Answer:
The answer to your question is below
Explanation:
Trial 1 Trial 2
mass of Mg 0.255 g 0.353 g
mass of MgO 0.418 g 0.576 g
Chemical reaction
2Mg(s) + O₂(g) ⇒ 2MgO(s)
Question 1.
Atomic mass of Mg = 24.31 x 2 = 48.62 g
Molecular mass of MgO = 2(24.31 + 16) = 80.62 g
Trial 1
48.62 g of Mg ----------------- 80.62 g of MgO
0.255 g ---------------- x
x = (0.255 x 80.62)/48.62
x = 0.422 g of MgO
Trial 2 48.62 g of Mg ----------------- 80.62 g of MgO
0.353 g ---------------- x
x = (0.353 x 80.62)/48.62
x = 0.585 g of MgO
Question 2
Trial 1
Percent yield = 0.418/0.422 x 100 = 99%
Trial 2
Percent yield = 0.576/0.585 x 100 = 98.5%
Question 3
Average = (99 + 98.5)/2
= 98.75%
Answer:
<em>Lower vapor pressures of a substance has an obvious effect on a</em> <em>boiling point</em>. <em>The</em> <em>freezing point </em><em>the rate at which the solid melts is equal to the rate which freezes. </em>
Explanation:
<em>In practice, small differences between these quantities can be observed. It is difficult, if not impossible, to heat a solid above its melting point because the heat </em>
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<em>Hope this helps (: </em>
Rain bc it’s hot then cools
Answer:
108.3kPa
Explanation:
Given parameters:
Initial temperature = 76k
Initial pressure = 78.4kPa
Final temperature = 105k
Unknown:
Final or new pressure = ?
Solution:
To solve this problem, we apply the combined gas law:
= 
T1 = 76k
P1 = 78.4kPa
T2 = 105k
= 
P2 = 108.3atm
