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____ [38]
3 years ago
9

if a 2.0g sample of water at 5.0celcius absorbs 21.8Joules of energy, the temprature of the sample will be raised by

Chemistry
1 answer:
Cerrena [4.2K]3 years ago
8 0
You'd use the temperature change equation. The specific heat of water is always 4.18J/(g °C).
Equation to use: q=mCΔT

21.8=(2.0)(4.18)(Tf-5)
21.8=(8.36)(Tf-5)
21.8/8.36=Tf-5
2.61=Tf-5
2.61+5=Tf
Tf=7.61 °C

Since you want to know how many °C it raises, you wouldn't pay attention to the last 2 steps, however if you need to know the final temp, you want to go to the last step.
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1.For the first ten reactions, write a balanced reaction for each tube in which a reaction occurred. If there was no reaction, w
slamgirl [31]

The equations of reaction occurring in the tubes are as follows:

  • 2 MnO₄⁻ + 6 Br⁻ + 8 H⁺ → 2 MnO₂ + 3 Br₂ + 4 H₂O
  • 2 MnO₄⁻ + 6 I⁻ + 8 H⁺ → 2 MnO₂ + 3 I₂ + 4 H₂O
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<h3>What are the reactions occurring in the tubes?</h3>

The reactions occurring in the tubes are redox reactions.

Based on the table the equations of reaction are as follows:

  • 2 MnO₄⁻ + 6 Br⁻ + 8 H⁺ → 2 MnO₂ + 3 Br₂ + 4 H₂O
  • 2 MnO₄⁻ + 6 I⁻ + 8 H⁺ → 2 MnO₂ + 3 I₂ + 4 H₂O
  • No reaction
  • 2 Fe³⁺ + 2 I⁻ → 2 Fe²⁺ + I₂

In conclusion, redox reaction are reactions in which electrons are transferred.

Learn more about redox reactions at: brainly.com/question/26750732

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6 0
2 years ago
Match each decimal number to the correct scientific notation.
Effectus [21]

3.07 × 10^4=30,700

3.07 × 10^-4=0.000307

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5 0
3 years ago
Read 2 more answers
2Al + 6HCl → 2AlCl3 + 3H2<br> If 85.0 grams of HCl react, how many moles of H2 are produced?
Murrr4er [49]

Answer:

1.17 mol

Explanation:

Step 1: Write the balanced equation

2 Al + 6 HCl → 2 AlCl₃ + 3 H₂

Step 2: Calculate the moles corresponding to 85.0 g of HCl

The molar mass of HCl is 36.46 g/mol.

85.0 g × 1 mol/36.46 g = 2.33 mol

Step 3: Calculate the number of moles of H₂ produced from 2.33 moles of HCl

The molar ratio of HCl to H₂ is 6:3.

2.33 mol HCl × 3 mol H₂/6 mol H₂ = 1.17 mol H₂

8 0
2 years ago
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