Answer:
The given metal sample is not aluminum because its density is 3.0 g/cm³ while density of aluminum is 2.7 g/cm³.
Explanation:
Given data:
Density of aluminum = 2.7 g/cm³
Mass of metal sample = 52.0 g
Volume of metal sample = 17.1 cm³
which sample is that = ?
Solution:
The given problem will be solve through density formula.
d = m/v
d = density
m = mass
v= volume
Now we will put the values in formula.
d = 52.0 g/ 17.1 cm³
d = 3.0 g/cm³
It is given in question the density of aluminum is 2.7 g/cm³. The given metal sample is not aluminum because its density is 3.0 g/cm³.
Answer: What best describes the reaction is "A single replacement reaction takes place because zinc is more reactive than hydrogen."
Using Hess' Law, we can calculate the heat of reaction of the gasification of coal. Multiplying the second reaction by 2 and reversing the third reaction:
<span>C(s) + O2(g) → CO2(g) ∆H=-394 kj
2H2(s) + O2(g) → H2O(l) ∆H=-572kj
</span>CO2(g) + 2H2O(l) → CH4(g) + 2O2(g) ∆H=891kj
Adding the three reaction would result to
<span>C(s) + 2H2(g) → CH4(g) ∆H = -394 + -572 + 891 = -75 kJ
The answer is
</span><span>(B) -75 kJ
</span>
Answer:
Kindly check the attached picture for the diagram of the chemical compound.
Explanation:
So, the following parameters were given from the question above;
=> A triplet at 0.9 ppm and a quartet at 1.4 ppm, a singlet at 1.35 ppm. Now, the unknown compound has a molecular formula of C7H16O.
For a triplet at 0.9ppm, there are nine (9) atoms of hydrogen, for the quartet at 1.4ppm there are six(6) atoms of hydrogen and for the singlet at 1.35 ppm, the number of hydrogen atoms is one(1). Hence, the total number of hydrogen atoms = 16.
Therefore, number of bondings = [(2 × number of carbon atoms) + 2 - number of hydrogen atoms present on the compound)/2 .
Thus number of bonds =[( 2× 7) + 2 - 16] ÷ 2 = 0.
Hence, there is no double bond or ring in the compound.
Answer:
long
Explanation:
Uranus has a tilt, causing seasons, and they are each 21 earth years long.
