Question

if a volume of nitric oxide gas at 25.0 °c increases from 2.00 l to 3.00 l, what is the final celsius temperature? assume pressure and amount remains constant. -74 °c 17 °c 174 °c 38 °c 199 °c question 2 0.25 pts in the previous question, what happened to the volume and the temperature? the temperature increased and the volume decreased. the temperature decreased and the volume increased. the temperature decreased and the volume decreased. the temperature increased and the volume increased.

Explanation:

Question 1 (First Question)

Step1: Recall Charles's Law

Charles's Law states that for a fixed amount of gas at constant pressure, $\frac{V_1}{T_1}=\frac{V_2}{T_2}$, where $V$ is volume and $T$ is absolute temperature (in Kelvin).

Step2: Convert initial temperature to Kelvin

Initial temperature $T_1 = 25.0^\circ\text{C} + 273.15 = 298.15\ \text{K}$. Initial volume $V_1 = 2.00\ \text{L}$, final volume $V_2 = 3.00\ \text{L}$.

Step3: Solve for $T_2$

Rearrange Charles's Law: $T_2=\frac{V_2\times T_1}{V_1}$. Substitute values: $T_2=\frac{3.00\ \text{L}\times298.15\ \text{K}}{2.00\ \text{L}} = 447.225\ \text{K}$.

Step4: Convert back to Celsius

Final temperature in Celsius: $T_2 - 273.15 = 447.225 - 273.15 = 174.075^\circ\text{C}\approx174^\circ\text{C}$.

From the first question, volume increased from 2.00 L to 3.00 L, and temperature increased from 25.0 °C to ~174 °C (since $T_2 > T_1$). So both volume and temperature increased.

Answer:

174 °C (Option: 174 °C)

Question 2 (Second Question)