Answer:
0.25 mole of CO₂
Explanation:
We'll begin by calculating the mass of oxygen in 1 mole of carbon dioxide (CO₂). This is illustrated below:
Molecular formula of carbon dioxide
=> CO₂
Mass of oxygen in CO₂ = 2O
= 2 × 16
= 32 g
Thus, 1 mole of CO₂ contains 32 g of oxygen.
Finally, we shall determine the number of mole of CO₂ that contains 8 g of oxygen. This can be obtained as follow:
1 mole of CO₂ contains 32 g of oxygen.
Therefore, Xmol of CO₂ will contains 8 g of oxygen i.e
Xmol of CO₂ = 8/32
Xmol of CO₂ = 0.25 mole
Thus, 0.25 mole of CO₂ contains 8 g of oxygen.
Answer:
The dynamic viscosity of the liquid is 0.727 kg/m*s
Explanation:
In the equation for that viscosimeter, ν = KR⁴t, <u>the terms K and R are not dependent on the liquid that is being tested</u>, unlike ν and t.
Using that equation and the data given in the problem, we can calculate the product of K and R⁴.
1.19*10⁻³m²/s = (KR⁴)* 1430 s
KR⁴=8,32*10⁻⁷m²/s²
We can now calculate the<em> </em><u><em>kinematic</em></u> viscosity of the unknown liquid.
ν=8,32*10⁻⁷m²/s²*900s
ν=7.49*10⁻⁴m²/s
The relationship between the <em>kinematic</em> viscosity and the <em>dynamic</em> viscosity is given by the equation μ=ν * ρ, where μ is the dynamic viscosity and ρ is the density. Thus:
μ=7.49*10⁻⁴m²/s * 970 kg/m³
μ=0.727 kg/m*s
Respuesta:
90.0 %
Explicación:
Paso 1: Escribir la ecuación química balanceada
N₂ + 3 H₂ ⇒ 2 NH₃
Paso 2: Calcular el rendimiento teórico de NH₃ a partir de 140 g de N₂
En la ecuación balanceada, participan de N₂: 1 mol × 28.01 g/mol = 28.01 g y de NH₃: 2 mol × 17.03 g/mol = 34.06 g.
140 g N₂ × 34.06 g NH₃ /28.01 g N₂ = 170 g NH₃
Paso 3: Calcular el rendimiento porcentual de NH₃
El rendimiento experimental de NH₃ es 153 g. Podemos calcular el rendimiento porcentual usando la siguiente fórmula.
R% = rendimiento experimental / rendimiento teórico × 100%
R% = 153 g / 170 g × 100% = 90.0 %
Answer:
10g/cm^3, I think.
Explanation:
2x2x2=8cm^3 for the volume.
Divide 80g by that, you get 10g/cm^3, I think.
Answer:
The forward reaction will be favored.
Explanation:
The reaction is:
As per equation (equilibrium equation), there are two moles of gaseous molecules on product side and three moles of reactant side.
a) If we increase pressure, the volume will decrease.
b) Due to decrease in volume, the moles per unit volume will increase.
c) In order to attain equilibrium again, the system will shift in the direction where it can nullify this effect [Le Chatelier's principle]
d) This can be done, if system moves in the direction where number of moles of gaseous molecules are less, which is product side.
e) Thus forward reaction will be favored.
