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netineya [11]
2 years ago
11

Student Exploration: Limiting Reactants Vocabulary: chemical equation, chemical formula, chemical reaction, coefficient, limitin

g reactant, molecule, product, reactant, subscript Prior Knowledge Questions (Do these BEFORE using the Gizmo.) Imagine you and your friends are making hot dogs. A complete hot dog consists of a wiener and a bun. At the store, you buy four packages of eight wieners and three bags of 10 buns. 1. How many total hot dogs can you make
Chemistry
1 answer:
SIZIF [17.4K]2 years ago
6 0

Answer:

30 hot dogs

Explanation:

It is given that :

There are 4 packets of eight wieners, i.e. 4 x 8 = 32 wieners

There are 3 bags of ten buns, i.e. 3 x 10 = 30 buns

One hot dogs need 1 bun and 1 wiener to make a hot dog.

There are 30 buns, so 30 hot dogs can be made out by using all the 30 buns and the 30 wieners out of the 32 wieners.

Therefore, 30 hot dogs.

And the number of extra wieners left = 32 - 30 = 2 wieners.

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Please help!! 20 points!! Posted this previously and forgot to change it to 20 points but it is now
spayn [35]

Answer:

0.571 mol

Explanation:

Given data:

Number of moles of NaHCO₃ = 0.571 mol

Number of moles of CO₂ produced = ?

Solution:

Chemical equation:

NaHCO₃ + C₃H₆O₃   →     CO₂  + C₃H₅NaO₃ + H₂O

Now we will compare the moles of CO₂ with NaHCO₃ from balance chemical equation.

                             NaHCO₃          :            CO₂

                                    1                :               1

                                 0.571            :            0.571

So number of moles of CO₂  produced are 0.571.

3 0
3 years ago
Read 2 more answers
Find the number of moles of butane (c4h10) in 21g sample of butane gas​
iogann1982 [59]

Answer:

0.362 moles

Explanation:

Mass of butane = 21g

Molar mass of carbon = 12g / mol

Molar mass of hydrogen = 1g/mol

Molar mass of butane ? = [(12*4) * (1*10)]

Molar mass of butane = 58g / mole

Number of moles = mass of molecules / molar mass of molecule

Number of moles = 21 / 58

Number of moles of butane = 0.362 moles

The number of moles in 21g of butane is 0.362 moles

8 0
3 years ago
A 17.11 gram sample of an organic compound containing only C, H, and O is analyzed by combustion analysis and 21.71 g CO2 and 5.
Andru [333]

Answer:  The empirical formula and the molecular formula of the organic compound is CHO and C_4H_4O_4 respectively.

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

C_xH_yO_z+O_2\rightarrow CO_2+H_2O

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and oxygen respectively.

We are given:

Mass of CO_2 = 21.71 g

Mass of H_2O= 5.926 g

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 21.71 g of carbon dioxide, =\frac{12}{44}\times 21.71=5.921g of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 5.926 g of water, =\frac{2}{18}\times 5.926=0.658g of hydrogen will be contained.

Mass of oxygen in the compound = (17.11) - (5.921+0.658) = 10.53  g

Mass of C = 5.921 g

Mass of H = 0.658 g

Mass of O = 10.53 g

Step 1 : convert given masses into moles.

Moles of C =\frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{5.921g}{12g/mole}=0.493moles

Moles of H=\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.658g}{1g/mole}=0.658moles

Mass of O=\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{10.53g}{16g/mole}=0.658moles

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C =\frac{0.493}{0.493}=1

For H =\frac{0.658}{0.493}=1

For O=\frac{0.658}{0.493}=1

The ratio of C : H: O =  1: 1: 1

Hence the empirical formula is CHO.

empirical mass of CHO = 12(1) + 1(1) + 1 (16) = 29

Molecular mass = 104.1 g/mol

n=\frac{\text {Molecular mass}}{\text {Equivalent mass}}=\frac{104.1}{29}=4

Thus molecular formula = n\times {\text {Empirical formula}}=4\times CHO=C_4H_4O_4

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2 years ago
How many Sig figs does 3.0050?
Novay_Z [31]
5 sig figs

Trailing zeroes always count as a sig fig if there is a decimal point
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3 years ago
Does anyone know any top brainly users that are good at chemistry?
Law Incorporation [45]

Answer:

yes

Explanation:

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2 years ago
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