fully described by the ideal gas equation.

The molecules that make up an ideal gas do not usually attract or repel each other, and their volume is negligible compared to the volume of the container that contains it. Although in our nature the case of an ideal gas does not exist, the differences between the behavior of a real gas in temperature and pressure margins do not substantially alter the calculations, so we can make use of the equation with all the security, to solve various gas exercises.

Explanation:

The collisions that occur between the molecules and with the molecules and with the walls is elastic because the moment is preserved, in addition to the kinetic energy.

It can be synthesized that a gas is ideal when all collisions that occur between atoms or molecules are completely elastic and there are no attractive forces that are intermolecular.

In ideal gases the kinetic energy is proportional to its temperature. The gases approach an ideal gas if they are mono atomic gases, if it is under pressure and also at room temperature.

The amount of gas in a body is measured in moles. One mole of any type of gas reaches 22.4 liters, in normal condition, 0 ° Celsius and 1 of the pressure atmosphere. That volume is called normal molar volume.

Ideal gases have an equation called the Ideal Gas Equation and is based on three main laws that are Boyle's law, Gay-Lussac's law, Charles's law and also Avogadro's law.

4 0

3 years ago

What is the answer for this question?

emmainna [20.7K]

Hey there!

The more energy a substance is, the more movement it has.

The energy of a substance determines its state of matter.

From least to most energy, it goes solid, liquid, gas.

So it needs to be going from a lower energy state to a higher energy state.

The only one that goes from a lower energy state to a higher energy state is C. H2O (l) --> H2O (g).

Hope this helps!

6 0

3 years ago

Consider the following chemical equation: NH4NO3(s)⟶NH+4(aq)+NO−3(aq) What is the standard change in free energy in kJmol at 298

Galina-37 [17]

Answer:

$\Delta _rG=-4.3\frac{kJ}{mol}$

Explanation:

Hello,

In this case, for the given dissociation reaction, we can compute the enthalpy of reaction considering the enthalpy of formation of each involved species (products minus reactants):

$\Delta _rH=\Delta _fH_{NH^{4+}}+\Delta _fH_{NO_3^-}-\Delta _fH_{NH_4NO_3}\\\\\Delta _rH=-132.5+(-205.0)-(-365.6)=28.1kJ/mol$

Next, the entropy of reaction considering the standard entropy for each involved species (products minus reactants):

$\Delta _rS=S_{NH^{4+}}+S_{NO_3^-}-S_{NH_4NO_3}\\\\\Delta _rS=113.4+146.4-151.1=108.7J/mol*K$

Next, since the Gibbs free energy of reaction is computed in terms of both the enthalpy and entropy of reaction at the given temperature (298.15 K), we finally obtain (two significant figures):

$\Delta _rG=\Delta _rH-T\Delta _rS\\\\\Delta _rG=28.1kJ/mol-(298.15 K)(108.7\frac{J}{mol*K}*\frac{1kJ}{1000J} )\\\\\Delta _rG=-4.3\frac{kJ}{mol}$

Best regards.

6 0

3 years ago

Chlorine, selenium and bromine are located near each other on the periodic table. Which of

andriy [413]

Answer:

GIMME DEM POINTS

Explanation:

TROLLLLLEDDDD

5 0

3 years ago

what is the approximate ph at the equivalence point of a weak acid-strong base titration if 25 ml of aqueous formic acid require

vivado [14]

Answer:

pH at equivalence point is 8.52

Explanation:

$HCOOH+NaOH\rightarrow HCOO^{-}Na^{+}+H_{2}O$

1 mol of HCOOH reacts with 1 mol of NaOH to produce 1 mol of $HCOO^{-}$

So, moles of NaOH used to reach equivalence point equal to number of moles $HCOO^{-}$ produced at equivalence point.

As density of water is 1g/mL, therefore molarity is equal to molality of an aqueous solution.

So, moles of $HCOO^{-}$ produced = $\frac{29.80\times 0.3567}{1000}moles=0.01063moles$

Total volume of solution at equivalence point = (25+29.80) mL = 54.80 mL

So, at equivalence point concentration of $HCOO^{-}$ = $\frac{0.01063\times 1000}{54.80}M=0.1940M$

At equivalence point, pH depends upon hydrolysis of $HCOO^{-}$ . So, we have to construct an ICE table.

$HCOO^{-}+H_{2}O\rightleftharpoons HCOOH+OH^{-}$

I: 0.1940 0 0

C: -x +x +x

E: 0.1940-x x x

So, $\frac{[HCOOH][OH^{-}]}{[HCOO^{-}]}=K_{b}(HCOO^{-})=\frac{10^{-14}}{Ka(HCOOH)}$

species inside third bracket represent equilibrium concentrations

So, $\frac{x^{2}}{0.1940-x}=5.56\times 10^{-11}$

or, $x^{2}+(5.56\times 10^{-11}\times x)-(1.079\times 10^{-11})=0$

So, $x=\frac{-(5.56\times 10^{-11})+\sqrt{(5.56\times 10^{-11})^{2}+(4\times 1.079\times 10^{-11})}}{2}$

So, $x=3.285\times 10^{-6}M$

So, $pH=14-pOH=14+log[OH^{-}]=14+logx=14+log(3.285\times 10^{-6})=8.52$

5 0

3 years ago

if the gas pressure exerted by a gas at 45 degrees celsius in a volume of 1.944 ATM, how many moles of gas are present?​

if the gas pressure exerted by a gas at 45 degrees celsius in a volume of 1.944 ATM, how many moles of gas are present?