Explanation:
The reaction is as follows:
2Mg(s) + O2(g) ---> 2MgO(s)
and the researcher said that 32 g of MgO was produced.
Stoichiometry:
28 g Mg × (1 mol Mg/24.305 g Mg) = 1.15 mol Mg
15 g O2 × (1 mol O2/15.999 g O2) = 0.938 mol O2
1.15 mol Mg × (2 mol MgO/2 mol MgO) = 1.15 mol MgO
1.15 mol MgO × (40.3044 g MgO/1 mol MgO) = 46.6 g MgO
0.938 mol O2 × (2 mol MgO/1 mol O2) = 1.88 mol MgO
1.88 mol MgO × (40.3044 g MgO/1 mol MgO = 75.6 g MgO
Based on these numbers, the amount of product after the reaction is much less than expected so these results don't seem to support the law of conservation of matter.
Answer:
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Explanation:
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First, we have to correct the equation in the question to b(g)⇆ 1/2 A(g)
at the first equation A(g)⇆ 2 B(g) so,
Kc = [B]^2 [ A] = 0.03
by reverse the equation 2B⇆ A
∴ Kc(original) = [A] / [B]^2
= 1/0.03 = 33 M^-1
and the new equation B⇆ (1/2) A
So, the new Kc = √Kc(original = √33
∴ KC = 5.7
Answer: The original volume in liters was 0.0707L
Explanation:
Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.
The combined gas equation is,
where,
= initial pressure of gas = 0.85 atm
= final pressure of gas = 456 mm Hg = 0.60 atm (760mmHg=1atm)
= initial volume of gas = ?
= final volume of gas = 94.0 ml
= initial temperature of gas = 
= final temperature of gas = 
Now put all the given values in the above equation, we get:
(1L=1000ml)
Thus the original volume in liters was 0.0707L
