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3 years ago

Help I really need to understand this please show how you do it !!

Chemistry

1 answer:

maks197457 [2]3 years ago

4 0

Answer:

HCl

Explanation:

A limiting reactant is the lowest amount of reactant so that the reaction will stop after all that reactant used.

To answer this question, you have to change all reactant units into moles. You have 52g HCl and its molecular mass is 36.46g/mole. The number of HCl in moles will be: 52g/ (36.46g/mole)= 1.43 moles.

In the balanced reaction formula, you can see that you need one mole of HCl and one mole of NaOH for each reaction. Both molecule's coefficient is 1.

If we used up all NaOH, then the number of HCl left will be:

(moles of NaOH used * NaOH coefficient) - (moles of HCl used * HCl coefficient)

(moles of HCl you have * HCl coefficient) - (moles of NaOH used * NaOH coefficient)

(1.43 moles *1 ) - (2.5 moles*1 ) = -1.07 mole

Since the result is minus, then it means we need more HCl and we can't use all NaOH.

If we used up all the HCl, then the number of NaOH left will be:

(moles of NaOH you have* NaOH coefficient) - (moles of HCl used * HCl coefficient)

(2.5 moles*1 )- (1.43 moles *1 )= 1.07 moles

Since the result is plus, then it means we can use all HCl. Then HCl is the limiting reactant

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What is the quantity of heat (in kJ) associated with cooling 185.5 g of water from 25.60°C to ice at -10.70°C?Heat Capacity of S

Cerrena [4.2K]

Taking into account the definition of calorimetry, sensible heat and latent heat, the amount of heat required is 37.88 kJ.

<h3>Calorimetry</h3>

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

<h3>Sensible heat</h3>

Sensible heat is defined as the amount of heat that a body absorbs or releases without any changes in its physical state (phase change).

<h3>Latent heat</h3>

Latent heat is defined as the energy required by a quantity of substance to change state.

When this change consists of changing from a solid to a liquid phase, it is called heat of fusion and when the change occurs from a liquid to a gaseous state, it is called heat of vaporization.

<u><em>25.60 °C to 0 °C</em></u>

First of all, you should know that the freezing point of water is 0°C. That is, at 0°C, water freezes and turns into ice.

So, you must lower the temperature from 25.60°C (in liquid state) to 0°C, in order to supply heat without changing state (sensible heat).

The amount of heat a body receives or transmits is determined by:

Q = c× m× ΔT

where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.

In this case, you know:

c= Heat Capacity of Liquid= 4.184 $\frac{J}{gC}$
m= 185.5 g
ΔT= Tfinal - Tinitial= 0 °C - 25.60 °C= - 25.6 °C

Replacing:

Q1= 4.184 $\frac{J}{gC}$ × 185.5 g× (- 25.6 °C)

Solving:

<u><em>Change of state</em></u>

The heat Q that is necessary to provide for a mass m of a certain substance to change phase is equal to

Q = m×L

where L is called the latent heat of the substance and depends on the type of phase change.

In this case, you know:

n= 185.5 grams× $\frac{1mol}{18 grams}$ = 10.30 moles, where 18 $\frac{g}{mol}$ is the molar mass of water, that is, the amount of mass that a substance contains in one mole.