Will give BRAINLIEST A chemist reacted 11.50 grams of sodium metal with an excess amount of chlorine gas. The chemical reaction that occurred is shown.

Na + Cl2 → NaCl

If the percentage yield of the reaction is 85%, what is the actual yield? Show your work, including the use of stoichiometric calculations and conversion factors.

Explanation:

A chemical reaction is a process by which one or more substances, called reactants,

are transformed into another or other substances with different properties, calledproducts

In a general chemical reaction:

aA + bB > cC

ReactantsProdut

There are two types of yield in a chemical reaction:

The theoretical yield is the amount of product that, according to stoichiometric

calculations, is formed when all the limiting reactant reacts.

The actual yield is the amount of product actually obtained in a chemical reaction.

The equation used to determine the percent yield (% yield) is as follows:

% yield =(actual yield/theoretical yield)x100

Data:  

The chemical reaction carried out is as follows:

Na + Cl2  > NaCl

mass of Na = 11.50 g

excess chlorine gas

% yield = 85%

Unknown:

actual yield =?

To determine the actual yield, it is necessary:

-First, we determine the molar mass (MM) of the substances involved:

MMNa = 23.0 g/mol MMCl = 35.5 g/mol

MMCl2 = 2x35.5 g/mol = 71.0 g/mol

MMNaCl = (1x23.0 g/mol) + (1x35.5 g/mol) = 58.5 g/mol

-Second, we balance the chemical reaction:

2Na + Cl2 > 2NaCl

-Third, with the molar masses of the substances and the stoichiometry of the reaction, we obtain the relationship of teorca mass between substance:

.2Na + Cl2 > 2NaCl

2mole..1mol2mole

2x23.0.1x71.02x58.5

46.0g71.0g117 g

-Fourth, with the mass of Na and the ratio of theoretical mass between Na and NaCl, we can obtain the mass of NaCl produced (theoretical yield):

11.50 g of Nax(117 g of NaCl/46.0 g of Na) = 29.25 g of NaCl

-Finally, with the theoretical yield and the percentage of yield, we can obtain the actual yield from the following equation:

actual yield = (%yieldxtheoretical yield)/100

Substituting:

actual yield = (85x29.25g)/100

actual yield  = 24.86 g of NaCl

when 25.0 ml of 0.700 mol/l naoh was mixed in a calorimeter with 25.0 ml of 0.700 mol/l hcl, both initially at 20.0 °c, the temperature increased to 22.1 °c. the heat capacity of the calorimeter is 279 j/°c.

the equation for the reaction is:

naoh + hcl → nacl + h₂o

moles of hcl = 0.0250 l hcl ×

0.700

mol hcl

1 l hcl = 0.0175 mol hcl

volume of solution = (25.0 + 25.0) ml = 50.0 ml

mass of solution = 50.0 ml soln ×

1.00

ml soln

= 50.0 g soln

δt=t2-t1

= (22.1 – 20.0) °c = 2.1 °c

the heats involved are

heat from neutralization + heat to warm solution + heat to warm calorimeter = 0

q1+q2+q3=0

nδh+mcδt+cδt=0

0.0175 mol ×

δh

+ 50.0 g × 4.184 j·g⁻¹°c⁻¹ × 2.1 °c + 279 j°c⁻¹ × 2.1 °c = 0

0.0175 mol ×

δh

+ 439.32 j + 585.9 j = 0

0.0175 mol ×

δh

= -1025.22 j

δh=1025.22j0.0175 mol= -58 600 j/mol = -58.6 kj/mol

the answer is minerals.