Answer:
001: 71.2 g per ML
002: Consider a block of marble that occupies 287 cm3 and has a mass of 869 g.
a. What is its density?
d=m/v=869g/287 cm3=3.03 g/cm3
b. Will it float in:
H2O(l)? Why or why not?
Nope! Density > 1.00 g/mL
Hg(l) (density=13.55 g/mL)? Why or why not?
Yep! Density < 13.55 g/mL
003:
Use the given functions to set up and simplify
0.309 cm3
g/cm3=g/cm3
0.309cm3=g/cm3
Explanation:
http://childschemistry.weebly.com/uploads/7/8/6/3/78638416/density_key.pdf
Hope this helps I tried my best
Answer:
1. Testable
2. Testable
3. I’d say surfing (just my personal opinion)
4. Testable
Explanation:
I guessed
(3) The concen<span>tration of the solution remains constant.</span>
To answer this problem, we write first the stoichiometric equation. Thus we have,
Cu2S + O2 => 2Cu + SO2
Next, we check if the equation is balanced or not.
(left) (right)
2 Cu = 2 Cu
1 S = 1 S
2 O = 2 O
So the stoichiometric equation is balanced, let's proceed in solving the theoretical yield of Cu given 5 g of Cu2S.
First, we solve for Cu2S in moles,
5 g Cu2S x <u>1 mol Cu2S </u> = 0.0314 mol Cu2S
159.16 g Cu2s
Secondly, convert moles of Cu2S to moles Cu. Note for every mole of Cu2S we get 2 moles of Cu. Thus,
0.0314 mo Cu2S x <u> 2 mol Cu </u> = 0.0628 mole Cu<u>
</u> 1 mol Cu2S
Lastly, we convert mole Cu to g Cu via multiplying by Cu's MW.
0.0628 mole Cu x <u>63.546 g Cu </u> = 3.99 g Cu or 4 g Cu<u>
</u> 1 mole Cu
<em>ANSWER: 4 g Cu</em>
The substances largely ionic are:
NF3
N2
BrF3
PCl3