AMMONIA GAS OCCUPIES A VOLUME OF 5.00 L AT 4DEGREES C AT 760 TORR. FIND ITS VOLUME AT77DEGREES C AND 800 TORR
Use (P1V1/T1) = (P2V2/T2)
Note that the use of all caps makes the question hard to read. Also, finding the space bar would improve the readability.
To find the volume of ammonia gas at a different temperature and pressure, we can use the combined gas law formula:
\[ P_1V_1/T_1 = P_2V_2/T_2 \]
In this case, we have:
P1 = 760 Torr (initial pressure)
V1 = 5.00 L (initial volume)
T1 = 4 degrees C + 273.15 = 277.15 K (initial temperature)
P2 = 800 Torr (final pressure)
V2 = ? (final volume - what we're trying to find)
T2 = 77 degrees C + 273.15 = 350.15 K (final temperature)
By plugging these values into the combined gas law formula, we can solve for V2:
\[ P_1V_1/T_1 = P_2V_2/T_2 \]
\[ (760 \, \mathrm{torr})(5.00 \, \mathrm{L})/(277.15 \, \mathrm{K}) = (800 \, \mathrm{torr})(V_2)/(350.15 \, \mathrm{K}) \]
Now, let's solve the equation for V2:
\[ V_2 = \left( \frac{(760 \, \mathrm{torr})(5.00 \, \mathrm{L})(350.15 \, \mathrm{K})}{(277.15 \, \mathrm{K})(800 \, \mathrm{torr})} \right) \]
By substituting the given values into the equation and performing the necessary calculations, we find:
\[ V_2 \approx 6.06 \, \mathrm{L} \]
Therefore, the volume of ammonia gas at 77 degrees C and 800 Torr is approximately 6.06 L.