How many ne atoms are contained in 32.0g of the element?

2. If a student drops a 2.3 g piece of magnesium into a flask of hydrochloric acid, this reaction occurs: Mg + 2HCl MgCl2 + H2

mezya [45]

1.2 L of hydrogen can be produced at a pressure of 2 atm and a temperature of 298 K.

<h3>What is an ideal gas equation?</h3>

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

Step 1: Write the balanced equation

Mg + 2 HCl ⇒ MgCl₂ + H₂

Step 2: Calculate the moles corresponding to 2.3 g of Mg

The molar mass of Mg is 24.31 g/mol.

2.3 g × 1 mol ÷24.31 g = 0.095 mol

Step 3: Calculate the moles of H₂ produced

0.095 mol Mg × 1 mol H₂ ÷ 1 mol Mg = 0.095 mol H₂

Step 4: Calculate the volume occupied by the hydrogen

We will use the ideal gas equation.

P × V = n × R × T

V = n × R × T÷P

V = 0.095 mol × (0.0821 atm.L/mol.K) × 298 K÷2 atm

V = 1.2 L

Learn more about the ideal gas here:

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2 years ago

If you are given an ideal gas with pressure (p)259,392.00 pa and temperature (T)=200°c of 1 mole Argon gas in a volume 8.8dm3,ca

GuDViN [60]

Answer: $R=4.82436 \frac{Pa. m^{3}}{mol. K}$

Explanation:

The Ideal Gas equation is:

$P.V=n.R.T$ (1)

Where:

$P$ is the pressure of the gas

$n$ the number of moles of gas

$R=8.3144598 \frac{Pa. m^{3}}{mol. K}$ is the gas constant

$T$ is the absolute temperature of the gas in Kelvin.

$V$ is the volume

It is important to note that the behavior of a real gas is far from that of an ideal gas, taking into account that <u>an ideal gas is a single hypothetical gas</u>. However, under specific conditions of standard temperature and pressure (T=0\°C=273.15 K and P=1 atm=101,3 kPa) one mole of real gas (especially in noble gases such as Argon) will behave like an ideal gas and the constant R will be $8.3144598 \frac{Pa. m^{3}}{mol. K}$ .

However, in this case we are not working with standard temperature and pressure, therefore, even if we are working with Argon, the value of R will be far from the constant of the ideal gases.

Having this clarified, let's isolate $R$ from (1):