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3 years ago

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A chemist determined by measurements that 0.070 moles of barium participated in a chemical reaction. Calculate the mass of bariu

m that participated in the chemical reaction.
Be sure your answer has the correct number of significant digits.

1 answer:

34kurt3 years ago

5 0

Answer: 9.59g
remember: mass = moles x Mr

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How is energy obtained from different sources stored, transported, and used?

Fed [463]

Answer:

Mode of transportation and source of energy

Energy sources are used in several major ways

Gasoline is used in cars, motorcycles, light trucks, and boats. Aviation gasoline is used in many types of airplanes. Distillate fuels are used mainly by trucks, buses, and trains and in boats and ships. Jet fuel is used in jet airplanes and some types of helicopters.

Explanation:

3 0

2 years ago

Charcoal from the dwelling level of the Lascaux Cave in France gives an average count of 0.97 disintegrations of ^14 C per minut

Verdich [7]

Answer:

Explanation:

count given by old sample = .97 disintegrations per minute per gram

count given by fresh sample = 6.68 disintegrations per minute per gram

Half life of radioactive carbon = 5568 years

rate of disintegration

dN / dt = λ N

In other words rate of disintegration is proportional to no of radioactive atoms present . As number reduces rate also reduces .

Let initial no of radioactive be N₀ and after time t , number reduces to N

N₀ / N = 6.68 / .97

Now

$N=N_0e^{-\lambda t}$

$\frac{N}{N_0} =e^{-\lambda t}$

$\frac{6.68}{.97} = e^{\lambda t}$

λ is disintegration constant

λ = .693 / half life

= .693 / 5568

= .00012446 year⁻¹

Putting the values in the equation above

$\frac{6.68}{.97} = e^{.00012446\times t}$

$6.8866 = e^{.00012446\times t}$

1.929577 = .00012446 t

t = 15503.6 years .

4 0

3 years ago

A 3.00 L flexible container holds a sample of hydrogen gas at 153 kPa.

Lisa [10]

The volume of the flexible container that holds a sample of hydrogen gas at 153 kPa is 1.51L (option B).

<h3>How to calculate volume?</h3>

The volume of a substance can be calculated using the following formula:

P1V1 = P2V2

Where;

P1 = initial pressure
P2 = final pressure
V1 = initial volume
V2 = final volume

153 × 3 = 304 × V2

459 = 304V2

V2 = 459/304

V2 = 1.51L

Therefore, the volume of the flexible container that holds a sample of hydrogen gas at 153 kPa is 1.51L.

Learn more about volume at: brainly.com/question/2098026

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8 0

2 years ago

Consider the equation for the formation of water. 2h2 o2 right arrow. 2h2o what is the theoretical yield of h2o if 130 g of h2o

Montano1993 [528]

The theoretical yield is the reaction yield that measures the product of the reaction from the conversion of the limiting reagent. The theoretical yield is 160 gm.

<h3>What is mass?</h3>

Mass or the theoretical yield is the result of the multiplication of mole and the molar mass of the compound.

The reaction between hydrogen and oxygen is shown as,

$\rm 2H_{2} + O_{2} \rightarrow 2H_{2}O$

Moles of water is calculated as:

$\begin{aligned}\rm moles &= \rm \dfrac{mass}{molar\; mass}\\\\&= \dfrac{18}{2}\\\\&= 9\;\rm moles\end{aligned}$

The theoretical yield of water is calculated as:

$\begin{aligned}\rm \text{weight of water} &= \rm moles \times molar \; mass\\\\&= 9 \times 18\\\\&= 162 \;\rm gm\end{aligned}$

Therefore, option D. 160 gm is the theoretical yield of water.

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5 0

2 years ago

Chloroform, formerly used as an anaesthetic and now believed to be a carcinogen, has a heat of vaporization ΔHvaporization = 31.

djverab [1.8K]

Answer:

Chloroform is expected to boil at 333 K (60 $^{0}\textrm{C}$ ).

Explanation:

For liquid-vapor equilibrium at 1 atm, $\Delta G^{0}$ = 0.

We know, $\Delta G^{0}=\Delta H^{0}-T\Delta S^{0}$ , where T is temperature in kelvin scale.

Here both $\Delta H^{0}$ and $\Delta S^{0}$ are corresponding to vaporization process therefore T represents boiling point of chloroform.

So, $0=(31.4\times 10^{3}\frac{J}{mol})-[T\times (94.2\frac{J}{mol.K})]$

or, T = 333 K

So, at 333 K (60 $^{0}\textrm{C}$ ) , chloroform is expected to boil.

6 0

3 years ago

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