One mole of an ideal gas with a volume of 4.00 liters and a temperature of $0^{\circ} \mathrm{C}$ is mixed with one mole of an ideal gas with a volume of 2.00 liters and a temperature of $100^{\circ} \mathrm{C}$. The volume of the mixture is 6 liters. What is the number density of the mixture?
A) $3.56 \times 10^{26} \mathrm{~m}^{-3}$
B) $2.66 \times 10^{26} \mathrm{~m}^{-3}$
C) $3.21 \times 10^{26} \mathrm{~m}^{-3}$
D) $1.75 \times 10^{26} \mathrm{~m}^{-3}$
E) $2.01 \times 10^{26} \mathrm{~m}^{-3}$

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The Answer of  One mole of an ideal gas with a volume of 4.00 liters and a temperature of $0^{\circ} \mathrm{C}$ is mixed with one mole of an ideal gas with a volume of 2.00 liters and a temperature of $100^{\circ} \mathrm{C}$. The volume of the mixture is 6 liters. What is the number density of the mixture?
A) $3.56 \times 10^{26} \mathrm{~m}^{-3}$
B) $2.66 \times 10^{26} \mathrm{~m}^{-3}$
C) $3.21 \times 10^{26} \mathrm{~m}^{-3}$
D) $1.75 \times 10^{26} \mathrm{~m}^{-3}$
E) $2.01 \times 10^{26} \mathrm{~m}^{-3}$

One Mole of an Ideal Gas with a Volume of 4.00