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ASHA 777 [7]
3 years ago
7

Write a word equation for the overall reaction that occurred in the baggie. The reactants are sodium bicarbonate, carbon dioxide

, and water. Write a balanced equation for the overall reaction that occurred in the baggie.

Chemistry
1 answer:
Fynjy0 [20]3 years ago
6 0

Answer:

Explanation:

In a baggie, sodium bicarbonate is decomposed into sodium carbonate and carbondioxie and water is given off as gases:

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Two samples of carbon tetrachloride were decomposed into their constituent elements. One sample produced 32.4 g of carbon and 37
Gnoma [55]

Answer:

The answer to your question is:

Explanation:

Law of constant composition states that a given compound always contains its component elements in a fixed ratio.

Data

Sample 1   32.4 g of C and 373 g of Cl

Sample 2  12.3 g of C and 112 g of Cl

Convert the grams to moles and compare the ratios

Sample 1                                             Sample 2

          12 g of C --------------- 1 mol                        12 g of C --------------  1 mol

          32.4 g    ----------------  x                              12.3         -------------   x

          x = (32.4 x 1) / 12                                        x = (12.3 x 1) / 12

          x = 2.7 moles of C                                     x = 1.025 moles of C

          35.5 g of Cl ----------   1 mol                       35.5 g of Cl ----------  1 mol

          373 g  ------------------    x                             112 g of Cl   -----------  x

         x = (373 x 1) / 35.5                                       x = (112 x 1) / 35.5

         x = 10.5 moles of Cl                                    x = 3.15 moles of Cl

Ratio

        10.5 / 2.7 = 3.9                                             3.15/1.025 = 3.1

The ratio must be equal in both samples to say that the law is constant. So the answer is NO.

2.-

1) H3PO4                           3 hydrogens

2) Na2HPO4                     1 hydrogen

3) Ca(HCO3)2                   2 hydrogens

4) Ba(C2H3O2)2               6 hydrogens

                           

8 0
3 years ago
Methylhydrazine, CH6N2, is commonly used as a liquid rocket fuel. The heat of combustion of methylhydrazine is −1.30 × 103 kJ/mo
Step2247 [10]

Answer:

There is 5720 J of heat released.

Explanation:

Step 1: Data given

Molar mass of CH6N2 = 46.07 g/mol

The heat of combustion of methylhydrazine is −1.30 × 103 kJ/mol

Mass of methylhydrazine = 202.7 grams

Step 2: Calculate number of moles

Moles CH6N2 = mass of CH6N2 / Molar mass CH6N2

Moles CH6N2 = 202.7 grams / 46.07 g/mol

Moles CH6N2 = 4.4 moles

Step 3: Calculate heat released when 202.7 grams of CH6N2 is burned

q = 1300 J/mol * 4.4 moles

q = 5720 J

(Since there is heat released, ΔH = negative)

There is 5720 J released.

7 0
3 years ago
Gaseous ethane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . Supposed 0.301 g of methane
Nina [5.8K]

Answer:

The maximum mass of CO2 that could be produced is 0.1925 grams

Explanation:

Step 1: Data given

Mass of methane = 0.301 grams

Mass of oxygen = 0.28 grams

Molar mass of ethane = 16.04 g/mol

Molar mass of oxygen = 32 g/mol

Step 2: The balanced equation

CH4 + 2O2 → CO2 + 2H2O

For 1 mole methane consumed, we need 2 moles of O2 to produce 1 mole of CO2 and 2 moles of H2O

Step 3: Calculate moles of methane

Number of moles =Mass / Molar mass

Number of moles CH4 = 0.301 grams /16.04 g/mol

Moles CH4 = 0.0188 moles

Step 4: Calculate moles oxygen

Number of moles oxygen = 0.28 grams / 32 g/mol

Moles oxygen = 0.00875 moles

Step 5: the limiting reactant

For 1 mole methane consumed, we need 2 moles of O2

Oxygen is the limiting reactant. It will be completely consumed.

Methane is in excess. There will be consumed 0.00875 /2  = 0.004375 moles

There will remain 0.0188 - 0.004375 = 0.014425 moles

Step 6: Calculate moles of CO2

For 1 mole methane consumed, we need 2 moles of O2 to produce 1 mole of CO2

For 0.00875 moles oxygen , we have 0.004375 moles CO2

Step 7: Calculate mass of CO2

Mass CO2 = moles CO2 * Molar mass CO2

Mass CO2 =0.004375 * 44.01 g/mol = 0.1925 grams CO2

The maximum mass of CO2 that could be produced is 0.1925 grams

8 0
3 years ago
Turgor, an internal stimulus, refers to —
VladimirAG [237]

Answer:

which has a lower freeging point oxgyen or ethanol

6 0
3 years ago
Fuel cell cars that use hydrogen as fuel have the potential to be quiet, produce low emissions, and require less maintenance tha
Delvig [45]
Advocates for the use of hydrogen fuel cells posit that unlike other sources of power, these fuel cells do not emit harmful carbon emissions in the air that cause pollution and affect global warming. Although the chemical process involves burning hydrogen<span>, it emits water, heat and other emissions but not carbon.

I hope my answer has come to your help. God bless and have a nice day ahead!
</span>
4 0
3 years ago
Read 2 more answers
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