Nickel metal reacted with oxygen: Ni (s) + O2 (g) --> Ni2O3 (s). 95.00g of Nickel is reacted with 2.000L oxygen at 10.56 atm and 30.00 degrees Celsius. At the end of the reaction the pressure was reduced to 7.56 atm at the same temperature and volume. How many grams of Nickel (III) oxide are produced?

To find the number of grams of Nickel (III) oxide (Ni2O3) produced, we need to use the given information about the reaction and the change in pressure.

Here's the step-by-step solution:

1. Convert the given temperature from Celsius to Kelvin:
Kelvin = Celsius + 273.15
Temperature in Kelvin: 30.00 + 273.15 = 303.15 K

2. Apply the ideal gas law equation to calculate the initial number of moles of oxygen:
PV = nRT
n = (PV) / RT
P = pressure = 10.56 atm
V = volume = 2.000 L
R = ideal gas constant = 0.0821 L·atm/mol·K
T = temperature in Kelvin = 303.15 K

n = (10.56 atm * 2.000 L) / (0.0821 L·atm/mol·K * 303.15 K)

3. Calculate the initial moles of oxygen:
n = 0.827 mol

4. According to the balanced chemical equation:
2 moles of nickel react with 3 moles of oxygen to produce 1 mole of Nickel (III) oxide (Ni2O3).

5. Determine the moles of Nickel (III) oxide (Ni2O3) produced:
Since the moles of oxygen is known, we need to find the moles of Ni2O3.
Using the mole ratio from the balanced equation:
n(Ni2O3) = (n(O2) / 3) * 2
n(Ni2O3) = (0.827 mol / 3) * 2

6. Calculate the molar mass of Ni2O3:
Atomic mass of Ni = 58.69 g/mol
Atomic mass of O = 16.00 g/mol
Molar mass of Ni2O3 = (2 * 58.69 g/mol) + (3 * 16.00 g/mol) = 165.18 g/mol

7. Calculate the mass of Ni2O3 produced:
Mass of Ni2O3 = n(Ni2O3) * Molar mass of Ni2O3

Mass of Ni2O3 = ((0.827 mol / 3) * 2) * 165.18 g/mol

8. Round the final answer to the appropriate significant figures based on the given data.

To determine the number of grams of Nickel (III) oxide produced in the reaction, we need to use the given information about the reactants and conditions and apply the principles of stoichiometry and gas laws. Here's the step-by-step process to find the answer:

Step 1: Convert the given temperature from Celsius to Kelvin:
Given temperature = 30.00°C
Convert to Kelvin: T(K) = T(°C) + 273.15
T(K) = 30.00°C + 273.15 = 303.15 K

Step 2: Use the ideal gas law to calculate the number of moles of oxygen:
PV = nRT
Where:
P = pressure (in atmospheres) = 10.56 atm
V = volume (in liters) = 2.000 L
n = number of moles of gas
R = gas constant = 0.0821 L·atm/(mol·K)
T = temperature (in Kelvin) = 303.15 K

Rearranging the equation, we get:
n = PV / RT

Substitute the given values:
n = (10.56 atm)(2.000 L) / (0.0821 L·atm/(mol·K))(303.15 K)

Calculate the value of 'n'.

Step 3: Determine the mole ratio between Nickel and Nickel (III) oxide:
From the balanced equation:
Ni (s) + O2 (g) --> Ni2O3 (s)
The stoichiometric ratio is 2 moles of Ni2O3 produced per 1 mole of Ni consumed.

Step 4: Convert moles of Nickel (III) oxide to grams:
Use the molar mass of Nickel (III) oxide (Ni2O3) to convert moles to grams.

Molar mass of Ni2O3 = (atomic mass of Ni x 2) + (atomic mass of O x 3)

Look up the atomic masses of Ni and O from the periodic table and calculate the molar mass of Ni2O3.

Step 5: Calculate the mass of Nickel (III) oxide produced:
Multiply the number of moles of Nickel (III) oxide by its molar mass to get the mass in grams.

Using these steps, you can find the answer to the question.