400cm of nitrogens at 30°c is heated at constant pressure to an temperature of 50°c find the new volume of nitrogen
The volume of a given mass of a gas at 20°c and 75cmhg pressure is 228cmsquare3 what will be it's volume at 25°c and 76cmhg pressure?
A certain gas occupied a volume at 150cmsquare3 at an atmosphere pressure of 10suquare5nm-2 what will be its new pressure if the volume is reduced 100cmsquare3 assuming than is no change in temperature ?
A certain amount of gas occupies 5.0cdmsquare3 at 2ATM and 10°c calculate the number of moles present R=0.82Atmdmsquare3 mole
It's difficult to answer multiple questions on one post. Here is the first and second one. For #1, you must mean 400 cc.
Use (V1/T1/) = (V2/T2)
Remember T1 and T2 must be in kelvin.
#2. I have no idea what 228 cmsquare3 means. You probably meant 228 cc or 228 cm^3.
Use (P1V1/T1) = (P2V2/T2)
Remember to convert T2 and T1 to kelvin.
Post your work if you get stuck.
To find the new volume of nitrogen, you can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (constant in this case)
V = volume of the gas (initial and final)
n = number of moles of the gas (constant in this case)
R = ideal gas constant
T = temperature of the gas (initial and final)
R = 0.0821 L·atm/mol·K (ideal gas constant)
First, convert the given temperature from Celsius to Kelvin using the equation:
T(K) = T(°C) + 273.15
Initial temperature (T1) = 30°C + 273.15 = 303.15 K
Final temperature (T2) = 50°C + 273.15 = 323.15 K
Now, plug in the known values into the ideal gas law equation:
P1V1 / T1 = P2V2 / T2
The pressure (P) and number of moles (n) are constant, so they cancel out in this case.
V1 / T1 = V2 / T2
Finally, rearrange the equation to solve for the final volume (V2):
V2 = (V1 * T2) / T1
Given:
V1 = 400 cm^3
Substituting the values:
V2 = (400 cm^3 * 323.15 K) / 303.15 K
Calculating:
V2 ≈ 426.07 cm^3
Therefore, the new volume of nitrogen at a constant pressure, heated from 30°C to 50°C, is approximately 426.07 cm^3.