The moon does not have its own _______
1 answer:
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Answer:
The space that NH3 occupies is 1,205L
Explanation:
Using the ideal gas law we can find the volume of the gas
Where:
- P is the pressure of the gas in Torr
- V is the volume of the gas in Liters
- n are the moles of gas
- T is the temperature of the gas in Kelvin
- R is the gas constant (62,36 L.Torr/K.mol)
First, we convert the temperature to kelvin, and find the moles of gas using the mass and molecular weight of NH3
T(K)= °C + 273,15= 40 + 273= 313K
Now we find the volume with the ideal gas law
Answer: 0.596
Explanation:
For this problem, we want to find . To do so, we will need to use the ICE chart. The I in ICE is initial quantity. In this case, it is the initial pressure. Pressure is in atm. The C in ICE is change in each quantity. The E is equilibrium.
H₂(g) + I₂(g) ⇄ 2HI(g)
I 3.12 5.52 0
C -0.869 -0.869 +1.738
E 2.251 2.251 1.738
<u>For the steps below, refer to the ICE chart above.</u>
1. Since we were given the initial of H₂, I₂ and equilibrium of 2HI, we can fill those into the chart.
2. Since we were not given the initial for 2HI, we will put 0 in their place.
3. For the change, we need to add pressure to the products to make the reaction reach equilibrium. We would add on the products and subtract from the reactants to equalize the reaction. Since we don't know how much the change in, we can use variable x. We know that the equilibrium of 2HI is 1.738, we know the change is 0.869 because 1.738/2=0.869. Since there are 2 moles of HI, we must divide the equilibrium by 2 to find x, so that we can fill that into the reactants side.
4. With the equilibrium values, we can find the equilibrium pressure. It is products over reactants. We use the values of E.
The [HI]² comes from 2HI. We more the moles to the exponent when we are calculating the equilibrium pressure.
We typically don't put units because K is unitless, but know that the units is atm throughout the entire problem.