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riadik2000 [5.3K]
2 years ago
8

How many grams of water will I obtain from the combustion of 0.9249 mol of pentane (C5H12) in the following reaction?

Chemistry
2 answers:
pshichka [43]2 years ago
8 0

Answer:

C5H12 + 8 (O2) --> 5 (CO2) + 6 (H2O)

*Molar Ratio of Pentane and water is 1:6

*Number of mol of H2O = 0.9249 ×6 = 5.5494 mol

* Molar mass of H2O = 18 g/mol

* Mass of H2O needded = 5.5494 mol × 18 g/mol

= 99.8892 g

Explanation:

* By balancing the equation we can get the stiochemetry of the reaction (Molar Ratio).

* Then we can find the number of mol of H2O neede relative to the no. of mol of Pentane.

* Multiply the mol of H2O by the molar mass of H2O to get the mass.

VLD [36.1K]2 years ago
5 0

Answer: watch?v=zdAtYbCPSnA

Explanation:Should help

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Answer:

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<u>Answer:</u>

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<u>For B:</u> The K_c for the given reaction is 1642.

<u>Explanation:</u>

The given chemical reaction follows:

2NO(g)+Cl_2(g)\rightleftharpoons 2NOCl(g)

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The expression of K_p for the above reaction follows:

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We are given:

p_{NOCl}=0.24 atm\\p_{NO}=9.10\times 10^{-2}atm=0.0910atm\\p_{Cl_2}=0.174atm

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  • <u>For B:</u>

Relation of K_p with K_c is given by the formula:

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K_p = equilibrium constant in terms of partial pressure = 4.0\times 10^1

K_c = equilibrium constant in terms of concentration = ?

R = Gas constant = 0.0821\text{ L atm }mol^{-1}K^{-1}

T = temperature = 500 K

\Delta ng = change in number of moles of gas particles = n_{products}-n_{reactants}=2-3=-1

Putting values in above equation, we get:

4.0\times 10^1=K_c\times (0.0821\times 500)^{-1}\\\\K_c=\frac{4.0\times 10^1}{(0.0821\times 500)^{-1})}=1642

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