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Ivahew [28]
3 years ago
10

determine the theoretical yield of the reacion below, if you started with 10 ml of the alcohol and 10 ml of 12 molar hcl g

Chemistry
1 answer:
Sonbull [250]3 years ago
6 0

Answer:

Hello there, the question asked is not complete (that is the reaction is not given) and similar Question could not be found. Hence, we will go with the information given above and make little assumptions.

Explanation:

So, from the the question above there is the need to determine the theoretical yield from the given starting materials that is 10 ml of the alcohol and 10 ml of 12 molar HCl g. So, let's say the alcohol given can be any alcohol Compound.

Thus, the equation showing the reaction is given as;

HCl + ROH =====> RCl + H20.

That's one mole of HCl react with alcohol to produce CH3Cl and water.

Let's assume that the HCl is the limiting reagent.

We have 10ml of 12M , thus the total number of moles = concentration × volume = 10mL × 12 = 0.01L × 12 = 0.12moles.

If 1 moles of RCl = 1 mole of HCl.

Then, y g/mol of RCl = 1 mol of RCl.

Thus, we have y (gram/mol) of RCl.

Therefore, the theoretical yield = .12 moles × y g/mol. = 0.12y grams.

SUMMARY: The theoretical yield is calculated by Determination of the mass in gram of the product through the use of limiting reagent.

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Answer:

Explanation:

mass of the reactant = mass of the product

15.31 + 1.50 = 16.81g

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3 years ago
Un átomo X posee 29 protones y de carga +2 ¿Cuántos electrones tiene?
lesya [120]

Responder:

27

Explicación:

Dado que:

Número de protones en el átomo X = 29

Carga en el átomo X = +2

Si no hay cargo neto;

número de protones = número de electrones

Sin embargo, dado que el átomo X tiene una carga de +2 (dando 2 electrones).

Por lo tanto,

Número de electrones = número de protones - número de carga en el átomo)

Número de electrones = (29 - 2) = 27

4 0
3 years ago
What is the MOLAR heat of combustion of methane(CH₄) if 64.00g of methane are burned to heat 75.0 ml of water from 25.00°C to 95
melamori03 [73]

Answer:

-5.51 kJ/mol

Explanation:

Step 1: Calculate the heat required to heat the water.

We use the following expression.

Q = c \times m \times \Delta T

where,

  • c: specific heat capacity
  • m: mass
  • ΔT: change in the temperature

The average density of water is 1 g/mL, so 75.0 mL ≅ 75.0 g.

Q = 4.184J/g.\°C \times 75.0g \times (95.00\°C - 25.00\°C) = 2.20 \times 10^{3} J = 2.20 kJ

Step 2: Calculate the heat released by the methane

According to the law of conservation of energy, the sum of the heat released by the combustion of methane (Qc) and the heat absorbed by the water (Qw) is zero

Qc + Qw = 0

Qc = -Qw = -22.0 kJ

Step 3: Calculate the molar heat of combustion of methane.

The molar mass of methane is 16.04 g/mol. We use this data to find the molar heat of combustion of methane, considering that 22.0 kJ are released by the combustion of 64.00 g of methane.

\frac{-22.0kJ}{64.00g} \times \frac{16.04g}{mol} = -5.51 kJ/mol

8 0
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patriot [66]

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Explanation:

The balanced chemical reaction for decomposition of ammonium perchlorate is:

2NH_4ClO_4\rightarrow N_2+Cl_2+2O_2+4H_2O  

According to stoichiometry :

2 moles of NH_4ClO_4 produce = 2 moles of O_2

Thus 0.055 moles of NH_4ClO_4 will produce =\frac{2}{2}\times 0.055=0.055moles of O_2

Thus 0.055 moles of O_2 are produced by the reaction of 0.055mol of ammonium perchlorate.

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