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3 years ago

Does someone know the combustion in a jacket potato???

Chemistry

1 answer:

Leya [2.2K]3 years ago

7 0

Answer:

Some varieties of potato, such as Russet and King Edward, are more suitable for baking than others, owing to their size and consistency. Despite the popular misconception that potatoes are fattening, baked potatoes can be part of a healthy diet.[2]

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Help?

tino4ka555 [31]

Answer:

There is 52.33 grams of water produced.

Explanation:

Step 1: Data given

Mass of propane burned = 32.00 grams

Molar mass of propane = 44.1 g/mol

Oxygen is in excess

Molar mass of water = 18.02 g/mol

Step 2: The balanced equation

C3H8 + 5O2 → 4H2O + 3CO2

Step 3: Calculate moles of propane

Moles of propane = mass propane / molar mass of propane

Moles of propane = 32.00 grams / 44.1 g/mol

Moles of propane = 0.726 moles

Step 4: Calculate moles of H2O

Propane is the limiting reactant.

For 1 mol of propane consumed, we need 5 moles of O2 to produce 4 moles of H2O and 3 moles of CO2

For 0.726 moles of propane we'll have 4*0.726 = 2.904 moles of H2O

Step 5: Calculate mass of H2O

Mass of H2O = moles of H2O * molar mass of H2O

Mass of H2O = 2.904 moles * 18.02 g/mol

Mass of H2O = 52.33 grams

There is 52.33 grams of water produced.

3 0

3 years ago

An aqueous antifreeze solution is 60.0% ethylene glycol (HOCH2CH2OH) by mass and has a density of 1.06 g/mL. Calculate the molal

galina1969 [7]

Answer:

[HOCH₂CH₂OH] = 24.1 m

Explanation:

Ethylene glycol → HOCH₂CH₂OH

60% by mass means that 60 g of ethylene glycol are contained in 100 g of solution.

Solution mass = Solute mass + Solvent mass

100 g = 60 g + Solvent mass

Solvent mass = 40 g

Molality are the moles of solute contained in 1kg of solvent.

We determine the moles of solute → 60 g . 1mol/62 g = 0.967 moles

We convert the mass of solvent from g to kg → 40 g . 1kg/1000 g = 0.04 kg

Molality → 0.967 mol / 0.04 kg = 24.1 m

4 0

3 years ago

How many kilojoules is 1,500,000 calories

pochemuha

Answer:

1 cal = 0.004187 kJ

1,500,000 cal = 6280.5 kJ

5 0

3 years ago

If 150 g dimethylhydrazine reacts with excess dinitrogen tetroxide and the product gases are collected at 127oC in an evacuated

zhuklara [117]

Answer : The the partial pressure of the nitrogen gas is 0.981 atm.

The total pressure in the tank is 2.94 atm.

Explanation :

The balanced chemical reaction will be:

$(CH_3)_2N_2H_2(l)+2N_4O_4(l)\rightarrow 3N_2(g)+4H_2O(g)+2CO_2(g)$

First we have to calculate the moles of dimethylhydrazine.

Mass of dimethylhydrazine = 150 g

Molar mass of dimethylhydrazine =60.104 g/mole

$\text{Moles of dimethylhydrazine}=\frac{\text{Mass of dimethylhydrazine}}{\text{Molar mass of dimethylhydrazine}}$

$\text{Moles of dimethylhydrazine}=\frac{150g}{60.104g/mole}=2.49mole$

Now we have to calculate the moles of $N_2$ gas.

From the balanced chemical reaction we conclude that,

As, 1 mole of $(CH_3)_2N_2H_2$ react to give 3 moles of $N_2$ gas

So, 2.49 mole of $(CH_3)_2N_2H_2$ react to give $2.49\times 3=7.47$ moles of $N_2$ gas

Now we have to calculate the partial pressure of nitrogen gas.

Using ideal gas equation :

$PV=nRT\\\\P_{N_2}=\frac{nRT}{V}$

where,

P = Pressure of $N_2$ gas = ?

V = Volume of $N_2$ gas = 250 L

n = number of moles $N_2$ gas = 7.47 mole

R = Gas constant = $0.0821L.atm/mol.K$

T = Temperature of $N_2$ gas = $127^oC=273+127=400K$

Putting values in above equation, we get:

$P_{N_2}=\frac{(7.47mole)\times (0.0821L.atm/mol.K)\times 400K}{250L}=0.981atm$

Thus, the partial pressure of the nitrogen gas is 0.981 atm.

Now we have to calculate the total pressure in the tank.

Formula used :

$P_{N_2}=X_{N_2}\times P_T$

$P_T=\frac{1}{X_{N_2}}\times P_{N_2}$

$P_T=\frac{1}{(\frac{n_{N_2}}{n_T})}\times P_{N_2}$

$P_T=\frac{n_{T}}{n_{N_2}}\times P_{N_2}$

where,

$P_T$ = total pressure = ?

$P_{N_2}$ = partial pressure of nitrogen gas = 0.981 atm

$n_{N_2}$ = moles of nitrogen gas = 3 mole (from the reaction)

$n_{T}$ = total moles of gas = (3+4+2) = 9 mole (from the reaction)

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

$P_T=\frac{9mole}{3mole}\times 0.981atm=2.94atm$

Thus, the total pressure in the tank is 2.94 atm.

8 0

3 years ago

Which of these can be classified as a pure substance

Eduardwww [97]

Salt can be classified as a pure substance as it is only composed of sodium chloride
while contain many other substances

8 0

3 years ago

Read 2 more answers