2 mols of oxygen are heated up from a temperature of 20 C and a pressure 1 atm to a temperature of 100 C. Compute:

a) Having constant volume, how much heat must be provided to the gas throughout the process?

b) Having constant pressure, how much work is done throughout the process?

c) Compute in a) and b) cases the variation in the internal energy.

My try:

The molar specific heat of an ideal gas at constant volume is:

$$C_v = \frac{3}{2}R$$

The molar specific heat of an ideal gas at constant pressure is:

$$C_p = \frac{5}{2}R$$

Then at a) it is just about using $Q = nC\Delta T$. My issue here is that the given outcome at a) uses n = 1:

$$Q = nC_v\Delta T = 997.68J$$

I obtained 1995.36J (I used n=2).

To compute Q at constant pressure:

$$Q = nC_p\Delta T = 1662.80J$$

I obtained 3325.6J (I used n=2).

I do not understand why it uses n=1 as it is specified that the gas is formed by 2 mols of oxygen.

b) When heat is supplied at constant pressure the gas disseminates and exerts a positive work (such as on a piston).

However the answer is given as a negative number, which means work is done by the system and not over it. Thus the given answer:

$$W = -nR\Delta T = -1330.24J$$

Here I got the same but positive.

c) Using the first principle of thermodynamics:

$$ \Delta E_i = Q + W$$

When volume is constant:

$$ \Delta E_i = Q_v + W = -332.56J$$

When pressure is constant:

$$ \Delta E_i = Q_p + W = 332.56J$$

What I got before seeing the answers:

When volume is constant:

$$ \Delta E_i = Q_v + W = 3325.60J$$

When pressure is constant:

$$ \Delta E_i = Q_p + W = 4655.84J$$

As you can see all comes down to the definition: $Q = nC_v\Delta T$ I have made some research and in Tipler and $C_v$, $C_p$ and Q are defined:

$$C_v = n\frac{3}{2}R$$

$$C_p = n\frac{5}{2}R$$

$$Q = C\Delta T$$

Eventually it is the same, since I multiplied by 2 (number of mols) in the definition: $Q = nC\Delta T$ and I did not do it my first $C_v$ and $C_p$ definitions. Therefore I think my outcomes are right but what do you think?