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yKpoI14uk [10]
4 years ago
6

This is anything with mass that occupies space.

Chemistry
2 answers:
FromTheMoon [43]4 years ago
5 0
the answer is matter
Leno4ka [110]4 years ago
5 0

The answer is matter because it takes up space

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4. Explain error and how it can impact your results from an experiment
Jet001 [13]

Random errors will shift each measurement from its true value by a random amount and in a random direction. These will affect reliability (since they're random) but may not affect the overall accuracy of a result.

3 0
3 years ago
A backpacker collects snow at 0°C, and places it in a cooking pot on a camp stove. It takes 643 kJ of heat energy to melt the sn
frutty [35]

Answer:

mass (m) of the snow that the backpacker collected= 0.855 kg

Explanation:

Given that:

Q = 643 kJ = 643000 J

ΔHfusion = 6.02 kJ/mol = 6020 J/mol

number of mole of water H2O = \frac{mass (m)}{18}

c = 4.18 J/g⋅K

ΔT = 100 K

Since there is a phase change from solid to liquid; then :

Q = Q_s + Q_l

ΔH = \frac{q}{mol}

However without the given mass; we substitute \frac{m}{18} for the number of moles; so:

Q = \delta H * \frac{m}{18} + m*c * \delta T

643000 =6020 * \frac{m}{18}+ m * 4.18 * 100

m = 855 g

m = 0.855 kg

mass (m) of the snow that the backpacker collected= 0.855 kg

8 0
3 years ago
Explain how the transfer of heat causes air to rise?
lisabon 2012 [21]

Answer:

Air in the atmosphere acts as a fluid. The sun's radiation strikes the ground, thus warming the rocks. As the rock's temperature rises due to conduction, heat energy is released into the atmosphere, forming a bubble of air which is warmer than the surrounding air. This bubble of air rises into the atmosphere.

Explanation:

I hope this helps and pls mark me brainliest :)

7 0
3 years ago
17. How many moles are there in a sample containing 1000 molecules of H2O?18. If you wanted a sample of H2O containing 6 x 23mol
Viefleur [7K]
17) mol of H_{2}O = \frac{no. of molecule}{L}
                            = \frac{1000  molecules}{6.03  *  10^{23}  molecules/mol }
                            = 1.658  *   10^{-21} mol

18) mol = \frac{molecule}{L}
      \frac{Mass}{Mr}  =   \frac{Molecule}{L}
      Let mass of oxygen = x
      \frac{x}{(2 * 1) + (16)}  =  \frac{6 * 10^{23} }{6.03 * 10^{23} }
      x =  (6 * 10^{23} ) (18 g/ mol)
             =  17.9 g
3 0
4 years ago
How do humans contribute to these excessive levels of phosphorus
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Get money all day and let em know we get cheese big dog, its big 5ive over here blood
5 0
3 years ago
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