Answer:
A. wool, silkworm, cocoon, and cellulose
Explanation:
I hope this helped!
718.65 degrees is the initial temperature of the zinc metal sample.
Explanation:
Data given:
mass of zinc sample = 2.50 grams
mass of water = 65 grams
initial temperature of water = 20 degrees
final temperature of water = 22.5 degrees
ΔT = change in temperature of water is 2.50 degrees
specific heat capacity of zinc cp= 0.390 J/g°C
initial temperature of zinc sample = ?
cp of water = 4.186 J/g°C
heat absorbed = heat released (no heat loss)
formula used is
q = mcΔT
q water = 65 x 4.286 x 2.5
q water = 696.15 J
q zinc = 2.50 x 0.390 x (22.50- Ti)
equating the two equations
696.15 = - 22.50+ Ti
Ti = 718.65 degrees is the initial temperature of zinc.
<span>Molar mass(C)= 12.0 g/mol
Molar mass (O2)=2*16.0=32.0 g/mol
Molar mass (CO2)=44.0 g/mol
18g C*1mol C/12 g C = 1.5 mol C
C + O2 → CO2
from reaction 1 mol 1 mol 1 mol
from problem 1.5 mol 1.5 mol 1.5 mol
1.5 mol O2*32 g O2/1 mol O2 = 48 g O2
In reality this reaction requires only 48 g O2 for 18 g carbon.
And from 18 g carbon you can get only
1.5 mol CO2*44 g CO2/1 mol CO2=66 g CO2
But these problem has 72g CO2. The best that we can think, it is a mix of CO2 and O2.
So to find all amount of O2 that was added for the reaction (probably people who wrote this problem wanted this)
we need (the mix of 72g - mass of carbon 18 g)= 54 g.
So the only answer that is possible is </span><span>2.) 54 g.</span>
Volume:
2.00 x 11.0 x 11.0 => 242 cm³
mass : 213 g
D = m / V
D = 213 / 242
D = 0.880 g/cm³
Answer B
hope this helps!
