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NeTakaya
3 years ago
5

A student places a beaker on a hot plate. To the beaker, he adds a clear liquid and a white powder. The mixture instantly begins

to bubble. He concludes that a chemical reaction has occurred. Do you agree with his conclusion? Why or why not? Please explain.
Chemistry
2 answers:
Elenna [48]3 years ago
7 0
True, because if it wasn't a chemical reaction it would have proceeded to stay the same. but it begins to bubble.
sorry if this isn't the best answer I'm trying my best.
emmainna [20.7K]3 years ago
7 0
Yes, the bubbling of the solution means a gas is being created, which is proof of a chemical reaction
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5. A penny weighs about 2.5 g. How many moles of pennies would be required to equal the mass of the moon (7.3x10^24 kg)
schepotkina [342]

5. 1.16 x 10^{26} moles  moles of pennies would be required to equal the mass of the moon.

6. 12.86 moles of ethanol are in a 750 ml bottle of vodka.

Explanation:

5 .Data given:

mass of penny = 2.5 grams

atomic mass of penny = 62.93 grams/mole

moles present in mass of the moon given as = 7.3 x 10^{24} kg

number of moles = \frac{mass}{atomic mass of  1 mole}

number of moles = \frac{2.5}{62.93}

0.039 moles of penny is present in 2.5 grams

0.039 moles of penny in 2.5 grams of it

so, x moles in 7.3 X 10^{27}  grams

\frac{0.039}{2.5} =\frac{x}{7.3 X 10^{27} }

x = 1.16 x 10^{26} moles

so when the mass of the penny given is equal to the mass of moon, number of moles of penny present is 1.1 x 10^{26} .

6.

Given:

vodka = 40% ethanol

volume of vodka bottle = 750 ml

moles of ethanol =?

density of ethanol =0.79 g/ml

atomic mass of ethanol = 46.07 grams/mole

so, from the density of ethanol given we can calculate how much ethanol is present in the solution.

density = \frac{mass}{volume}

density x volume = mass

0.79 x 750 = 592.5 grams

number of moles = \frac{mass}{atomic mass of 1 mole}

number of moles of ethanol = \frac{592.5}{46.07}

                                               = 12.86 moles of ethanol

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Butane, C4H10, reacts with oxygen, O2, to form water, H2O, and carbon dioxide, CO2, as shown in the following chemical equation:
Wittaler [7]
The balanced chemical reaction is:

<span>2C4H10(g)+13O2(g)->10H2O(g)+8CO2(g) 
</span>
<span>Calculate the mass of water produced when 1.77 grams of butane reacts with excessive oxygen?
</span>1.77 g C4H10 (1 mol C4H10/58.14 g C4H10) (10 mol H2O / 2 mol C4H10) ( 1.01 g H2O / 1 mol H2O ) = <span>0.15 g H2O

</span><span>Calculate the mass of butane needed to produce 71.6 of carbon dioxide.
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4 0
3 years ago
Read 2 more answers
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