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2 years ago

A 0.500 g sample of tin (Sn) is reacted with oxygen to give 0.534 g of product. What is the empirical formula of the oxide?

Chemistry

1 answer:

larisa [96]2 years ago

5 0

Answer:

$Sn_2O$

Explanation:

Hello,

In this case, given the mass of the sample and mass of tin we can compute the mass of oxygen via:

$m_O=0.534g-0.500g=0.034g$

Thus, by using the atomic bas of tin and oxygen we can compute their moles:

$n_{Sn}=0.500gSn*\frac{1molSn}{118.8gSn} =0.00421mol\\\\n_O=0.034gO*\frac{1molO}{16gO}=0.002125mol$

Next, we need to divide both moles by the moles of oxygen as those are the smallest in order to compute the subscript in the chemical reaction:

$Sn=\frac{0.00421}{0.002125}=2\\ \\O=\frac{0.002125}{0.002125}= 1$

Therefore, empirical formula of the oxide should be:

$Sn_2O$

Best regards.

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Which reactions performed in the experiment involved chemical changes? crushing calcium carbonate mixing calcium carbonate and h

lisov135 [29]

Mixing calcium carbonate and HCl.
Heating copper sulfate pentahydrate.
Mixing potassium iodide and lead nitrate.
Combining magnesium and hcl.
Burning the candle.
Let's look at the available options and see what are chemical changes and what are physical changes. As a side note, line breaks, capitalization, and punctuation are VERY important. I spent almost as much time attempting to actually figure out what your options were as I spent in distinguishing between what were chemical reactions and physical changes.
Crushing calcium carbonate.
* This is a mere physical change. You start with large pieces of calcium carbonate and end up with smaller pieces. So this is a bad choice.
Mixing calcium carbonate and HCl.
* This is a chemical reaction where the calcium carbonate and hydrochloric acid react with each other and produce carbon dioxide plus other compounds. So this is a good choice.
Boiling water.
* Another physical change from liquid to vapor. You can cool down the resulting vapor and end up with the original water. So this is a bad choice.
Heating copper sulfate pentahydrate.
* This is a chemical change in that you're converting CuSO4 . 5H2O(s) into CuSO4 and H2O. So this too is a good choice.
Separating iron filing and sulfur.
* You start out with iron filings and sulfur and end up with iron filings and sulfur. Things are a bit more orderly, but no chemical reactions have occurred. So this is a bad choice.
Mixing potassium iodide and lead nitrate. * You start with 2 white solids and upon mixing them, you get a yellow solid.
A chemical reaction has occurred. So this is a good choice.

Combining magnesium and hcl.
* When you combine these two items, you get hydrogen gas as a product. So you have a chemical reaction. And this is a good choice.
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5 0

2 years ago

Read 2 more answers

An aspirin tablet contains 325.0 mg of aspirin, which has the molecular formula, C9H8O4. How many molecules of aspirin are in th

Inga [223]

Answer:

1.08X10²¹ molecules aspirin are in the tablet

Explanation:

Molar mass of aspirin is 180.15 g/m (C₉H₈O₄)

This data means that 1 mol weighs 180.15 g so:

325 mg = 0.325 g

If 180.15 g are contained in 1 mol of aspirin

0.325 g (which is the weight from the tablet) are contained in ...

(0.325 g .1m)/180.15 g = 1.80x10⁻³ moles

1 mol has 6.02x10²³ molecules (NA)

1.80x10⁻³ moles are contained by ...

1.80x10⁻³ . NA = 1.08X10²¹ molecules

6 0

2 years ago

A solution was prepared by dissolving 200.0 g of KCI in 215 g of water.

Archy [21]

Answer:mole fraction of KCl = 0.18

Explanation:

no of moles of KCl = Mass/Molar mass

where mass (weight) of KCl = 200.0g

molar mass of KC1= 74.6g/mol

= 200/74.6 = 2.68 moles

no of moles of H2O = Mass/Molar mass

where mass (weight) of water = 215.0g

molar mass of water = 18.0g/mol

= 215/18 = 11.94moles

mole fraction of KCl = no of moles of KCl/(no of moles KCl + no of moles of H2O(water))

= 2.68/(2.68+ 11.94)

= 2.68/14.62 = 0.18

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2 years ago

What is the theoretical yield of C6H5Br if 42.1 g of C6H6 react with 73.0 g of Br2?

Norma-Jean [14]

1) Chemical reaction

C6H6 + Br2 ---> C6H5Br + HBr

2) Molar raios

1 mol C6H6 : 1 mol Br2 : 1 mol C6H5Br

3) Convert the data to moles

42.1 g of C6H6

molar mass of C6H6 = 6*12g/mol + 6*1g/mol = 78 g/mol

42.1 g / 78 g/mol = 0.54 mol

73.0 g of Br2

molar mass of Br2 = 2 * 79.9 g/mol = 159.8 g/mol

73.0 g / 159.8 g/mol = 0.46 mol of Br2

=> limiting reagent is the Br2.

4) Product

1 mol of Br2 (limiting reagent) yields 1 mole of C6H5Br, then you will obtain 0.46 mol of C6H5Br

5) Convert the product to grams

molar mass of C6H5Br = 6*12g/mol + 5*1g/mol + 79.9 g/mol = 156.9 g/mol

0.46mol*156.9g/mol = 72.2 g.

Answer: 72.2 g

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2 years ago

Butyl butyrate is an ester that is a naturally occurring oil used in the flavor industry for its fruity scent. If the steam dist

Snezhnost [94]

Answer:

The correct answer is 62.5 %.

Explanation:

Based on the given information, the partial pressure of butyl butyrate is 50 mmHg and the partial pressure of water is 710 mmHg.

Hence, the total pressure is 710+50 = 760 mmHg

According to Dalton's law of partial pressure,

Partial pressure = mole fraction * total pressure

Mole fraction of water is,

Partial pressure of water/Total pressure = 710/760 = 0.93

Similarly, the mole fraction of butyl butyrate is,

Partial pressure of butyl-butyrate/Total pressure = 50/760 = 0.07

Therefore, mole% of water is 0.93 * 100 = 93 %

For calculating mass%,

Mass of H2O = 0.93 * 18 = 16.8 grams (The molecular mass of water is 18 grams per mole)

The molecular mass of butyl-butyrate is 144 gram per mole

The mass of butyl-butyrate = 144 * 0.07 = 10.08 grams

The mass percent of water will be,

Mass % of water/Total mass % * 100 = 16.8 / 10.08 + 16.8 * 100 = 62.5%.

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2 years ago