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BlackZzzverrR [31]
2 years ago
6

John and Alex were asked to make a 0.70 M solution. John measure out .35 L from the 2.0 M solution before asking how much soluti

on was needed. Alex remembered that measured out solutions are never put back in the stock bottle so went ahead and used all that was measured out. How many liters of the 0.70 M solution was made?
Chemistry
1 answer:
nasty-shy [4]2 years ago
3 0

Answer:

1.0 L

Explanation:

Given data

  • Initial volume (V₁): 0.35 L
  • Initial concentration (C₁): 2.0 M
  • Final volume (V₂): ?
  • Final concentration (C₂): 0.70 M

John and Alex prepared a diluted solution from a concentrated one. We can find the volume of the diluted solution using the dilution rule.

C₁ × V₁ = C₂ × V₂

V₂ = C₁ × V₁ / C₂

V₂ = 2.0 M × 0.35 L / 0.70 M

V₂ = 1.0 L

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A chemical change can be seen in how the molecular formulas of the products are different from the reactants, since the reactants have chemically changed into completely different molecules.

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What are two possible fates of stars larger than 8 sol
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3 years ago
Where do reactions in a solid generally take place?
Sholpan [36]

Answer:

It's D.  On the surface of the solid.

Explanation:

If the reactant is a solid, the surface area of the solid will impact how fast the reaction goes. This is because the two types of molecule can only bump into each other at the liquid solid interface, i.e. on the surface of the solid. So the larger the surface area of the solid, the faster the reaction will be.

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. Where does the corn get energy?
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3 years ago
Lighters are usually fueled by butane (c4h10). when 1 mole of butane burns at constant pressure, it produces 2658 kj of heat and
Leokris [45]

Answer:

ΔE = -2661 KJ/mole

ΔH = -2658 KJ/mole

Explanation:

ΔH = q - PΔV

ΔE = q + w

<u>First, to find ΔE:</u>

The reaction PRODUCES 2658 kJ of h (q), and does 3 kJ of work (w).

2658 kJ(q) + 3 kJ(w) = 2661 kJ, BUT the reaction <u><em>PRODUCES</em></u> heat, which means ΔE is negative.

ΔE = -2661 KJ/mole

<u>Second, to find ΔH:</u>

ΔH = q - PΔV

ΔH = 2658 kJ(q) - PΔV

Now, the question states that butane burns at a constant pressure; that just translates to the pressure of the reaction is equal to 0.

ΔH = 2658 KJ(q) - (0)ΔV

ΔH = 2658 KJ - 0

ΔH = 2658 kJ, BUT, like before, the reaction PRODUCES heat, which also mean ΔH is negative.

ΔH = -2658 KJ/mole

I hope this helped! Have a nice week.

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