<span>Using PV=nRT to find the moles and then convert back.
</span><span>4x=.8944
</span><span>solve for x then use the pressure for lets say CO2 put that into PV=nRT then solve for n then convert over.
</span>
<span>(.2236)(2)/(298*.08206) = .0183*96g/mol = 1.76g
</span>
<span>For C:
[NH3]^2[CO2][H2O] = Kp
x=0.2236
(2*.2236)^2(.2236)*(.2236)
=0.001
</span>
Answer:
The mass number (A), also called atomic mass number or nucleon number, is the total number of protons and neutrons (together known as nucleons) in an atomic nucleus. The mass number is different for each different isotope of a chemical element.
Answer: option B.
carbon + oxygen → carbon dioxide
Explanation:
Answer:
0.382 atm
Explanation:
In order to find the pressure, you need to know the moles of carbon dioxide (CO₂) gas. This can be found by multiplying the mass (g) by the molar mass (g/mol) of CO₂. It is important to arrange the conversion in a way that allows for the cancellation of units.
Molar Mass (CO₂): 12.011 g/mol + 2(15.998 g/mol)
Molar Mass (CO₂): 44.007 g/mol
15 grams CO₂ 1 mole
---------------------- x ------------------------ = 0.341 moles CO₂
44.007 grams
To find the pressure, you need to use the Ideal Gas Law equation.
PV = nRT
In this equation,
-----> P = pressure (atm)
-----> V = volume (L)
-----> n = moles
-----> R = Ideal Gas Constant (0.08206 atm*L/mol*K)
-----> T = temperature (K)
After you convert Celsius to Kelvin, you can plug the given and calculated values into the equation and simplify to find the pressure.
P = ? atm R = 0.08206 atm*L/mol*K
V = 20 L T = 0 °C + 273.15 = 273.15 K
n = 0.341 moles
PV = nRT
P(20 L) = (0.341 moles)(0.08206 atm*L/mol*K)(273.15 K)
P(20 L) = 7.64016
P = 0.382 atm
Au, N, O ( give me brainliest please)