Would all have the same ratio of elements.
Answer:A theory is a well-substantiated explanation of an aspect of the natural world that can incorporate laws, hypotheses and facts.
Explanation:
The theoretical yield of acetate is 2607 g. The actual yield of acetate is 1066.8 g. The percentage yield of acetate is 41%.
If 1 mole of vinegar contains 6.02 x 10^23 particles
x moles of vinegar contains 9.02 x 10^24 particles
x = 1 mole x 9.02 x 10^24 /6.02 x 10^23
x = 15 moles of vinegar
The reaction is as follows;
2HC2H3O2 + CaCO3 -----> Ca(C2H3O2)2 + H2O + CO2
Since 2 moles of vinegar reacts with 1 mole of carbonate
x moles of vinegar reacts with 16.5 moles of carbonate
x = 2 moles x 16.5 moles/ 1 mole
x = 33 moles of vinegar
We can see that the vinegar is the reactant in excess hence the carbonate is the limiting reactant.
Theoretical yield = 16.5 moles x 158 g/mol = 2607 g
Actual yield = 6.35 moles x 158 g/mol = 1066.8 g
Percent yield = 1066.8 g/2607 g × 100/1
= 41%
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32 degrees F
0 degrees C= 32 degrees F
Answer:
The equilibrium partial pressure of NO2 is 0.152 atm
Explanation:
Step 1: Data given
Initial pressure of NO2 = 0.500 Atm
Total pressure inside the vessel at equilibrium = 0.674 atm
Step 2: The balanced equation
2 NO2(g) ⇌ 2 NO(g) + O2(g)
Step 3: The initial pressures
pNO2 = 0.500 atm
pNO = 0 atm
pO2 = 0 atm
Step 4: The pressure at the equilibrium
pNO2 = 0.500 - 2x
pNO = 2x
pO2 = x
Total pressure = 0.674 = (0.500 - 2x) + 2x + x
0.674 = 0.500 + x
x = 0.174
pNO2 = 0.500 - 2*0.174 = 0.152 atm
pNO = 2x = 0.348 atm
pO2 = x = 0.176 atm
The equilibrium partial pressure of NO2 is 0.152 atm
