Question

Какова температура 1,6x10^-2 кг водорода находящегося под давлением 10^6 Па и занимающего объем 2x10^-3 м^3 ? Молярная масса кислорода 0,002 кг/моль

Answer 1

Fтяж=mg,
m - масса в кг
g - ускорение свободного падения и равно оно 10 м/с^2

Answer 2

Calculation of Temperature

To calculate the temperature of the given amount of hydrogen gas, we can use the ideal gas law equation:

PV = nRT

Where: - P is the pressure of the gas (in Pascals) - V is the volume of the gas (in cubic meters) - n is the number of moles of the gas - R is the ideal gas constant (8.314 J/(mol·K)) - T is the temperature of the gas (in Kelvin)

First, we need to calculate the number of moles of hydrogen gas using its molar mass and the given mass:

n = m / M

Where: - n is the number of moles - m is the mass of the gas (in kilograms) - M is the molar mass of the gas (in kg/mol)

Given: - Mass of hydrogen gas (m) = 1.6 x 10^-2 kg - Molar mass of hydrogen (M) = 0.002 kg/mol

Using the given values, we can calculate the number of moles of hydrogen gas:

n = (1.6 x 10^-2 kg) / (0.002 kg/mol)

Now, we can substitute the values into the ideal gas law equation and solve for the temperature (T):

P * V = n * R * T

Given: - Pressure of hydrogen gas (P) = 10^6 Pa - Volume of hydrogen gas (V) = 2 x 10^-3 m^3 - Ideal gas constant (R) = 8.314 J/(mol·K)

Substituting the values into the equation:

(10^6 Pa) * (2 x 10^-3 m^3) = [(1.6 x 10^-2 kg) / (0.002 kg/mol)] * (8.314 J/(mol·K)) * T

Simplifying the equation:

2 x 10^3 J = (8.314 J/(mol·K)) * T * [(1.6 x 10^-2 kg) / (0.002 kg/mol)]

Solving for T:

T = (2 x 10^3 J) / [(8.314 J/(mol·K)) * [(1.6 x 10^-2 kg) / (0.002 kg/mol)]]

Now, let's calculate the temperature using the given values:

T = (2 x 10^3 J) / [(8.314 J/(mol·K)) * [(1.6 x 10^-2 kg) / (0.002 kg/mol)]]

T = 381.7 K

Therefore, the temperature of the given amount of hydrogen gas is approximately 381.7 Kelvin.

Please note that the calculation assumes ideal gas behavior and neglects any deviations from the ideal gas law.