Answer:
46.97g
Explanation:
Hello,
To find the theoretical yield, we must first of all get the equation of reaction right in order to know how the compounds combine together.
Equation of reaction;
2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O
From the equation of reaction,
2 moles of C₂H₆ reacts with 7 moles of O₂ to produce 4 moles of CO₂.
Number of moles = mass / molar mass
Mass = number of moles × molar mass
Mass of CO₂ = 4 × 44 = 176g
Mass of C₂H₆ = 2 × 30 = 60g
Mass of O₂ = 7 × 32 = 224g
Therefore, 224g + 60g (O₂ + C₂H₆) = 176g of CO₂.
284g of reactants = 176g of product(CO₂)
(18 + 57.8)g of reactants = x g of products(CO₂)
X = (75.8 × 176) /284
X = 46.97g of CO₂.
Theoretical yield of CO₂ is 46.97g
Explanation:
An element just has one-type atoms/atom (e.g. O2). Meanwhile, a compound is a variety of atoms (e.g. H2O).
Answer:
do you want me to make a vid and send it?
Explanation:
From equation;
P1V1=P2V2
V2=P1V1÷P2
since P2=380mmHg
now;1atm=760mmHg
how about 380mmHg is equal to how many atm?
380×1÷760=0.5atm
P2 now is equal to 0.5atm
back from equation;
P1V1=P2V2
V2=P1V1÷P2
V2=4.0atm×2.0L÷0.5atm
V2=16L
therefore V2=16L.
Answer:
The balanced equation is:
2 HNO3 + Mg ---> Mg(NO3)2 + H2
From the equation, we can see that we need twice the moles of HNO3 than the moles of Mg
Moles of Mg:
Molar mass of Mg = 24 g/mol
Moles = Given mass / Molar Mass
Moles of Mg = 4.47 / 24 = 0.18 moles (approx)
Hence, 2(moles of Mg) = 0.36 moles of HNO3 will be consumed
Number of moles of HNO3 after the reaction is finished is the number of unreacted moles of HNO3
Unreacted moles of HNO3 = Total Moles - Moles consumed
Unreacted moles of HNO3 = 0.64 moles (approx)
Since we approximated the value of moles of Mg, the value of remaining moles of HNO3 will also be approximate
From the given options, we can see that 0.632 moles is the closest value to our answer
Therefore, 0.632 moles will remain after the reaction
