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3 years ago

Hhheeeeelllllppppppppp

Chemistry

2 answers:

babunello [35]3 years ago

6 0

Answers c. Thank me later

suter [353]3 years ago

4 0

Answer:

A gsjebdvxgjdkelsöeösldcj

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How much CO2 is produced from the combustion of a tank of propane C3H8? Assume the tank contains 9kgs of propane and the molecul

Zinaida [17]

<u>Answer:</u> The mass of carbon dioxide produced is 26.9 kg

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of propane = 9 kg = 9000 g (Conversion factor: 1 kg = 1000 g)

Molar mass of propane = 44.1 g/mol

Putting values in equation 1, we get:

$\text{Moles of propane}=\frac{9000g}{44.1g/mol}=204.08mol$

The chemical equation for the combustion of propane follows:

$C_3H_8+5O_2\rightarrow 3CO2+4H_2O$

By Stoichiometry of the reaction:

1 mole of propane produces 3 moles of carbon dioxide.

So, 204.08 moles of propane will produce = $\frac{3}{1}\times 204.08=612.24mol$ of carbon dioxide.

Now, calculating the mass of carbon dioxide by using equation 1, we get:

Molar mass of carbon dioxide = 44.01 g/mol

Moles of carbon dioxide = 612.24 moles

Putting values in equation 1, we get:

$612.24mol=\frac{\text{Mass of carbon dioxide}}{44.01g/mol}\\\\\text{Mass of carbon dioxide}=(612.24mol\times 44.01g/mol)=26944.7g=26.9kg$

Hence, the mass of carbon dioxide produced is 26.9 kg

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3 years ago

Help please! Chem is not fun! :(

ad-work [718]

I think the answer is c

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3 years ago

Directions: Match each of the following actions with the correct type of weathering (Mechanical or Chemical)

lozanna [386]

Answer:

1. D. Weathering by the actions of plants

2. C. Mechanical Weathering

3. A. Weathering by the actions of animals

4. B. Chemical Weathering

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3 years ago

Helppppppp it's due for tomorrow

jek_recluse [69]

C. the Fins of a fish , because of the branching out sort of structure

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3 years ago

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Calculate the mass of nitrogen dissolved at room temperature in an 89.0 LL home aquarium. Assume a total pressure of 1.0 atmatm

yaroslaw [1]

Answer : The mass of nitrogen dissolved is, 79.4 grams

Explanation :

The Raoult's law for liquid phase is:

$p_{N_2}=x_{N_2}\times p_T$

where,

$p_{N_2}$ = partial vapor pressure of nitrogen = ?

$p_T$ = total pressure = 1.0 atm

$x_{N_2}$ = mole fraction of nitrogen = 0.78

Now put all the given values in the above formula, we get:

$p_{N_2}=0.78\times 1.0atm$

$p_{N_2}=0.78atm$

Now we have to calculate the mass of nitrogen.

Using ideal gas equation:

$PV=nRT\\\\PV=\frac{w}{M}RT$

where,

P = pressure of gas = 0.78 atm

V = volume of gas = 89.0 L

T = temperature of gas = $25^oC=273+25=298K$

R = gas constant = 0.0821 L.atm/mole.K

w = mass of gas = ?

M = molar mass of nitrogen gas = 28 g/mole

Now put all the given values in the ideal gas equation, we get:

$(0.78atm)\times (89.0L)=\frac{w}{28g/mole}\times (0.0821L.atm/mole.K)\times (298K)$

$w=79.4g$

Therefore, the mass of nitrogen dissolved is, 79.4 grams

7 0

4 years ago