To answer this question, we need to use the ideal gas law equation, which is PV = nRT.

Given:
- Pressure (P) = 2.0 x 10^5 Pa
- Volume (V) = 0.030 m^3
- Temperature (T) = 600 K
- Gas constant (R) = 8.31 J/(mol.K)

We can calculate the number of moles of oxygen (n) using the ideal gas law:

n = PV/RT = (2.0 x 10^5 Pa x 0.030 m^3) / (8.31 J/(mol.K) x 600 K) = 1.2 mol

The balanced chemical equation for the reaction of magnesium with oxygen is 2Mg + O2 - 2MgO.

From this equation, we can see that 1 mol of oxygen reacts with 2 mol of magnesium to form 2 mol of MgO.

Since we only have 1 mol of magnesium, only half of the oxygen will be used up.

Therefore, the percentage of the oxygen that will be used up is 50%.

None of the options A, B, C, D are correct.

Question

To answer this question, we need to use the ideal gas law equation, which is PV = nRT.

Given:
- Pressure (P) = 2.0 x 10^5 Pa
- Volume (V) = 0.030 m^3
- Temperature (T) = 600 K
- Gas constant (R) = 8.31 J/(mol.K)

We can calculate the number of moles of oxygen (n) using the ideal gas law:

n = PV/RT = (2.0 x 10^5 Pa x 0.030 m^3) / (8.31 J/(mol.K) x 600 K) = 1.2 mol

The balanced chemical equation for the reaction of magnesium with oxygen is 2Mg + O2 -> 2MgO.

From this equation, we can see that 1 mol of oxygen reacts with 2 mol of magnesium to form 2 mol of MgO.

Since we only have 1 mol of magnesium, only half of the oxygen will be used up.

Therefore, the percentage of the oxygen that will be used up is 50%.

None of the options A, B, C, D are correct.

Knowee AI · Accepted Answer