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3 years ago

KMnO₄ solution

Chemistry

2 answers:

kicyunya [14]3 years ago

7 0

"B. purple" is the correct answer.

zaharov [31]3 years ago

7 0

KMnO4 solution is purple.
Bromine solution is orange.
Hope I helped!

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Does water have mass? Yes or no. Thanks everyone for your help

Mice21 [21]

Answer: The density of a material is defined as its mass per unit volume. In this example, each volume of water is different and therefore has a specific and unique mass. The mass of water is expressed in grams (g) or kilograms (kg), and the volume is measured in liters (L), cubic centimeters (cm3), or milliliters (mL).

Explanation: HOPE IT HELPS :)

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3 years ago

Calculate the percentage by mass of nitrogen in ptcl2(nh3)2.

Sav [38]

Molar Mass: 300.0510 g/mol

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3 years ago

A slice of pizza has 500 kcal. If we could burn the pizza and use all the heat to warm a 50-L container of cold water, what woul

gayaneshka [121]

Answer:

10°C

Explanation:

Heat gain by water = Heat lost by the slice of pizza

Thus,

$m_{water}\times C_{water}\times \Delta T=Q$

<u>For water: </u>

Volume = 50.0 L

Density of water= 1 kg/L

So, mass of the water:

$Mass\ of\ water=Density \times {Volume\ of\ water}$

$Mass\ of\ water=1 kg/L \times {50.0\ L}$

Mass of water = 50 kg

Specific heat of water = 1 kcal/kg°C

ΔT = ?

For slice of pizza:

Q = 500 kcal

So,

$50\times 1\times \Delta T=500$

ΔT = 10°C

Increase in temperature = 10°C

3 0

3 years ago

What is the velocity of a plane traveling west if it flies 1575 km in 2.75 hours

dalvyx [7]

Answer:

572.72kmh (after decimal is repeating)

Explanation:

1575/2.75

8 0

3 years ago

A tank contains an ideal gas mixture of 5 g of O2 and 8 g of CO2 at 160kPa and specified temperature. If O2 were separated from

erica [24]

Answer:

74 or 74 kPa.

Explanation:

Hello,

In this case, based on the initial information, it is seen that the oxygen and the carbon dioxide form the mixture at 160 kPa, thus, by isolating the oxygen, its pressure will be equal to its initial partial pressure because it gets isolated, hence, we compute its molar fraction as:

$x_{O_2}=\frac{5gO_2*\frac{1molO_2}{32gO_2} }{5gO_2*\frac{1molO_2}{32gO_2} +8gCO_2*\frac{1molCO_2}{44gCO_2} } =0.46$

Therefore, its initial pressure turns out:

$p_{O_2}=160kPa*0.46=73.9kPa$

Such pressure will be the oxygen's pressure once it is isolated. Finally, considering the request, the answer will be just 74 (by rounding to the nearest integer and without units).

Best regards.

8 0

3 years ago