Volume of Hydrogen V1 = 351mL
Temperature T1 = 20 = 20 + 273 = 293 K
Temperature T2 = 38 = 38 + 273 = 311 K
We have V1 x T2 = V2 x T1
So V2 = (V1 x T2) / T1 = (351 x 311) / 293 = 372.56
Volume at 38 C = 373 ml
Answer:
23
Explanation:
if if you look at the screenshot it has the explanation
Answer:
Explanation:
a ) false.
NH₃ is more polar molecule than PH₃ so inter-molucular attraction is greater in NH₃ ( hydrogen bond ) . Hence vapour pressure is low for NH₃ .
b ) false .
The average kinetic energy of boiling water molecules is lower on a mountaintop than it is at sea level. It is so because water boils at lower temperture on mountain and kinetic energy of molecules depends upon temperature .
c ) false
vapour pressure depends upon temperature .
d ) True
CCl4 is more volatile than CBr4
e ) false
vapour pressure increases as temperature increases.
Answer: gas particles that are in constant motion and exhibit perfectly elastic collisions
Explanation:
<u>Answer:</u> The change in internal energy of the gas is 29.414 kJ.
<u>Explanation:</u>
To calculate the temperature of the gas at different volumes, we use ideal gas equation:
- When volume =
We are given:
Conversion used: 
Putting values in above equation:
- When volume =
We are given:
Putting values in above equation:
- To calculate the change in internal energy, we use the equation:
where,
= change in internal energy = ?
n = number of moles = 4.0 mol
= heat capacity at constant volume = 
= final temperature = 1095.06 K
= initial temperature = 505.41 K
Putting values in above equation, we get:
Converting this value in kilojoules, we use the conversion factor:
1 kJ = 1000 J
So, 
Hence, the change in internal energy of the gas is 29.414 kJ.
