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Flauer [41]
3 years ago
8

The combustion of ethane (C2H6)(C2H6) produces carbon dioxide and steam. 2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(g) 2C2H6(g)+7O2(g)⟶4CO2(g)

+6H2O(g) How many moles of CO2CO2 are produced when 5.95 mol5.95 mol of ethane is burned in an excess of oxygen? moles of CO2:CO2:
Chemistry
1 answer:
Vera_Pavlovna [14]3 years ago
8 0

Answer:

11.9 moles of carbon-dioxide will produced.

Explanation:

Given moles of ethane = 5.95 mol

2C_2H_6(g)+7O_2(g)\rightarrow 4CO_2(g)+6H_2O(g)

According to reaction 2 moles of ethane produces 4 moles of carbon-dioxide.

Then, 5.95 moles of ethane will produce:

\frac{4}{2}\times 5.95 mol=11.9 mol of carbon-dioxide

11.9 moles of carbon-dioxide will produced.

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REY [17]

Answer:

volume = 0.288 L

Explanation:

To find the volume, you need to (1) convert grams LiBr to moles LiBr (via molar mass) and then (2) calculate volume (via molarity equation). It is important to arrange the ratios in a way tat allows for the cancellation of units (desired units in the numerator).

<u>(Step 1)</u>

Molar Mass (LiBr): 6.9410 g/mol + 79.904 g/mol

Molar Mass (LiBr): 86.845 g/mol

100 grams LiBr           1 mole
-----------------------  x  ------------------  =  1.15 moles LiBr
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<u>(Step 2)</u>

Molarity (M) = moles / volume (L)

4 M = 1.15 moles / volume

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3 0
2 years ago
What is the freezing point of a 0.743m aqueous solution if KCI? (Report amount to three decimal points)
Aleksandr-060686 [28]
This is a question about the colligative property known as freezing point depression. Freezing point depression (the amount the normal freezing point of the solvent is decreased) can be calculated with this equation:

ΔT = i Kf<span> m
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Here i = 2 (KCl dissociates into 2 ions, K+ and Cl-), Kf = 1.86 C/m (for water), and m = 0.743m).

ΔT = 2 x 1.86 C/m x 0.743m = <span>2.764C
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That means the freezing point of the solution is 2.764C less than the pure solvent (water), making it 0C - 2.764C = -2.764C.
5 0
3 years ago
Question 2
Mazyrski [523]

There is an increase in the frequency of particle collisions which leads to the increased rate of the reaction.

<u>Explanation:</u>

Hydrochloric acid reacts faster with the powdered zinc than with the equal mass of zinc strips.  

Since the surface area of the Zinc particle increases when it is powdered and has more active spots when compared to less number of active sites in Zinc strips and so the number of collision between the Zinc particles and the particles of Hydrochloric acid also increases and consequently the rate of the reaction also enhances.

So there is an increase in the frequency of particle collisions.

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3 years ago
What is the Celsius temperature of 1 mole of a gas that has an average kinetic energy of 4,265 joules?
algol [13]
96°C If I'm not mistaking
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What is the balanced equation for the complete combustion of pentane (C5H12)?
LekaFEV [45]
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=20+12
6 0
3 years ago
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