Using the ideal gas law: PV = nRT; and given the initial conditions:
V1 = 20 cc
T1 = 25 C or 298 K
We are asked to determine the volume at 0 C or 273 K. Assume that the pressure and number of moles are constant. Thus,
V/T = constant, then
V1/T1 = V2/T2
Solve for V2:
20 cc/ 298 K = V2/ 273 K
V2 = 18.32 cc
Answer:
47.5 g of water can be formed
Explanation:
This is the reaction:
CH₄ + 2O₂ → CO₂ + 2H₂O
Methane combustion.
In this process 1 mol of methane react with 2 moles of oxygen to produce 2 moles of water and 1 mol of carbon dioxide.
As ratio is 1:2, I will produce the double of moles of water, with the moles of methane I have.
1.320 mol .2 = 2.64 moles
Now, we can convert the moles to mass (mol . molar mass)
2.64 mol . 18g/mol = 47.5 g
Answer:
V = 0.24 L.
Explanation:
Hello there!
In this case, it is possible to approach this problem by using the ideal gas equation defined by:
Whereas our unknown is V, volume, and we solve for it as follows:
Then since the STP conditions are ate 273.15 K and 1 atm, the volume of 0.011 moles of CO2 gas turns out to be:
Regards!
Answer: absorbs food, breaks down food
Answer:
density of a piece of metal = 7 gr/ml
Explanation:
See the file please