Chemistry College

Based on the procedure, which of the following are reasonable sources of errors in determining heat lost or gained? One or more answers are correct and you will receive negative points for incorrect answers. Group of answer choices The cap of the calorimeter was not closed immediately after mixing. The final temperature was measured before the temperature stopped changing. Temperatures were not measured right before mixing. Volumes of solutions were not measured accurately.

Answers

Answer 1

Answer:

The possible source of errors as regard the Procedure are:

The final temperature was measured before the temperature stopped changing The cap of the calorimeter was not closed immediately after mixing temperatures where not measured right before mixing

Explanation:

The procedure referred to should a experiment with regards heat

The possible source of errors as regards the Procedure are:

The final temperature was measured before the temperature stopped changing The cap of the calorimeter was not closed immediately after mixing temperatures where not measured right before mixing

Related Questions

Explain why water and syrup are able to mix?​

Answers

you can’t because the water would rise and the syrup consistency would not mix

Which of the following compounds is the most stable?​

Answers

Answer:

Hey mate......

Explanation:

This is ur answer......

fluorides

Thus, fluorides are the most stable while iodides are the least stable.

Hope it helps!

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Answer:

LICI

Explanation:

a p e x :)

To determine the concentration of a sodium thiosulfate solution as in this experiment, a student pipetted 25.0 mL of 0.0100 M potassium iodate (KIO3) solution into a 125 mL Erlernmeyer flask. Potassium iodide and sulfuric acid were added as in this experiment. The titration needed 15.21 mL of the sodium thiosulfate to reach the end point. What is the concentration of the sodium thiosulfate solution

Answers

Answer:

0.0986M is the concentration of the Na₂S₂O₃ solution

Explanation:

Potassium iodate, KIO₃, reacts with sodium thiosulfate, Na₂S₂O₃, as follows:

KIO₃ + 6Na₂S₂O₃ +5KI + 3H₂SO₄ → 3H₂O + 3K₂SO₄ + 3Na₂S₄O₆ + 6NaI

To solve this question we must find the moles of sodium thiosulfate that reacts as follows:

Moles KIO₃:

0.0250L * (0.0100mol / L) = 2.5x10⁻⁴moles KIO₃

Moles Na₂S₂O₃:

2.5x10⁻⁴moles KIO₃ * (6mol Na₂S₂O₃ / 1mol KIO₃) = 1.5x10⁻³ moles Na₂S₂O₃

Molar concentration:

1.5x10⁻³ moles Na₂S₂O₃ / 0.01521L =

0.0986M is the concentration of the Na₂S₂O₃ solution
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