Question

At 127°C temperature and 152 cm pressure calculate the volume
occupied by 34 gram of ammonia​

Answer 1

Answer:

22.4L

Molar mass of NH3 is 17g. So the volume of 17g of NH3 i.e 1 mole NH3 at N.T.P. will be 22.4L.

Answer 2

The volume occupied by 34 grams of ammonia at a temperature of 127°C and a pressure of 152 cm is approximately 191 mL.

To calculate the volume occupied by 34 grams of ammonia at a temperature of 127°C and a pressure of 152 cm, we can use the ideal gas law equation:

PV = nRT

where P is the pressure in atm, V is the volume in liters, n is the number of moles, R is the gas constant (0.08206 L·atm/mol·K), and T is the temperature in Kelvin.

First, we need to convert the given temperature from Celsius to Kelvin:

T = 127°C + 273.15 = 400.15 K

Next, we can calculate the number of moles of ammonia using its molar mass:

molar mass of NH3 = 14.01 g/mol

number of moles = 34 g / 14.01 g/mol = 2.427 mol

Now we can plug in the values into the ideal gas law equation:

PV = nRT

V = (nRT) / P

V = $(2.427 mol x 0.08206 L·atm/mol·K x 400.15 K) / (152 cm / 760 cm/atm)$

V = 0.191 L or 191 mL

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