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lyudmila [28]
3 years ago
14

How many moles of H2O are produced when 64.0 g C2H2 burns in oxygen

Chemistry
1 answer:
Gnoma [55]3 years ago
6 0
The balanced chemical reaction will be: 

C2H2 + 5/2O2 = 2CO2 + H2O

We are given the amount of C2H2 being burned. This will be our starting point.

64.0 g C2H2 (1 mol C2H2 / 26.02 g C2H2) (1 mol H2O/1mol C2H2) ( 18.02 g H2O/1mol H2O) = 44.32 g H2O.

Thus, the answer is 44.32 g H2O.
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Answer:

60 dollars!

Explanation:

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Now, we can solve this by finding the value for only <u>one</u> orange, then multiplying that by 20 to get our answer!

So, the value of one orange is $36 / 12 = $3. One orange is worth $3 dollars.

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4 0
3 years ago
The vapor pressure of a substance is measured over a range of temperatures. A plot of the natural log of the vapor pressure vers
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28.7664 kJ /mol

Explanation:

The expression for Clausius-Clapeyron Equation is shown below as:

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Where,

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c is the constant.

The graph of ln P and 1/T gives a slope of - ΔHvap/ R and intercept of c.

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So,

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