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WITCHER [35]
3 years ago
12

The quantity of heat required to change the temperature of 1 g of a substance by 1°C is defined as ____.

Chemistry
1 answer:
Allushta [10]3 years ago
5 0

Answer:

specific heat

Explanation:

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10) A student’s calculation w as found to have a 15.6% error, and the actual value w as determined to be 25.7 mL. W hat are the
goblinko [34]

Answer:

The actual value = 25.7 ml

The error = 15.6%

This means that the value of error = 0.156 * 25.7 = 4.0092 ml

Now, the error percentage found means that the student got the value either greater than the actual one with the value of error or less than the actual one with the value of error.

This means that the two possible readings are:

either : 25.7 + 4.0092  = 29.7092 ml

or : 25.7 - 4.0092  = 21.6908 ml

Explanation:

7 0
3 years ago
1. What metal is oxidized in the most common dry cell?<br> zinc<br> iron<br> carbon<br> copper
GREYUIT [131]

Answer:

the correct answer is zinc

4 0
3 years ago
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A compound has been shown to contain 14.5 percent hydrogen and 85.5 percent carbon by mass.
Sedaia [141]

Answer:

  • <em>Option d. Its empirical formula is CH</em><em>₂</em><em>.</em>

Explanation:

The percent composition of the compound allow you to calculate the empirical formula of the compound but is not enough to calculate either the molar mass or the molecular formula. So, since now you can discard options b. and c.

Telling that it is a hydrocarbon (option e.) is true but very vague compared with finding the empirical formula. So, you can also discard the option e.

The fact that the product has a triple bond cannot be concluded from the percent composition, you should find the molecular formula to assert whether it contains or not a triple bond. So, you could discard option a., which lets you only with choice d.

Let us find the empirical formula to be certain that it is CH₂.

1.  <u>First, assume a basis of 100 g of compound</u>:

  • H: 14.5% × 100 g = 14.0 g
  • C: 85.5% × 100 g = 85.5 g

2. <u>Divide each element by its atomic mass to find number of moles</u>:

  • H: 14.0 g / 1.008 g/mol = 14.38 mol
  • C: 85.5 g / 12.011 g/mol = 7.12 mol

3. <u>Divide both amounts by the smallest number, to find the mole ratio</u>:

  • H: 14.38 mol / 7.12 mol ≈ 2
  • C: 7.12 mol / 7.12 mol = 1.

Hence, the ratio is 2:1 and the empirical formula is CH₂.

7 0
3 years ago
Can someone please help me with this?
Sergio039 [100]
Amu valie on the top and abundsnce percent in decimals on the bottom for each isotope

7 0
3 years ago
How many moles of water are in 1.23 x 10^18 water molecules?
TiliK225 [7]

<span>1.23x10^24 atoms/6.022x10^23 atom/mol = 2.04 mol H20 </span>
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3 years ago
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