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2 years ago

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A gas at 42. 0°c occupies a volume of 1. 32 l. if the volume increases to 2. 24 l, what is the new temperature in kelvin?

1 answer:

Nina [5.8K]2 years ago

8 0

the answer is 534.54 kelvin

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Atmospheric pressure at the summit of mount everest is about one third the pressure at sea level, which is 760 mm hg. if oxygen

vichka [17]

Atmospheric pressure at sea level is 760 mmHg.
We have been told that at the summit the pressure is only one third the pressure at sea level.
Then the pressure at the mountain top is $\frac{760}{3}$ mmHg
Air is made of a mixture of gases. the pressure that each gas exerts individually contributes to the total pressure of the system. The pressure that each gas exerts is the partial pressure of that gas which depends on the mole fraction of that gas or percentage composition of the individual gas.
Partial pressure of Oxygen - total pressure x percentage composition
Therefore pO₂ - $\frac{760 * 0.21}{3}$ = 53.2 mmHg
Answer is 53 mmHg

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3 years ago

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Wastewater from a cement factory contains 0.280 g of Ca2+ ion and 0.0220 g of Mg2+ ion per 100.0 L of solution. The solution den

faltersainse [42]

<u>Answer:</u> The concentration of $Ca^{2+}\text{ and }Mg^{2+}$ ions are 2.797 ppm and 0.212 ppm respectively.

<u>Explanation:</u>

To calculate the mass of solution, we use the equation:

$\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}$

Volume of gold = 100 L = 100000 mL (Conversion factor: 1 L = 1000 mL)

Density of gold = 1.001 g/mL

Putting values in above equation, we get:

$1.001g/mL=\frac{\text{Mass of solution}}{100000mL}\\\\\text{Mass of solution}=1.001\times 10^5g$

To calculate the concentration in ppm (by mass), we use the equation:

$ppm=\frac{\text{Mass of solute}}{\text{Mass of solution}}\times 10^6$

<u>Calculating the concentration of calcium ions:</u>

Mass of $Ca^{2+$ ions = 0.280 g

Putting values in above equation, we get:

$ppm(Ca^{2+})=\frac{0.280g}{1.001\times 10^5}\times 10^6=2.797ppm$

<u>Calculating the concentration of magnesium ions:</u>

Mass of $Mg^{2+$ ions = 0.0220 g

Putting values in above equation, we get:

$ppm(Mg^{2+})=\frac{0.0220g}{1.001\times 10^5}\times 10^6=0.212ppm$

Hence, the concentration of $Ca^{2+}\text{ and }Mg^{2+}$ ions are 2.797 ppm and 0.212 ppm respectively.

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3 years ago

Select the chemical equation below that is balanced

denis23 [38]

Answer:

cucl⁴
h2o4
5 hco4
kso4(nh4)

6 0

2 years ago

You have two containers. The first container contains 22.99 grams of solid

Vikki [24]

Answer:

The sodium has more moles.

n(Na)=2.09 mole

n(O)=0.999 mole

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3 years ago

An atom of magnesium and two atoms of chloride react and yield the compound of magnesium chloride which option represents the sc

svetoff [14.1K]

Answer:

$\boxed{\text{Mg + 2Cl $\longrightarrow$ MgCl$_{2}$}}$

Explanation:

Convert the word equation to a chemical equation.

one atom magnesium + two atoms Cl form magnesium chloride

Mg + 2Cl ⟶ MgCl₂

3 0

3 years ago

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