What is the density (in g/L) of hydrogen gas at 18.0 C and a pressure of 1670 psi?

Why did the scarecrow win an award? Because he was outstanding in his field!

Now, let's calculate the density of hydrogen gas. The first thing we need to do is convert the pressure from psi to atm, as the density formula requires pressure in atm.

1 atm = 14.7 psi

So, dividing the given pressure of 1670 psi by 14.7, we get:

1670 psi / 14.7 psi = 113.61 atm

Now, let's use the ideal gas law equation to find the number of moles of hydrogen gas:

PV = nRT

Given:
P = 113.61 atm (pressure)
V = ? (volume)
n = ? (number of moles)
R = 0.0821 (gas constant)
T = 18.0°C + 273.15 = 291.15 K (temperature in Kelvin)

Now, let's solve for n:

n = PV / RT
= (113.61 atm) (V) / (0.0821 L*atm/mol*K) (291.15 K)

Then, we can use the density formula to calculate the density of hydrogen gas:

Density = mass / volume

Since we know the molar mass of hydrogen is approximately 2.016 g/mol, we can calculate the mass:

mass = n * molar mass = (0.003909 mol) * (2.016 g/mol) = 0.007876 g

Finally, we can calculate the density:

Density = mass / volume

We don't have the volume given, so unfortunately, we can't provide the density of hydrogen gas at 18.0°C and a pressure of 1670 psi. I guess the density of humor in this bot's response is high, but the density of hydrogen gas will have to remain a mystery!

To find the density of hydrogen gas at a given temperature and pressure, we can use the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

First, let's convert the pressure from psi to atm, since the gas constant (R) is determined in terms of atm.

1 atm = 14.7 psi

So,

1670 psi / 14.7 psi/atm = 113.605 atm

Next, we need to convert the temperature from Celsius to Kelvin, since the gas constant is also determined in terms of Kelvin.

To convert Celsius to Kelvin, we can use the formula:

K = °C + 273.15

T = 18.0°C + 273.15 = 291.15 K

Now, let's rearrange the ideal gas law equation to solve for density (d):

PV = nRT

n/V = P/RT

Since density (d) = n/V (moles/volume), we can substitute d for n/V:

d = P/RT

Plugging in the values, we get:

d = (113.605 atm) / [(0.0821 L·atm/mol·K) x (291.15 K)]

Using the gas constant R = 0.0821 L·atm/mol·K, we can calculate the density:

d = 0.290 g/L

Therefore, the density of hydrogen gas at 18.0°C and a pressure of 1670 psi is approximately 0.290 g/L.

To find the density of hydrogen gas at a given temperature and pressure, we can use the ideal gas law formula, which is:

PV = nRT

Where:
P is the pressure in atmospheres (atm)
V is the volume in liters (L)
n is the number of moles (mol)
R is the ideal gas constant, which is 0.0821 L·atm/(mol·K)
T is the temperature in Kelvin (K)

First, we need to convert the given pressure from psi to atm. There are 14.696 psi in 1 atm, so we can use this conversion factor to convert the pressure:

1670 psi * (1 atm / 14.696 psi) = 113.66 atm

Next, we need to convert the given temperature from Celsius to Kelvin. To do this, we use the formula:

T(K) = T(°C) + 273.15

T(K) = 18.0°C + 273.15 = 291.15 K

Substituting the values into the ideal gas law formula, we have:

(113.66 atm) * V = n * (0.0821 L·atm/(mol·K)) * (291.15 K)

Now, we need to rearrange the equation to solve for the number of moles (n):

n = (113.66 atm * V) / (0.0821 L·atm/(mol·K) * 291.15 K)

Since we are looking for the density of hydrogen gas, we want to find the number of moles per liter (mol/L). To do this, we need to divide the number of moles (n) by the volume (V) in liters:

Density = n / V

Density = [(113.66 atm * V) / (0.0821 L·atm/(mol·K) * 291.15 K)] / V

Simplifying the equation, we get:

Density = [113.66 atm / (0.0821 L·atm/(mol·K) * 291.15 K)]

Now, we can directly calculate the density of hydrogen gas.

Density = 0.003945 g/L

So, the density of hydrogen gas at 18.0°C and a pressure of 1670 psi is approximately 0.003945 g/L.

You know the density of H2 at sTP...one mole (2grams) in 22.4 liters.

density at STP is 2/22.4 g/L

so....think this out...

density2=densitySTP*1670PSI /14.6PSI *(273)/(273+18)