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aliina [53]
2 years ago
8

How many moles of NH3 are there in 77.5 g of NH3?

Chemistry
1 answer:
Vanyuwa [196]2 years ago
4 0

Answer:

4.6 (Rounded)

Explanation:

Given: 77.5g of NH3

<u>77.5g of NH3</u>

         1

Plug in your units.

<u>77.5g of NH3</u>    x    <u>         mol of NH3  </u>

         1                                g of NH3

Since we are using grams, find the mass of NH3. To save you time, I'll tell you. It's 17.03052.

Now, plug is number into the equation with 1 on the top because you are trying to find 1 moles worth.

<u>77.5g of NH3</u>    x    <u>     1    mol of NH3  </u>

         1                     17.03052g of NH3

Now solve by multiplying the numbers across.

<u>    77.5x1    </u>    = <u>    77.5    </u>   = 4.55065377.

1x17.03052      17.03052

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Answer:

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Explanation:

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1.6\times 10^{-7} mol/L s=(6.4\times 10^{-9} L/mol s)[HI]^2

[A_o]=5 mol/L

Final concentration of HI after t = [A]

t = 4.53\times 10^{10} s

Integrated rate law for second order kinetics is given by:

\frac{1}{[A]}=kt+\frac{1}{[A_o]}

\frac{1}{[A]}=6.4\times 10^{-9} L/mol s\times 4.53\times 10^{10} s+\frac{1}{[5 mol/L]}

[A]=0.00345 mol/L

The concentration of HI after 4.53\times 10^{10} s is 0.00345 mol/L.

5 0
3 years ago
If you collect 1.75 L of hydrogen gas during a lab experiment when the room temperature is 23oC and the barometric pressure is 1
ziro4ka [17]

Answer:

n=0.0747mol

Explanation:

Hello,

In this case, since we can consider hydrogen gas as an ideal gas, we check the volume-pressure-temperature-mole relationship by using the ideal gas equation:

PV=nRT

Whereas we are asked to compute the moles given the temperature in Kelvins, thr pressure in atm and volume in L as shown below:

n=\frac{105kPa*\frac{0.009869atm}{1kPa}*1.75L}{0.082\frac{atm*L}{mol*K}*(23+273.15)K} \\\\n=0.0747mol

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2 years ago
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m_a_m_a [10]

Answer:

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3 years ago
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siniylev [52]

Answer:

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Explanation:

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Step 2: Divide all the numbers by the smallest one, i.e. 0.729

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The empirical formula of the compound is PCl₃.

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What is generally the best approach when liquid from a large reagent bottle is needed in an experiment
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Answer:

See the answer below

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The best approach would be to <u>pour the liquid from the large reagent bottle into a small-size beaker or reagent bottle first</u>, before measuring the required quantity out into the reaction vessel. This is necessary in order to maintain safety in the laboratory.

Pouring the liquid directly from the large reagent bottle into the measuring cylinder or directly into the reaction bottle can compromise safety in the laboratory. The liquid might splash out and cause harm to the handler or create other harmful circumstances in the laboratory.

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