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Usimov [2.4K]
3 years ago
13

Which of the following is an example of a homogeneous mixture?

Chemistry
1 answer:
elena-s [515]3 years ago
7 0

A. Apple juice is an example of a homogeneous mixture.

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Which alkaline earth metal is a component of gypsum​
Allisa [31]

Answer:

calcium is the correct answer :)

4 0
3 years ago
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ASAP please and thankyou<br><br>Options:<br>pollen<br>pistil<br>purple<br>white​
AURORKA [14]

Answer:

pistil

Explanation:

5 0
3 years ago
Identify the type of reaction described in the sentence below. then, write a chemical equation. be sure to specify the states of
natulia [17]

Answer : The type of reaction described in the sentence is Synthesis or Combination

Explanation :

The balanced equation for the reaction between Phosphorous and Oxygen gas can be written as

4P (s) + 5O_{2} (g) ------>  P_{4} O_{10}  (s)

From the above equation we can see that there are two different reactants ( P and O₂ ) which are combining with each other to give a single product.

This type of reaction is known as Combination or Synthesis.

A general form of Synthesis reaction is given below.

A + B ---->  AB

Here we can conclude that a synthesis / combination reaction is the one where 2 or more reactants combine together to give only one product .

6 0
3 years ago
If 0.0692 mol CaCl2 is dissolved in water to make a 0.810 M solution, what is the volume of the solution?
Natali5045456 [20]

Answer:

Just ask google for help

Explanation:

I always do it and get it right

8 0
3 years ago
Arizona was the site of a 400,000-acre wildfire in June 2002. How much carbon dioxide (CO2) was produced into the atmosphere by
kodGreya [7K]

Answer:

2.97 × 10¹³ g

Explanation:

First, we have to calculate the biomass the is burned. We can establish the following relations:

  • 2.47 acre = 10,000 m²
  • 10 kg of C occupy an area of 1 m²
  • 50% of the biomass is burned

The biomass burned in the site of 400,000 acre is:

400,000acre\times\frac{10,000m^{2} }{2.47acre} \times \frac{10kgC}{m^{2} } \times 50\% = 8.10 \times 10^{9} kgC

Let's consider the combustion of carbon.

C(s) + O₂(g) ⇒ CO₂(g)

We can establish the following relations:

  • The molar mass of C is 12.01 g/mol
  • 1 mole of C produces 1 mole of CO₂
  • The molar mass of CO₂ is 44.01 g/mol

The mass of  produced is CO₂:

8.10 \times 10^{12}gC \times \frac{1molC}{12.01gC} \times \frac{1molCO_{2}}{1molC} \times \frac{44.01gCO_{2}}{1molCO_{2}} =2.97 \times 10^{13} gCO_{2}

4 0
3 years ago
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