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GalinKa [24]
3 years ago
8

all of the rocks (A) are removed from a desert ecosystem, what would happen to the population of the rock dwelling lizards (B) a

nd in turn the animals which eat them? (B)- Biotic (A)-abiotic
Chemistry
1 answer:
lbvjy [14]3 years ago
5 0
The rock dwelling lizards would lose their hiding/refuge places from other prey and also for shade from the intense sun so their prey would be able to capture them easily which could result in over eating  of them and then their decimation and resultant loss of sustainable food for the prey thus resulting in dying off of the prey as well or migration to other areas where the rocks still existed and the lizards.
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Given 2AL + 6HCL → 2ALCL3 + 3H2, how many grams of aluminum do I need to produce 11 L of hydrogen gas at STP?
Setler79 [48]

Mass of Aluminum= 8.829 g

<h3>Further explanation</h3>

Given

Reaction

2Al + 6HCl → 2AlCl₃ + 3H₂

Required

mass of Aluminum

Solution

At STP, 1 mol gas = 22.4 L

For 11 L of Hydrogen :

= 11 : 22.4

= 0.491

From equation, mol ratio Al : H₂ = 2 : 3, so mol Al :

= 2/3 x mol H₂

= 2/3 x 0.491

= 0.327

Mass Aluminum(Ar=27 g/mol) :

= 0.327 mol x 27 g/mol

= 8.829 g

3 0
3 years ago
The image above shows a type of metamorphic rock called gneiss. Gneiss is characterized by alternating bands of light and dark m
finlep [7]

Answer: first blank is heating second blank is pressure i think but i know that its NOT freezing

Explanation:

I did it and got it right

4 0
3 years ago
Calculate the energy (in kJ) required to heat 10.1 g of liquid water from 55 oC to 100 oC and change it to steam at 100 oC. The
Maksim231197 [3]

Answer:

           \large\boxed{\large\boxed{24.6kJ}}

Explanation:

<u>1. Energy to heat the liquid water from 55ºC to 100ºC</u>

     Q=m\times C\times \Delta T

  • m = 10.1g
  • C = 4.18g/JºC
  • ΔT = 100ºC - 55ºC = 45ºC

     Q=10.1g\times 4.18J/g\ºC\times 45\ºC=1,899.81J

<u>2. Energy to change the liquid to steam at 100ºC</u>

      L=\lambda \times n

  • λ = 40.6kJ/mol
  • n = 10.1g / 18.015g/mol = 0.5606mol

      L=40.6kJ/mol\times 0.5604mol=22.76214kJ=22,762.14J

<u>3. Total energy</u>

       1,899.81J+22,762.14J=24,661.95J\approx24,662J\approx24.6kJ

7 0
3 years ago
Assuming it behaves as an ideal gas, calculate the density of sulfur dioxide, so2, at stp.
Arisa [49]
Hello!

At Standard Pressure and Temperature, an ideal gas has a molar density of  0,04464 mol/L.

So, we need to apply a simple conversion factor to calculate the density of Sulfur Dioxide using the molar mass of Sulfur Dioxide.

\frac{0,04464 mol SO_2}{1 L SO_2}* \frac{64,066 g SO_2}{1 mol SO_2}=2,8599 g/L

So, the Density of Sulfur Dioxide (SO₂) at STP is 2,8599 g/L

Have a nice day!


6 0
3 years ago
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Pls this need this I am doing a test and I need to get this
Alexxx [7]

Answer:

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Explanation:

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6 0
3 years ago
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