A 2.747-g sample of manganese metal is reacted with excess HCl gas to produce 3.22 L of H2 at 373 K and 0.951 atm and manganese chloride compound (MnClx) what is the formula of manganese chloride compond produced in the reaction?

Use PV = nRT to calculate the number of mols H2 that was generated. Convert that to mols HCl and from there x of MnClx.

To determine the formula of the manganese chloride compound produced in the reaction, we need to calculate the moles of hydrogen gas produced and the moles of manganese present in the sample.

Step 1: Calculate the moles of hydrogen gas (H2) produced
Using the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature, we can rearrange it to solve for n (number of moles):

n = PV / RT

Given:
Pressure (P) = 0.951 atm
Volume (V) = 3.22 L
Temperature (T) = 373 K
Ideal gas constant (R) = 0.0821 L·atm/(mol·K)

n = (0.951 atm * 3.22 L) / (0.0821 L·atm/(mol·K) * 373 K)
n ≈ 0.115 moles of H2

Step 2: Calculate the moles of manganese (Mn)
Using the molar mass of manganese (Mn), we can convert the mass of the sample to moles:

Molar mass of Mn = 54.938 g/mol (from the periodic table)
Mass of the sample = 2.747 g

moles of Mn = mass of sample / molar mass of Mn
moles of Mn = 2.747 g / 54.938 g/mol
moles of Mn ≈ 0.050 moles of Mn

Step 3: Determine the ratio of Mn to Cl in the compound
Now we need to find the ratio of moles of Mn to Cl in the compound. This can be done by dividing the moles of Mn by the moles of H2:

Moles of Cl = moles of Mn / moles of H2
Moles of Cl = 0.050 moles of Mn / 0.115 moles of H2
Moles of Cl ≈ 0.435 moles of Cl

Step 4: Determine the formula of the compound
To determine the formula of the manganese chloride compound, we need to find the simplest whole-number ratio of Mn to Cl. In this case, the ratio is approximately 1:2.

Therefore, the formula of the manganese chloride compound produced in the reaction is MnCl2.

To determine the formula of the manganese chloride compound produced in the reaction, we need to analyze the given information about the reactants and products.

First, let's convert the mass of manganese metal (2.747 g) to moles. The molar mass of manganese (Mn) is 54.938045 g/mol, so we can calculate:

Number of moles of Mn = Mass of Mn / Molar mass of Mn
= 2.747 g / 54.938045 g/mol

Now, since the reaction is performed with excess HCl gas, the amount of H2 produced is determined by the moles of manganese metal consumed. According to the stoichiometry of the reaction, 1 mole of manganese reacts with 2 moles of HCl to produce 1 mole of H2. Therefore, the number of moles of H2 produced is equal to the number of moles of Mn consumed.

Number of moles of H2 = Number of moles of Mn

Next, we can use the ideal gas law to calculate the number of moles of H2. The ideal gas law is given by:

PV = nRT

Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.

Rearranging the equation to solve for moles (n), we have:

n = PV / RT

Plugging in the values, we get:

Number of moles of H2 = (0.951 atm * 3.22 L) / (0.0821 L·atm/mol·K * 373 K)

Now that we have the number of moles of both Mn and H2, we can determine the ratio of moles between them. Since 1 mole of Mn reacts with 1 mole of MnClx, and 1 mole of MnClx contains x moles of Cl, the formula of the manganese chloride compound can be determined by comparing the ratio of moles of Mn to moles of Cl.

If the ratio of moles of Mn to moles of Cl is 1:1, then the formula of the manganese chloride compound is MnCl.

If the ratio of moles of Mn to moles of Cl is 1:2, then the formula of the manganese chloride compound is MnCl2.

To find out the exact ratio, divide the number of moles of Mn by the number of moles of H2, and determine if it is approximately 1 or 2.

Once the ratio of moles is determined, the formula of the manganese chloride compound produced in the reaction can be deduced.