In addition to white blood cell,_____ also help fight bacteria and disease.

Answers

Answer 1

Answer:

The white blood cells are the ones who leave the blood and enter tissues to fight off pathogens and invaders. They are not platelets because platelets help the healing of wounds and prevent it from bleeding by forming blood clots on the wounded area. They are not red blood cells because they carry oxygen all throughout the body organs. And they are not capillaries because capillaries are the ones that transports the oxygenated blood into the arteries.

Answer 2

Answer:

antibodies is your answer

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how many grams of silver chromate will precipitate when 150 ml of 0.500 M silver nitrate are added to 100 mL of 0.400 M potassium chromate

Answers

Final answer:

When 150 ml of 0.500 M silver nitrate are added to 100 mL of 0.400 M potassium chromate, a silver chromate precipitate forms. Considering the stoichiometry of the reaction and the quantities of reactants, 24.88 grams of silver chromate will precipitate.

Explanation:

The subject of this question is based on precipitation reactions in Chemistry. Precipitation reactions occur when two solutions combine to form an insoluble solid known as a precipitate. The moles of silver nitrate present in a 150 mL of 0.500 M solution can be calculated using the formula Molarity = Moles ÷ Volume (in Litres).

Thus, Moles of AgNO3 = 0.500 M * 0.15 L = 0.075 mol AgNO3. According to the reaction equation 2AgNO3 + K2CrO4 → 2AgCrO4(precipitate) + 2KNO3, for every mole of K2CrO4, we have two moles of AgNO3. Thus, based on stoichiometry and the given quantities of the reactants, the limiting reactant will be AgNO3, and it will totally react and form the silver chromate precipitate. The moles of Ag2CrO4 formed would therefore also be 0.075 mol. To convert this into grams, we use the molar mass of Ag2CrO4, which is approximately 331.73 g/mol. Hence, grams of Ag2CrO4 = 0.075 mol Ag2CrO4 * 331.73 g/mol = 24.88 g Ag2CrO4.

Learn more about Precipitation Reactions here:

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When a liquid is heated, the temperature stops rising at the liquid’s ____________________.

Answers

Turn into a gas/steam/gets cooler/or condenses - I say the most likely one is condenses

Consider the dissolution of 2.50 grams of salt XY in 75.0 mL of water within a calorimeter. The temperature of the water decreased by 0.93 oC. The heat capacity of the calorimeter is 42.2 J/oC. The density of the water (and the solution) is 1.00 g/mL. The specific heat capacity of the solution is 4.184 J/goC. Calculate the enthalpy change for dissolving this salt on a energy per mass basis (units of J/g).

Answers

The enthalpy change for dissolving this salt on a energy per mass is 136.32 J/g

How to determine the mass of the water

Density of water = 1 g/mL
Volume of water = 75 mL
Mass of water =?

Mass = Density × Volume

Mass of water = 1 × 75

Mass of water = 75 g

How to determine the heat absorbed by the solution

Mass of water = 75 g
Mass of salt = 2.50 g
Mass of solution (M) = 75 + 2.5 = 77.5 g
Temperature change (ΔT) = 0.93 °C
Specific heat capacity of the solution = 4.184 J/gºC
Heat of solution (Q) =?

Q = MCΔT

Q = 77.5 × 4.184 × 0.93

Q = 301.5618 J

How to determine the heat consumed by the calorimeter

Heat capacity of the calorimeter (C) = 42.2 J/ºC
Temperature change (ΔT) = 0.93 °C

Heat by calorimeter (H) =?

H = CΔT

H = 42.2 × 0.93

H = 39.246 J

How to determine the total heat released

Heat of solution (Q) = 301.5618 J
Heat by calorimeter (H) = 39.246 J

Total heat =?

Total heat = 301.5618 + 39.246

Total heat = 340.8078 J

How to determine the enthalpy change

Total heat = 340.8078 J
Mass of salt = 2.5 g

Enthalpy change (ΔH) =?

ΔH = Total heat / mass

ΔH = 340.8078 / 2.5

ΔH = 136.32 J/g

Learn more about heat transfer:

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Answer : The enthalpy change for dissolving this salt on a energy per mass basis is 132.4 J/g

Explanation :

Heat released by the reaction = Heat absorbed by the calorimeter + Heat absorbed by the water

$q=[q_1+q_2]$

$q=[c_1* \Delta T+m_2* c_2* \Delta T]$

where,

q = heat released by the reaction

$q_1$ = heat absorbed by the calorimeter

$q_2$ = heat absorbed by the water

$c_1$ = specific heat of calorimeter = $42.2J/^oC$

$c_2$ = specific heat of water = $4.184J/g^oC$

$m_2$ = mass of water = $Density* Volume=1/mL* 75.0mL=75.0g$

$\Delta T$ = change in temperature = $0.93^oC$

Now put all the given values in the above formula, we get:

$q=[(42.2J/^oC* 0.93^oC)+(75.0g* 4.184J/g^oC* 0.93^oC)]$

$q=331.08J$

Now we have to calculate the enthalpy change for dissolving this salt on a energy per mass basis.

$\Delta H=(q)/(m)$

where,

$\Delta H$ = enthalpy change = ?

q = heat released = 331.08 J

m = mass of salt = 2.50 g

$\Delta H=(331.08J)/(2.50g)=132.4J/g$

Therefore, the enthalpy change for dissolving this salt on a energy per mass basis is 132.4 J/g

Silicon dioxide and diamonds are best described as

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macromolecules !!!!!!!

How will the vapor pressure of an aqueous solution of sodium chloride compare to that of pure water?

Answers

The vapor pressure of a compound refers to the pressure generated by the vapour of a compound in equilibrium with its condensed stage. The major determinant of a compound vapour pressure is temperature. The vapour pressure of an aqueous solution of sodium chloride will be lower than that of pure water. This is because, dissolution of solute in a solvent always reduces the vapour pressure of the solution as a result of interactions between the molecule of the solute and the solvent. Thus, a pure compound will always have a higher vapour pressure than a solution.

The solutions vapor pressure would be lower.

18. Which of the following reactions are endothermic or exothermic? Explain your answers. A. When a certain amount of potassium nitrate is dissolved in water, the water temperature drops from 23°C to 18°C. B. Jack cooks himself a steak. C. When cold water is mixed with sulphuric acid, the mixture can rapidly reach the boiling point of water. D. A flare burns up slowly.

Answers

Answer:

The answer to your question is below

Explanation:

An endothermic reaction absorbs heat to proceed.

An exothermic reaction releases heat to proceed.

A. When a certain amount of potassium nitrate is dissolved in water, the water temperature drops from 23°C to 18°C. This is an example of an endothermic reaction because of the temperature diminishes.

B. Jack cooks himself a steak. This is an endothermic reaction because the steak does not cook itself it needs heat to be cooked.

C. When cold water is mixed with sulphuric acid, the mixture can rapidly reach the boiling point of water. This is an exothermic reaction because the temperature of water increases, which means that energy is been released.

D. A flare burns up slowly. I think it is an endothermic reaction because it was supply energy to proceed.

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