Thats a chemical reaction. I think
The ammonia gas, having a lower molecular weight than the hydrogen chloride, will diffuse faster and travel a greater length of the tube. Consequently, the white ring of ammonium chloride will form much closer to hydrochloric acid end of the tube. Which in conclusion your answer will be D :)
Answer:
173.8g
Explanation:
STP means standard temperature and pressure
The temperature there is 273k while the pressure is 1 atm
now we are to use the ideal gas equation to get the number of moles first
Mathematically;
PV = nRT
here P = 1 atm
V = 88.5 L
n = ?
R = molar gas constant = 0.082 L atm mol^-1 K^-1
Now rewriting the equation we can have
n = PV/RT
plugging the values we have
n = (1 * 88.5)/(0.082 * 273)
n = 88.5/22.386
n = 3.95 moles
Now we proceed to get the mass
Mathematically;
mass = no of moles * molar mass
molar mass of carbon iv oxide is 44g/mol
mass = 3.95 * 44 = 173.8 g
Answer:
42.9%
Explanation:
Step 1: Write the balanced decomposition reaction
PbO₂ ⇒ Pb + O₂
Step 2: Calculate the theoretical yield of O₂ from 5.77 g of PbO₂
According to the balanced equation, the mass ratio of PbO₂ to O₂ is 239.2:32.00.
5.77 g PbO₂ × 32.00 g O₂/239.2 g PbO₂ = 0.772 g O₂
Step 3: Calculate the percent yield of O₂
The real yield of O₂ is 0.331 g. The percent yield of O₂ is:
%yield = real yield / theoretical yield × 100%
%yield = 0.331 g / 0.772 g × 100% = 42.9%
Answer:
110.92 g
Explanation:
Amount of Ni2O3 consumed= 55.3/59 =0.94 moles
From the reaction equation;
2 moles of Ni2O3 yields 4 moles of Ni
0.94 moles yields 0.94 moles * 4/2
= 1.88 moles of Ni2O3
Mass of 1.88 moles of Ni2O3 = 1.88 moles of Ni2O3 * 59 gmol-1 = 110.92 g