A 226.4-l cylinder contains 65.5% he(g) and 34.5% kr(g) by mass at 27.0°c and 1.40 atm total pressure. what is the mass of he in
2 answers:
The helium (He) mass in the container is calculated to be 0.2 grams
Solution:
First, we need to determine the gas moles in the container using the ideal gas equation:
given that: P = 1.40 atm (pressure of the gas)
V = 226.4 L (volume) R = 0.0821 Latm/moleK (gas constant)
T =
n =? (moles of gas)
Substituting these values into the equation provides the total moles of gas present.
Next, we will calculate the moles of helium.
Then the mass of helium in the container can be ascertained.You might be interested in
In the reaction: <span>caco3(s) → cao(s) + co2(g), it is evident that
1 mol (which is 100 g) of CaCO3 yields 1 mol (which is 44 g) of CO2
Now, the molarity of CaCO3 present in the reaction system is
</span>=
=
= 0.45 mol
Thus, 0.45 mol of CaCO3 leads to the formation of 0.45 mol of CO2.
According to the ideal gas equation, we have PV = nRT
V =
.
Considering P = 645 torr = 0.8487 atm (because 1 atm = 760 torr)
In that case, V =
= 34.8 l
1 mol (which is 100 g) of CaCO3 yields 1 mol (which is 44 g) of CO2
Now, the molarity of CaCO3 present in the reaction system is
</span>=
=
Thus, 0.45 mol of CaCO3 leads to the formation of 0.45 mol of CO2.
According to the ideal gas equation, we have PV = nRT
V =
Considering P = 645 torr = 0.8487 atm (because 1 atm = 760 torr)
In that case, V =
= 34.8 l
Response:
Here's my calculation
Clarification:
Assume the starting concentrations of H₂ and I₂ are 0.030 and 0.015 mol·L⁻¹, respectively.
We need to determine the initial concentration of HI.
1. We will need a chemical equation with concentrations, so let's compile all the information in one location.
H₂ + I₂ ⇌ 2HI
I/mol·L⁻¹: 0.30 0.15 x
2. Calculate the concentration of HI
3. Plot the initial values
The graph below visualizes the initial concentrations as plotted on the vertical axis.
